I. The reaction is second order with respect to both A and B.
|
|
- Candice Sutton
- 7 years ago
- Views:
Transcription
1 IB Chemistry HL Topic 6 Questions 1 The reaction between NO 2 and F 2 gives the following rate data at a certain temperature What is the order of reaction with respect to NO 2 and F 2? [NO 2 ]/mol dm 3 [F 2 ]/mol dm 3 Rate /mol dm 3 min NO 2 order F 2 order A first first B first second C second first D second second 2 Which step in a multi-step reaction is the rate determining step? A The first step B The last step C The step with the lowest activation energy D The step with the highest activation energy 3 The rate expression for a reaction is shown below rate = k[a] 2 [B] 2 Which statements are correct for this reaction? I The reaction is second order with respect to both A and B II The overall order of the reaction is 4 III Doubling the concentration of A would have the same effect on the rate of reaction as doubling the concentration of B A I and II only B I and III only C II and III only D I, II and III 4 Values of a rate constant, k, and absolute temperature, T, can be used to determine the activation energy of a reaction by a graphical method Which graph produces a straight line? A k versus T
2 B k versus C ln k versus T D ln k versus 5 The rate expression for a particular reaction is Rate = k[p][q] Which of the units below is a possible unit for k? A mol 2 dm 6 min 1 B mol 1 dm 3 min 1 C mol dm 3 min 1 D mol 2 dm 6 min 1 6 The reaction 2X(g) + Y(g) 3Z(g) has the rate expression rate = k [X] 2 [Y] 0 The concentration of X is increased by a factor of three and the concentration of Y is increased by a factor of two By what factor will the reaction rate increase? A 6 B 9 C 12 D 18 7 A reaction occurs in four steps The steps and their rates are shown in the table Step Rate mol dm 3 s mol dm 3 s mol dm 3 min mol dm 3 min 1 Which is the rate-determining step? A Step 1 B Step 2 C Step 3 D Step 4 8 The rate expression for a reaction is rate = k[ch 3 Br][OH ] Which is a possible unit for k? A mol 2 dm 6 min 1 B mol dm 3 min 1 C mol 1 dm 3 min 1 D mol 2 dm 6 min 1
3 9 What happens to the rate constant (k) and activation energy (E a ) of a reaction when the temperature is increased? A k increases and E a is unaffected B k decreases and E a is unaffected C E a increases and k is unaffected D E a decreases and k is unaffected 10 The mechanism of a reaction is XY 2 + XY 2 X 2 Y 4 X 2 Y 4 X 2 + 2Y 2 X 2 + Y 2 2XY What is the overall equation for the reaction? A X 2 Y 4 2XY 2 B 2XY 2 X 2 + 2Y 2 C 2XY 2 2XY + Y 2 D X 2 Y 4 2XY + Y 2 11 Consider the reaction 2I (aq) + H 2 O 2 (aq) + 2H + (aq) I 2 (aq) + 2H 2 O(l) In the presence of S 2 O 3 2 (aq) and starch solution, the time taken for a blue colour to form was observed at various reactant concentrations Experiment [I ] / mol dm 3 [H 2 O 2 ] / mol dm 3 [H + ] / mol dm 3 Time / s What is the correct order with respect to I and H 2 O 2? I H 2 O 2 A 1 2 B C 2 1 D Which statement is correct about the rate expression for a chemical reaction? A It can be determined from its chemical equation B It can be predicted from the value of ΔH Ө for the reaction C It can be calculated from the effect of temperature on the reaction D It can be determined by measuring the change in concentration of a reactant or product over time
4 13 For the reaction 2NO 2 (g) + F 2 (g) 2NO 2 F(g) the accepted mechanism is NO 2 (g) + F 2 (g) NO 2 F(g) + F(g) NO 2 (g) + F(g) NO 2 F(g) slow fast What is the rate expression for this reaction? A rate = k[no 2 ] 2 [F 2 ] B rate = k[no 2 ][F 2 ] C rate = k[no 2 ][F] D rate = k[no 2 ] 2 14 The activation energy, of a reaction can be obtained from the rate constant, k, and the absolute temperature, T Which graph of these quantities produces a straight line? A k against T B k against C ln k against T D ln k against 15 What is the order of reaction with respect to NO 2 (g) and F 2 (g) given the following rate data at a certain temperature? [NO 2 (g)] / mol dm 3 [F 2 (g)] / mol dm 3 Rate / mol dm 3 min Order with respect to NO 2 (g) Order with respect to F 2 (g) A first first B first second C second first D second second 16 Nitrogen(II) oxide reacts with hydrogen as shown by the following equation 2NO(g) + 2H 2 (g) N 2 (g) + 2H 2 O(g) The table below shows how the rate of reaction varies as the reactant concentrations vary Experiment Initial [NO] / mol dm 3 Initial [H 2 ] / mol dm 3 Initial rate / mol N 2 dm 3 s (a) Determine the order of reaction with respect to NO and with respect to H 2 Explain how you determined the order for NO
5 NO H 2 (3) (b) Write the rate expression for the reaction (c) Calculate the value for the rate constant, including its units (d) A suggested mechanism for this reaction is as follows H 2 + NO X fast step X + NO Y + H 2 O slow step Y + H 2 N 2 + H 2 O fast step State and explain whether this mechanism agrees with the experimental rate expression in (b) (4) (e) Explain why a single step mechanism is unlikely for a reaction of this kind
6 (f) Deduce how the initial rate of formation of H 2 O(g) compares with that of N 2 (g) in experiment 1 Explain your answer (Total 14 marks) 17 The oxidation of nitrogen monoxide takes place as follows: 2NO(g) + O 2 (g) 2NO 2 (g) The following experimental data was obtained at 1013 kpa and 298 K Experiment Initial [NO] / mol dm 3 Initial [O 2 ] / mol dm 3 Initial rate / mol dm 3 s (a) Deduce the order of reaction with respect to O 2 (b) Deduce the order of reaction with respect to NO (c) State the rate expression for the reaction (d) Calculate the value of the rate constant and state the units
7 (e) Suggest a possible mechanism that is consistent with the rate expression Indicate which of the steps is the rate-determining step (3) (Total 8 marks) 18 An equation for the decomposition of substance A is 2A 2B + C A graph showing the change in concentration of A against time as the reaction proceeds at a particular temperature is shown below (a) Define the term half-life of reaction (b) Use the graph to measure values of half-life of reaction, starting from time = zero time = 1000 s (c) Deduce the order of the reaction with respect to A, giving a reason for your choice, and write the rate expression for the reaction (3) (d) For a different reaction, between compounds D and E, the rate expression is rate = k[d] 2 [E] Calculate the value of k, including units, for the reaction when the concentrations of
8 both D and E are mol dm 3 and the reaction rate is mol dm 3 min 1 19 In a particular experiment, various concentrations of HI(aq) are reacted with a constant H 2 O 2 (aq) concentration according to the following equation: H 2 O 2 (aq) + 2HI(aq) I 2 (aq) + 2H 2 O(I) A graph of [HI] against time is as follows: (3) (Total 9 marks) (a) Use the graph to deduce the order of reaction with respect to HI Give a reason for your answer (b) The order with respect to H 2 O 2 is the same as HI Deduce the rate expression for this reaction (c) Determine the half-life of the reaction from the graph and calculate the value for the rate constant (Total 5 marks) 20 (a) The table below shows kinetic data for the following reaction C + D E + F Experiment [C] / mol dm 3 [D] / mol dm 3 Initial rate / mol dm 3 min
9 (i) Deduce the order of reaction with respect to both C and D, giving a reason in each case C D (4) (ii) Deduce the rate expression for this reaction (iii) Use data from Experiment 1 to calculate a value for the rate constant for this reaction and deduce its units (3) (b) Define the term half-life and calculate the half-life for a first-order reaction with a rate constant of min 1 (Total 10 marks) 21 Nitrogen(II) oxide reacts with hydrogen according to the following equation: 2NO(g) + 2H 2 (g) N 2 (g) + 2H 2 O(g) The table shows how the rate of reaction varies as the concentrations of the reactants are changed Experiment Initial [NO] / Initial [H 2 ] / Initial rate / mol dm 3 mol dm 3 mol (N 2 ) dm 3 s
10 (a) Determine the order of reaction with respect to H 2 and with respect to NO H 2 NO (b) Write the rate expression for the reaction (c) Calculate the value for the rate constant, and state its units using the data from experiment 1 (d) A suggested mechanism for this reaction is as follows H 2 + NO X X + NO Y + H 2 O Y + H 2 N 2 + H 2 O fast step slow step fast step State and explain whether this mechanism agrees with the experimental rate expression in (b)
11 (4) (e) Explain why a single step mechanism is unlikely for a reaction of this kind (f) Deduce and explain how the initial rate of formation of H 2 O compares with that of N 2 (Total 13 marks) 22 The data below refer to a reaction between X and Y Initial concentration / Initial rate of reaction / mol dm 3 mol dm 3 s 1 Experiment X Y (i) Define the term order of reaction (ii) Deduce the order of reaction with respect to both X and Y Explain your reasoning
12 (4) (iii) Write the rate expression for the reaction and calculate the rate constant, including its units (4) (iv) Calculate the initial rate of reaction when the initial concentrations of X and Y are 040 mol dm 3 and 060 mol dm 3 respectively (Total 11 marks) 23 Oxygen and nitrogen monoxide react together to form nitrogen dioxide O 2 (g) + 2NO(g) 2NO 2 (g) The graph below shows how the initial rate of reaction changed during an experiment in which the initial [NO(g)] was kept constant whilst the initial [O 2 (g)] was varied (a) Deduce, giving a reason, the order of reaction with respect to O 2 (b) In a series of experiments, the initial [O 2 (g)] was kept constant while the initial [NO(g)] was varied The results showed that the reaction was second order with respect to NO Sketch a graph to show how the rate of reaction would change if the initial [NO(g)] was increased
13 (c) Deduce the overall order of this reaction (d) State and explain what would happen to the initial rate of reaction if the initial concentration of NO was doubled and that of O 2 was halved (3) (e) When the initial values are [O 2 (g)] = mol dm 3 and [NO(g)] = mol dm 3, the initial rate of reaction is mol dm 3 s 1 Write the rate expression for this reaction and calculate the rate constant, stating its units (4) (Total 12 marks) 24 The compound iodine chloride, ICl, reacts with hydrogen to form iodine and hydrogen chloride (i) (ii) Deduce the equation for this reaction The kinetics of this reaction were studied at a certain temperature, when all the reactants and products were in the gas phase The table shows the initial rate of reaction for different concentrations of reactants Experiment [ICl] / mol dm 3 [H 2 ] / mol dm 3 Initial rate / mol dm 3 s (iii) (iv) Deduce and explain the order of reaction with respect to ICl and to H 2 Write the rate expression for the reaction Use information from Experiment 1 to determine the value, with units, of the rate constant for the reaction (4) (v) Determine the rate of reaction when the concentrations of reactants in Experiment 1 are both doubled
14 25 (a) The variation of the rate constant, k, for a reaction with temperature is shown by the Arrhenius equation Two versions of this equation are shown in Table 1 of the Data Booklet (Total 9 marks) (i) Explain the significance of the Arrhenius constant, A, in this equation (ii) Explain what is meant by the term activation energy,e a (iii) Describe how, using a graphical method, values of A and E a can be obtained for a reaction (5) (b) The equation for a reaction used in industry is CH 2 CH 2 + Cl 2 CH 2 ClCH 2 CL ΔH Ө = 185 kj Iron(III) chloride can be used as a catalyst for the reaction (i) Explain the difference between the terms homogeneous and heterogeneous when applied to a catalyst (ii) Draw an enthalpy level diagram for this reaction, including labels for ΔH Ө, E a and the activation energy when a catalyst is used, E cat (4) (Total 12 marks) 26 Nitrogen(II) oxide reacts with bromine according to the following equation 2NO(g) + Br 2 (g) 2NOBr(g) ΔH = negative The data below were obtained for the reaction between NO(g) and Br 2 (g) at a specified temperature and pressure Experiment Initial [NO] / mol dm 3 Initial [Br 2 ] / mol dm 3 Initial rate / mol dm 3 s (a) Determine, giving a reason, the order of reaction with respect to NO and the order of reaction with respect to Br 2
15 (b) Derive the rate expression for the reaction between NO and Br 2 (c) Calculate the rate constant for the rate expression using experiment 1 and state its units (d) If the total volume of the reaction mixture was doubled at constant temperature, state the effect, if any, on (i) the rate constant (ii) the rate of change of the Br 2 (g) concentration (e) Draw a labelled enthalpy level diagram for the reaction between NO(g) and Br 2 (g), with and without the use of a catalyst (3) (Total 10 marks)
16 27 (i) The reaction between propanone, CH 3 COCH 3 and bromine, Br 2 in the presence of acid, H +, is found to be second order overall, but the rate is independent of the bromine concentration Write three possible rate expressions for the reaction (3) (ii) The concentration of each of the three reactants was doubled in three separate experiments Choose one of the rate expressions in (i) and predict the effect on the rate of the reaction of each of these changes (iii) The graph below shows how the concentration of propanone changes with time in a reaction (iv) Use the graph to confirm that the reaction is first order with respect to propanone showing your working The overall reaction is: CH 3 COCH 3 (aq) + Br 2 (aq) CH 3 COCH 2 Br(aq) + HBr(aq) Describe one observation that would allow you to follow the progress of the reaction State and explain the role of the acid in the reaction (4) (Total 11 marks) IB Chemistry HL Topic 6 Answers 1 C
17 2 D 3 D 4 D 5 B 6 B 7 C 8 C 9 A 10 C 11 A 12 D 13 B 14 D 15 C 16 (a) (order with respect to) NO = 2; (order with respect to) H 2 = 1; rate increases 4 when [NO] doubles/owtte; 3 (b) rate = k[no] 2 [H 2 ]; 1 ECF from (a) (c) ( mol dm 3 s 1 = k (0100 mol dm 3 ) 2 (0100 mol dm 3 )) k = ; 1 mol 2 dm 6 s 1 ; 1 ECF from (b) (d) agrees/yes; slow step depends on X and NO; X depends on H 2 and NO; (so) NO is involved twice and H 2 once; Overall equation matches the stoichiometric equation; Award [1] each for any three of the four above OWTTE ECF for no, depending on answer for (b) Or agrees/yes; and = constant; rate of slow step = k [X][NO] = k [H 2 ][NO] 2 ; 4
18 ECF for no, depending on answer for (b) (e) (f) reaction involves four molecules; statistically/geometrically unlikely; 2 the rate of formation of H 2 O(g) = 2 rate for N 2 (g); because 2 moles H 2 O formed with 1 mole N 2 /OWTTE; 2 [14] 17 (a) first order (with respect to O 2 ); 1 (b) second order (with respect to NO); 1 (c) rate = k[no] 2 [O 2 ]; 1 Allow ECF from parts (a) and (b) (d) dm 6 mol 2 s 1 ; 2 Award [1] mark for the answer and [1] mark for units Allow ECF from part (c) (e) NO + NO N 2 O 2 ; N 2 O 2 + O 2 2NO 2 ; second step is rate determining step; Allow ECF from part (c) OR NO + O 2 NO 3 ; NO 3 + NO 2NO 2 ; second step is rate determining step; 3 Allow ECF from part (c) [8] 18 (a) time for reactant concentration to halve/owtte; 1 Accept time for mass to halve (b) 1000 s; 1000 s; 2 Accept s (c) first order; constant half-life; rate = k[a]; 3 Allow ECF for rate expression from stated order (d) = 152; Accept answer in range 152 to 153
19 mol 2 dm 6 min 1 ; 3 [9] 19 (a) first order; constant half-life; 2 (b) rate = k[hi][h 2 O 2 ]; 1 ECF from(a) (c) 47 sec; Accept answer in range 45 to 49 2 Accept answer in range ECF from half-life 20 (a) (i) (C) first order; doubling [C] doubles rate/owtte; [5] (D) zero order; changing [D] has no effect on rate/owtte; 4 (ii) rate = k[c]/rate = k[c] 1 [D] 0 ; 1 Apply ECF from (a)(i) (iii) k = = ; min 1 ; Apply ECF from (a)(ii) 3 (b) time for half of (amount/concentration of) reactant to react/disappear; t ( = ) = 21 min; 2 Units needed for second mark [10] 21 (a) (order with respect to) H 2 = 1; (order with respect to) NO = 2; 2 (b) rate = k[h 2 ][NO] 2 ; 1 ECF from (a) (c) ( mol dm 3 s 1 = k(0100 mol dm 3 )(0100 mol dm 3 ) 2 ) k = ; mol 2 dm 6 s 1 ; 2 ECF from (b) (d) agrees/yes; slow step depends on X and NO; (so) NO is involved twice and H 2 once; overall equation matches the stoichiometric equation/owtte;
20 ECF for no, depending on answer for (b) OR agrees/yes; and = constant; rate of slow step = k[x][no]; but X depends on H 2 and NO; rate of slow step = k[h 2 ][NO] 2 ; 4 max Award [1] each for any three of the four above ECF for no, depending on answer for (b) (e) reaction involves four molecules; statistically/geometrically unlikely; 2 (f) the rate of formation of H 2 O = 2 rate for N 2 ; because 2 moles H 2 O formed with 1 mole N 2 /OWTTE; 2 [13] (i) the power of a reactant s concentration in the rate equation/sum of powers of concentration/rate = k[x] n, where n = order of reaction; 1 Must be in terms of powers of concentration (ii) (iii) experiment 1 2 : [X] doubles and rate 4; 2nd order for X; experiment 2 3 : [Y] doubles and rate 2; 1st order for Y; 4 rate = k[x] 2 [Y](ECF from (ii)) for experiment 1, = k (025) 2 (025); k = 064; mol 2 dm 6 s 1 ; 4 Allow ECF from rate expression (iv) rate = 064[040] 2 [060]; = 0061; 2 Final answer to 2 sig figs only Allow ECF from (iii) [11] 23 (a) 1/first order; rate is (directly) proportional to concentration of oxygen/owtte; 2 (b) correct axes; correct shape curve; 2 (c) 3/third order; 1 Allow ECF from (a) and (b) (d) overall effect on rate = 4 /doubled/ 2;
21 [NO(g)] doubled, rate = 4/quadrupled; [O 2 (g)] halved, rate = 1/halved; 3 Allow ECF from (a) and (b) (e) rate = k[no(g)] 2 [O 2 (g)]; ; = 70; mol 2 dm 6 s 1 ; 4 Allow ECF State symbols not needed [12] 24 (i) 2ICl + H 2 I 2 + 2HCl; 1 (ii) ICl order 1; because doubling [ICl] doubles rate (when [H 2 ] constant); H 2 order 2; because halving [H 2 ] quarters rate (when [ICl] constant); or doubling [H 2 ] quadruples rate (when [ICl] constant); 4 (iii) rate = k [ICl][H 2 ] 2 ; 1 ECF from (ii) (iv) k = = 20; mol 2 dm 6 s 1 ; 2 ECF from (iii) (v) rate = = (mol dm 3 s 1 ); 1 ECF from (iii) 25 (a) (i) it relates to the geometric requirements of the reaction/orientation of reactants on collision/owtte; 1 [9] (ii) minimum energy needed for reactants to react (on collision)/owtte; 1 (iii) k measured at different values of temperature; graph plotted of ln k against 1/T; intercept on y-axis is ln A; A = e intercept ; measured slope of graph = E a /R; E a = R gradient; 5 Award [1] each for any five (b) (i) homogeneous catalyst is in same phase as reactants and heterogeneous catalyst is in different phase from reactants; 1 (ii) 4 OR
22 reactants line higher than product line (labels not needed); ΔH label; E a label; E cat label; [12] 26 (a) order of NO: second/2 - [NO] doubled, rate 4/OWTTE; order of Br 2 : first/1 - as [Br 2 ] doubled, rate of reaction doubled/owtte; 2 Reason needed for each mark (b) rate = k [NO] 2 [Br 2 ]; 1 Allow ECF from (a) (c) = k( ) k = ; dm 6 mol 2 s 1 ; 2 Allow ECF from (b) (d) (i) no effect/k changes only with temperature/owtte; 1 (ii) decrease (by a factor of 2); 1 (e) curve clearly showing E a without catalyst (E a ); curve clearly showing E a with catalyst (E a (cat)); labelling for x axis; 3 Accept time/progress of reaction/course of reaction/owtte Award [2 max] if an enthalpy level diagram for an endothermic reaction has been correctly drawn 27 (i) rate = k[ch 3 COCH 3 ][H + ]; [10]
23 rate = k[ch 3 COCH 3 ] 2 ; rate = k[h + ] 2 ; 3 (ii) [CH 3 COCH 3 ] doubles, rate doubles and [H + ] doubles, rate doubles; [Br 2 ] double, no effect on rate; OR [CH 3 COCH 3 ] doubles, rate quadruples; [Br 2 ] doubles/[h + ] doubles, no effect on rate; OR [H + ] doubles, rate quadruples; [Br 2 ] doubles/[ch 3 COCH 3 ] doubles, no effect on rate; 2 The answer given must correspond to the selected expression in (i) (iii) (iv) constant half-life; at least two sets of data to justify statement; 2 eg [ ] from 16 to 08 mol dm 3, 10s; 08 to 04, 10s; 04 to 02, 10s decrease in the colour of the bromine/owtte; catalyst; increases rate/speeds up reaction; by lowering E a /activation energy (by providing an alternate pathway); 4 [11]
Chapter 13 Chemical Kinetics
Chapter 13 Chemical Kinetics Student: 1. The units of "reaction rate" are A. L mol -1 s -1. B. L 2 mol -2 s -1. C. s -1. D. s -2. E. mol L -1 s -1. 2. For the reaction BrO 3 - + 5Br - + 6H + 3Br 2 + 3H
More information1A Rate of reaction. AS Chemistry introduced the qualitative aspects of rates of reaction. These include:
1A Rate of reaction AS Chemistry introduced the qualitative aspects of rates of reaction. These include: Collision theory Effect of temperature Effect of concentration Effect of pressure Activation energy
More informationMEMORANDUM GRADE 11. PHYSICAL SCIENCES: CHEMISTRY Paper 2
MEMORANDUM GRADE 11 PHYSICAL SCIENCES: CHEMISTRY Paper 2 MARKS: 150 TIME: 3 hours Learning Outcomes and Assessment Standards LO1 LO2 LO3 AS 11.1.1: Plan and conduct a scientific investigation to collect
More informationCHEMICAL EQUILIBRIUM (ICE METHOD)
CHEMICAL EQUILIBRIUM (ICE METHOD) Introduction Chemical equilibrium occurs when opposing reactions are proceeding at equal rates. The rate at which the products are formed from the reactants equals the
More informationIB Chemistry. DP Chemistry Review
DP Chemistry Review Topic 1: Quantitative chemistry 1.1 The mole concept and Avogadro s constant Assessment statement Apply the mole concept to substances. Determine the number of particles and the amount
More informationChemical Kinetics. 2. Using the kinetics of a given reaction a possible reaction mechanism
1. Kinetics is the study of the rates of reaction. Chemical Kinetics 2. Using the kinetics of a given reaction a possible reaction mechanism 3. What is a reaction mechanism? Why is it important? A reaction
More informationThe relationship between the concentration of a reactant and the rate of reaction with respect to that reactant can be shown using rate time graphs.
The effect of concentration on rate Student sheet To study The relationship between the concentration of a reactant and the rate of reaction with respect to that reactant can be shown using rate time graphs.
More informationSummer Holidays Questions
Summer Holidays Questions Chapter 1 1) Barium hydroxide reacts with hydrochloric acid. The initial concentration of the 1 st solution its 0.1M and the volume is 100ml. The initial concentration of the
More informationReaction Rates and Chemical Kinetics. Factors Affecting Reaction Rate [O 2. CHAPTER 13 Page 1
CHAPTER 13 Page 1 Reaction Rates and Chemical Kinetics Several factors affect the rate at which a reaction occurs. Some reactions are instantaneous while others are extremely slow. Whether a commercial
More informationEnthalpy of Reaction and Calorimetry worksheet
Enthalpy of Reaction and Calorimetry worksheet 1. Calcium carbonate decomposes at high temperature to form carbon dioxide and calcium oxide, calculate the enthalpy of reaction. CaCO 3 CO 2 + CaO 2. Carbon
More informationIII. Chemical Kinetics
WARNING NOTICE: The experiments described in these materials are potentially hazardous and require a high level of safety training, special facilities and equipment, and supervision by appropriate individuals.
More informationMr. Bracken. Multiple Choice Review: Thermochemistry
Mr. Bracken AP Chemistry Name Period Multiple Choice Review: Thermochemistry 1. If this has a negative value for a process, then the process occurs spontaneously. 2. This is a measure of how the disorder
More informationName Date Class STOICHIOMETRY. SECTION 12.1 THE ARITHMETIC OF EQUATIONS (pages 353 358)
Name Date Class 1 STOICHIOMETRY SECTION 1.1 THE ARITHMETIC OF EQUATIONS (pages 353 358) This section explains how to calculate the amount of reactants required or product formed in a nonchemical process.
More informationChemistry 12 Worksheet 1-1 - Measuring Reaction Rates
Chemistry 12 Worksheet 1-1 - Measuring Reaction Rates 1. A chemist wishes to determine the rate of reaction of zinc with hydrochloric acid. The equation for the reaction is: Zn (s) + 2HCl (aq) oh 2(g)
More informationINTI COLLEGE MALAYSIA A? LEVEL PROGRAMME CHM 111: CHEMISTRY MOCK EXAMINATION: DECEMBER 2000 SESSION. 37 74 20 40 60 80 m/e
CHM111(M)/Page 1 of 5 INTI COLLEGE MALAYSIA A? LEVEL PROGRAMME CHM 111: CHEMISTRY MOCK EXAMINATION: DECEMBER 2000 SESSION SECTION A Answer ALL EIGHT questions. (52 marks) 1. The following is the mass spectrum
More informationChemistry B11 Chapter 4 Chemical reactions
Chemistry B11 Chapter 4 Chemical reactions Chemical reactions are classified into five groups: A + B AB Synthesis reactions (Combination) H + O H O AB A + B Decomposition reactions (Analysis) NaCl Na +Cl
More informationDETERMINING THE ENTHALPY OF FORMATION OF CaCO 3
DETERMINING THE ENTHALPY OF FORMATION OF CaCO 3 Standard Enthalpy Change Standard Enthalpy Change for a reaction, symbolized as H 0 298, is defined as The enthalpy change when the molar quantities of reactants
More informationNet ionic equation: 2I (aq) + 2H (aq) + H O (aq) I (s) + 2H O(l)
Experiment 5 Goals To determine the differential rate law for the reaction between iodide and hydrogen peroxide in an acidic environment. To determine the activation energy and pre-exponential factor for
More information5. Which temperature is equal to +20 K? 1) 253ºC 2) 293ºC 3) 253 C 4) 293 C
1. The average kinetic energy of water molecules increases when 1) H 2 O(s) changes to H 2 O( ) at 0ºC 3) H 2 O( ) at 10ºC changes to H 2 O( ) at 20ºC 2) H 2 O( ) changes to H 2 O(s) at 0ºC 4) H 2 O( )
More informationChapter 12 - Chemical Kinetics
Chapter 1 - Chemical Kinetics 1.1 Reaction Rates A. Chemical kinetics 1. Study of the speed with which reactants are converted to products B. Reaction Rate 1. The change in concentration of a reactant
More informationChapter 14. Chemical Kinetics
14.1 Factors that Affect Reaction Rates Chemical kinetics = the study of how fast chemical reactions occur. Factors which affect rates of reactions: Physical state of the reactants. Concentration of the
More informationCHAPTER 13 Chemical Kinetics: Clearing the Air
CHAPTER 13 Chemical Kinetics: Clearing the Air 13.1. Collect and Organize For the plot of Figure P13.1, we are to identify which curves represent [N O] and [O ] over time for the conversion of N O to N
More information1. What is the molecular formula of a compound with the empirical formula PO and a gram-molecular mass of 284 grams?
Name: Tuesday, May 20, 2008 1. What is the molecular formula of a compound with the empirical formula PO and a gram-molecular mass of 284 grams? 2 5 1. P2O 5 3. P10O4 2. P5O 2 4. P4O10 2. Which substance
More informationPaper 1 (7405/1): Inorganic and Physical Chemistry Mark scheme
AQA Qualifications A-level Chemistry Paper (7405/): Inorganic and Physical Chemistry Mark scheme 7405 Specimen paper Version 0.5 MARK SCHEME A-level Chemistry Specimen paper 0. This question is marked
More informationChemical Kinetics. Reaction Rate: The change in the concentration of a reactant or a product with time (M/s). Reactant Products A B
Reaction Rates: Chemical Kinetics Reaction Rate: The change in the concentration of a reactant or a product with time (M/s). Reactant Products A B change in number of moles of B Average rate = change in
More informationQ1. A student studied the reaction between dilute hydrochloric acid and an excess of calcium carbonate.
Q. A student studied the reaction between dilute hydrochloric acid and an excess of calcium carbonate. calcium carbonate + hydrochloric acid calcium chloride + water + carbon dioxide The student measured
More informationCalculations with Chemical Formulas and Equations
Chapter 3 Calculations with Chemical Formulas and Equations Concept Check 3.1 You have 1.5 moles of tricycles. a. How many moles of seats do you have? b. How many moles of tires do you have? c. How could
More information1. The graph below represents the potential energy changes that occur in a chemical reaction. Which letter represents the activated complex?
1. The graph below represents the potential energy changes that occur in a chemical reaction. Which letter represents the activated complex? 4. According to the potential energy diagram shown above, the
More informationChapter 14: Chemical Kinetics: Reactions in the Air We Breathe
Chapter 4: Chemical Kinetics: Reactions in the Air We Breathe Problems: 4.-4.9, 4.-4., 4.4, 4.6-4.33, 4.37, 4.4 Consider the formation of rust (or oxidation of iron). a. It can occur over a period of several
More informationChapter 3. Chemical Reactions and Reaction Stoichiometry. Lecture Presentation. James F. Kirby Quinnipiac University Hamden, CT
Lecture Presentation Chapter 3 Chemical Reactions and Reaction James F. Kirby Quinnipiac University Hamden, CT The study of the mass relationships in chemistry Based on the Law of Conservation of Mass
More informationAP Chemistry 2010 Scoring Guidelines Form B
AP Chemistry 2010 Scoring Guidelines Form B The College Board The College Board is a not-for-profit membership association whose mission is to connect students to college success and opportunity. Founded
More informationCambridge International Examinations Cambridge International Advanced Subsidiary and Advanced Level
Cambridge International Examinations Cambridge International Advanced Subsidiary and Advanced Level *0123456789* CHEMISTRY 9701/02 Paper 2 AS Level Structured Questions For Examination from 2016 SPECIMEN
More informationSUPPLEMENTARY TOPIC 3 ENERGY AND CHEMICAL REACTIONS
SUPPLEMENTARY TOPIC 3 ENERGY AND CHEMICAL REACTIONS Rearranging atoms. In a chemical reaction, bonds between atoms in one or more molecules (reactants) break and new bonds are formed with other atoms to
More informationIntroductory Chemistry, 3 rd Edition Nivaldo Tro. Roy Kennedy Massachusetts Bay Community College Wellesley Hills, Maqqwertd ygoijpk[l
Introductory Chemistry, 3 rd Edition Nivaldo Tro Quantities in Car an octane and oxygen molecules and carbon dioxide and water Chemical Reactions Roy Kennedy Massachusetts Bay Community College Wellesley
More informationThermochemical equations allow stoichiometric calculations.
CHEM 1105 THERMOCHEMISTRY 1. Change in Enthalpy ( H) Heat is evolved or absorbed in all chemical reactions. Exothermic reaction: heat evolved - heat flows from reaction mixture to surroundings; products
More informationTest Review # 9. Chemistry R: Form TR9.13A
Chemistry R: Form TR9.13A TEST 9 REVIEW Name Date Period Test Review # 9 Collision theory. In order for a reaction to occur, particles of the reactant must collide. Not all collisions cause reactions.
More informationInstructions Answer all questions in the spaces provided. Do all rough work in this book. Cross through any work you do not want to be marked.
GCSE CHEMISTRY Higher Tier Chemistry 1H H Specimen 2018 Time allowed: 1 hour 45 minutes Materials For this paper you must have: a ruler a calculator the periodic table (enclosed). Instructions Answer all
More informationStandard Free Energies of Formation at 298 K. Average Bond Dissociation Energies at 298 K
1 Thermodynamics There always seems to be at least one free response question that involves thermodynamics. These types of question also show up in the multiple choice questions. G, S, and H. Know what
More informationChapter 3: Stoichiometry
Chapter 3: Stoichiometry Key Skills: Balance chemical equations Predict the products of simple combination, decomposition, and combustion reactions. Calculate formula weights Convert grams to moles and
More informationGRADE 12 PHYSICAL SCIENCE 3 HOURS TRIALS PAPER 2 (CHEMISTRY) 150 MARKS
Name: GRADE 12 PHYSICAL SCIENCE 3 HOURS TRIALS PAPER 2 (CHEMISTRY) 150 MARKS PLEASE READ THE FOLLOWING INSTRUCTIONS CAREFULLY 1. This paper consists of: a question paper of 7 pages a data and formula booklet
More informationIn the box below, draw the Lewis electron-dot structure for the compound formed from magnesium and oxygen. [Include any charges or partial charges.
Name: 1) Which molecule is nonpolar and has a symmetrical shape? A) NH3 B) H2O C) HCl D) CH4 7222-1 - Page 1 2) When ammonium chloride crystals are dissolved in water, the temperature of the water decreases.
More informationIB Chemistry 1 Mole. One atom of C-12 has a mass of 12 amu. One mole of C-12 has a mass of 12 g. Grams we can use more easily.
The Mole Atomic mass units and atoms are not convenient units to work with. The concept of the mole was invented. This was the number of atoms of carbon-12 that were needed to make 12 g of carbon. 1 mole
More informationChapter Test B. Chapter: Measurements and Calculations
Assessment Chapter Test B Chapter: Measurements and Calculations PART I In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question. 1.
More informationFinal. Mark Scheme. Chemistry CHEM5. (Specification 2420) Unit 5: Energetics, Redox and Inorganic Chemistry
Version.2 General Certificate of Education (A-level) January 202 Chemistry CHEM5 (Specification 2420) Unit 5: Energetics, Redox and Inorganic Chemistry Final Mark Scheme Mark schemes are prepared by the
More information20.2 Chemical Equations
All of the chemical changes you observed in the last Investigation were the result of chemical reactions. A chemical reaction involves a rearrangement of atoms in one or more reactants to form one or more
More informationWord Equations and Balancing Equations. Video Notes
Word Equations and Balancing Equations Video Notes In this lesson, you will: Use the law of conservation of mass and provide standard rules for writing and balancing equations. Write and balance equations
More informationChapter 1: Moles and equations. Learning outcomes. you should be able to:
Chapter 1: Moles and equations 1 Learning outcomes you should be able to: define and use the terms: relative atomic mass, isotopic mass and formula mass based on the 12 C scale perform calculations, including
More informationThermodynamics. Thermodynamics 1
Thermodynamics 1 Thermodynamics Some Important Topics First Law of Thermodynamics Internal Energy U ( or E) Enthalpy H Second Law of Thermodynamics Entropy S Third law of Thermodynamics Absolute Entropy
More information7. 1.00 atm = 760 torr = 760 mm Hg = 101.325 kpa = 14.70 psi. = 0.446 atm. = 0.993 atm. = 107 kpa 760 torr 1 atm 760 mm Hg = 790.
CHATER 3. The atmosphere is a homogeneous mixture (a solution) of gases.. Solids and liquids have essentially fixed volumes and are not able to be compressed easily. have volumes that depend on their conditions,
More informationChemistry: Chemical Equations
Chemistry: Chemical Equations Write a balanced chemical equation for each word equation. Include the phase of each substance in the equation. Classify the reaction as synthesis, decomposition, single replacement,
More informationChapter 3! Stoichiometry: Calculations with Chemical Formulas and Equations. Stoichiometry
Chapter 3! : Calculations with Chemical Formulas and Equations Anatomy of a Chemical Equation CH 4 (g) + 2O 2 (g) CO 2 (g) + 2 H 2 O (g) Anatomy of a Chemical Equation CH 4 (g) + 2 O 2 (g) CO 2 (g) + 2
More informationChemical Equations. Chemical Equations. Chemical reactions describe processes involving chemical change
Chemical Reactions Chemical Equations Chemical reactions describe processes involving chemical change The chemical change involves rearranging matter Converting one or more pure substances into new pure
More information87 16 70 20 58 24 44 32 35 40 29 48 (a) graph Y versus X (b) graph Y versus 1/X
HOMEWORK 5A Barometer; Boyle s Law 1. The pressure of the first two gases below is determined with a manometer that is filled with mercury (density = 13.6 g/ml). The pressure of the last two gases below
More informationProblem Solving. Stoichiometry of Gases
Skills Worksheet Problem Solving Stoichiometry of Gases Now that you have worked with relationships among moles, mass, and volumes of gases, you can easily put these to work in stoichiometry calculations.
More information2. The percent yield is the maximum amount of product that can be produced from the given amount of limiting reactant.
UNIT 6 stoichiometry practice test True/False Indicate whether the statement is true or false. moles F 1. The mole ratio is a comparison of how many grams of one substance are required to participate in
More informationWriting, Balancing and Predicting Products of Chemical Reactions.
Writing, Balancing and Predicting Products of Chemical Reactions. A chemical equation is a concise shorthand expression which represents the relative amount of reactants and products involved in a chemical
More informationThe first law: transformation of energy into heat and work. Chemical reactions can be used to provide heat and for doing work.
The first law: transformation of energy into heat and work Chemical reactions can be used to provide heat and for doing work. Compare fuel value of different compounds. What drives these reactions to proceed
More informationChapter 1 The Atomic Nature of Matter
Chapter 1 The Atomic Nature of Matter 6. Substances that cannot be decomposed into two or more simpler substances by chemical means are called a. pure substances. b. compounds. c. molecules. d. elements.
More informationHonors Chemistry: Unit 6 Test Stoichiometry PRACTICE TEST ANSWER KEY Page 1. A chemical equation. (C-4.4)
Honors Chemistry: Unit 6 Test Stoichiometry PRACTICE TEST ANSWER KEY Page 1 1. 2. 3. 4. 5. 6. Question What is a symbolic representation of a chemical reaction? What 3 things (values) is a mole of a chemical
More informationCambridge International Examinations Cambridge International General Certificate of Secondary Education
Cambridge International Examinations Cambridge International General Certificate of Secondary Education *0123456789* CHEMISTRY 0620/04 Paper 4 Theory (Extended) For Examination from 2016 SPECIMEN PAPER
More informationAP CHEMISTRY 2013 SCORING GUIDELINES
AP CHEMISTRY 2013 SCORING GUIDELINES Question 4 (15 points) For each of the following three reactions, write a balanced equation for the reaction in part (i) and answer the question about the reaction
More informationFormulae, stoichiometry and the mole concept
3 Formulae, stoichiometry and the mole concept Content 3.1 Symbols, Formulae and Chemical equations 3.2 Concept of Relative Mass 3.3 Mole Concept and Stoichiometry Learning Outcomes Candidates should be
More informationChem 1100 Chapter Three Study Guide Answers Outline I. Molar Mass and Moles A. Calculations of Molar Masses
Chem 1100 Chapter Three Study Guide Answers Outline I. Molar Mass and Moles A. Calculations of Molar Masses B. Calculations of moles C. Calculations of number of atoms from moles/molar masses 1. Avagadro
More informationSample Exercise 8.1 Magnitudes of Lattice Energies
Sample Exercise 8.1 Magnitudes of Lattice Energies Without consulting Table 8.2, arrange the following ionic compounds in order of increasing lattice energy: NaF, CsI, and CaO. Analyze: From the formulas
More informationCambridge International Examinations Cambridge International General Certificate of Secondary Education
Cambridge International Examinations Cambridge International General Certificate of Secondary Education *0123456789* CHEMISTRY 0620/03 Paper 3 Theory (Core) For Examination from 2016 SPECIMEN PAPER 1 hour
More informationFORM A is EXAM II, VERSION 1 (v1) Name
FORM A is EXAM II, VERSION 1 (v1) Name 1. DO NOT TURN THIS PAGE UNTIL DIRECTED TO DO SO. 2. These tests are machine graded; therefore, be sure to use a No. 1 or 2 pencil for marking the answer sheets.
More informationChapter 5, Calculations and the Chemical Equation
1. How many iron atoms are present in one mole of iron? Ans. 6.02 1023 atoms 2. How many grams of sulfur are found in 0.150 mol of sulfur? [Use atomic weight: S, 32.06 amu] Ans. 4.81 g 3. How many moles
More informationAP Chemistry 2009 Scoring Guidelines
AP Chemistry 2009 Scoring Guidelines The College Board The College Board is a not-for-profit membership association whose mission is to connect students to college success and opportunity. Founded in 1900,
More informationChemical Calculations: Formula Masses, Moles, and Chemical Equations
Chemical Calculations: Formula Masses, Moles, and Chemical Equations Atomic Mass & Formula Mass Recall from Chapter Three that the average mass of an atom of a given element can be found on the periodic
More informationSpring 2009. kj mol 125 0-229 -92. H f. H rxn = Σ H f (products) - Σ H f (reactants)
Spring 2009 2. The reaction of an elemental halogen with an alkane is a very common reaction. The reaction between chlorine and butane is provided below. (NOTE: Questions a d and f pertain to this reaction.)
More informationHow To Calculate Mass In Chemical Reactions
We have used the mole concept to calculate mass relationships in chemical formulas Molar mass of ethanol (C 2 H 5 OH)? Molar mass = 2 x 12.011 + 6 x 1.008 + 1 x15.999 = 46.069 g/mol Mass percentage of
More informationEquilibria Involving Acids & Bases
Week 9 Equilibria Involving Acids & Bases Acidic and basic solutions Self-ionisation of water Through reaction with itself: The concentration of water in aqueous solutions is virtually constant at about
More informationTransfer of heat energy often occurs during chemical reactions. A reaction
Chemistry 111 Lab: Thermochemistry Page I-3 THERMOCHEMISTRY Heats of Reaction The Enthalpy of Formation of Magnesium Oxide Transfer of heat energy often occurs during chemical reactions. A reaction may
More information= 1.038 atm. 760 mm Hg. = 0.989 atm. d. 767 torr = 767 mm Hg. = 1.01 atm
Chapter 13 Gases 1. Solids and liquids have essentially fixed volumes and are not able to be compressed easily. Gases have volumes that depend on their conditions, and can be compressed or expanded by
More informationChapter 6 Chemical Calculations
Chapter 6 Chemical Calculations 1 Submicroscopic Macroscopic 2 Chapter Outline 1. Formula Masses (Ch 6.1) 2. Percent Composition (supplemental material) 3. The Mole & Avogadro s Number (Ch 6.2) 4. Molar
More informationUnit 10A Stoichiometry Notes
Unit 10A Stoichiometry Notes Stoichiometry is a big word for a process that chemist s use to calculate amounts in reactions. It makes use of the coefficient ratio set up by balanced reaction equations
More informationChemical Equations and Chemical Reactions. Chapter 8.1
Chemical Equations and Chemical Reactions Chapter 8.1 Objectives List observations that suggest that a chemical reaction has taken place List the requirements for a correctly written chemical equation.
More informationSample Problem: STOICHIOMETRY and percent yield calculations. How much H 2 O will be formed if 454 g of. decomposes? NH 4 NO 3 N 2 O + 2 H 2 O
STOICHIOMETRY and percent yield calculations 1 Steps for solving Stoichiometric Problems 2 Step 1 Write the balanced equation for the reaction. Step 2 Identify your known and unknown quantities. Step 3
More informationMOLES AND MOLE CALCULATIONS
35 MOLES ND MOLE CLCULTIONS INTRODUCTION The purpose of this section is to present some methods for calculating both how much of each reactant is used in a chemical reaction, and how much of each product
More informationTHE MOLE / COUNTING IN CHEMISTRY
1 THE MOLE / COUNTING IN CHEMISTRY ***A mole is 6.0 x 10 items.*** 1 mole = 6.0 x 10 items 1 mole = 60, 00, 000, 000, 000, 000, 000, 000 items Analogy #1 1 dozen = 1 items 18 eggs = 1.5 dz. - to convert
More information@ Oxford Fajar Sdn. Bhd. (008974-T) 2012. Matter. 1.1 Atoms and Molecules 1.2 Mole Concept 1.3 Stoichiometry
1 Matter 1.1 Atoms and Molecules 1.2 Mole Concept 1.3 Stoichiometry 2 Chemistry for Matriculation Semester 1 1.1 Atoms and Molecules LEARNING OUTCOMES Describe proton, electron and neutron in terms of
More informationCalculating Atoms, Ions, or Molecules Using Moles
TEKS REVIEW 8B Calculating Atoms, Ions, or Molecules Using Moles TEKS 8B READINESS Use the mole concept to calculate the number of atoms, ions, or molecules in a sample TEKS_TXT of material. Vocabulary
More informationStudying an Organic Reaction. How do we know if a reaction can occur? And if a reaction can occur what do we know about the reaction?
Studying an Organic Reaction How do we know if a reaction can occur? And if a reaction can occur what do we know about the reaction? Information we want to know: How much heat is generated? How fast is
More informationThe Kinetics of Enzyme Reactions
The Kinetics of Enzyme Reactions This activity will introduce you to the chemical kinetics of enzyme-mediated biochemical reactions using an interactive Excel spreadsheet or Excelet. A summarized chemical
More information1 Exercise 2.19a pg 86
In this solution set, an underline is used to show the last significant digit of numbers. For instance in x = 2.51693 the 2,5,1, and 6 are all significant. Digits to the right of the underlined digit,
More informationChemistry Assessment Unit AS 1
Centre Number 71 Candidate Number ADVANCED SUBSIDIARY (AS) General Certificate of Education January 2011 Chemistry Assessment Unit AS 1 assessing Basic Concepts in Physical and Inorganic Chemistry [AC111]
More information602X10 21 602,000,000,000, 000,000,000,000 6.02X10 23. Pre- AP Chemistry Chemical Quan44es: The Mole. Diatomic Elements
Pre- AP Chemistry Chemical Quan44es: The Mole Mole SI unit of measurement that measures the amount of substance. A substance exists as representa9ve par9cles. Representa9ve par9cles can be atoms, molecules,
More informationChapter 4: Chemical and Solution Stoichiometry
Chapter 4: Chemical and Solution Stoichiometry (Sections 4.1-4.4) 1 Reaction Stoichiometry The coefficients in a balanced chemical equation specify the relative amounts in moles of each of the substances
More informationMath 231:Introduction to Ordinary Differential Equations Mini-Project: Modeling Chemical Reaction Mechanisms
Department of Mathematics Fall 2012 The University of Tennessee H. Finotti Math 231:Introduction to Ordinary Differential Equations Mini-Project: Modeling Chemical Reaction Mechanisms Chemical kinetics,
More informationReading: Moore chapter 18, sections 18.6-18.11 Questions for Review and Thought: 62, 69, 71, 73, 78, 83, 99, 102.
Thermodynamics 2: Gibbs Free Energy and Equilibrium Reading: Moore chapter 18, sections 18.6-18.11 Questions for Review and Thought: 62, 69, 71, 73, 78, 83, 99, 102. Key Concepts and skills: definitions
More informationAP Chemistry 2008 Free-Response Questions
AP Chemistry 008 Free-Response Questions The College Board: Connecting Students to College Success The College Board is a not-for-profit membership association whose mission is to connect students to college
More informationStoichiometry. What is the atomic mass for carbon? For zinc?
Stoichiometry Atomic Mass (atomic weight) Atoms are so small, it is difficult to discuss how much they weigh in grams We use atomic mass units an atomic mass unit (AMU) is one twelfth the mass of the catbon-12
More informationChemistry 122 Mines, Spring 2014
Chemistry 122 Mines, Spring 2014 Answer Key, Problem Set 9 1. 18.44(c) (Also indicate the sign on each electrode, and show the flow of ions in the salt bridge.); 2. 18.46 (do this for all cells in 18.44
More informationIMPORTANT INFORMATION: S for liquid water is 4.184 J/g degree C
FORM A is EXAM II, VERSION 2 (v2) Name 1. DO NOT TURN THIS PAGE UNTIL DIRECTED TO DO SO. 2. These tests are machine graded; therefore, be sure to use a No. 1 or 2 pencil for marking the answer sheets.
More informationMoles. Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities Equations
Moles Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities Equations Micro World atoms & molecules Macro World grams Atomic mass is the mass of an
More informationChemical Calculations: The Mole Concept and Chemical Formulas. AW Atomic weight (mass of the atom of an element) was determined by relative weights.
1 Introduction to Chemistry Atomic Weights (Definitions) Chemical Calculations: The Mole Concept and Chemical Formulas AW Atomic weight (mass of the atom of an element) was determined by relative weights.
More informationChapter 8: Chemical Equations and Reactions
Chapter 8: Chemical Equations and Reactions I. Describing Chemical Reactions A. A chemical reaction is the process by which one or more substances are changed into one or more different substances. A chemical
More informationThermochemistry. r2 d:\files\courses\1110-20\99heat&thermorans.doc. Ron Robertson
Thermochemistry r2 d:\files\courses\1110-20\99heat&thermorans.doc Ron Robertson I. What is Energy? A. Energy is a property of matter that allows work to be done B. Potential and Kinetic Potential energy
More informationAP Chemistry 2005 Scoring Guidelines Form B
AP Chemistry 2005 Scoring Guidelines Form B The College Board: Connecting Students to College Success The College Board is a not-for-profit membership association whose mission is to connect students to
More informationCHEMICAL REACTIONS AND REACTING MASSES AND VOLUMES
CHEMICAL REACTIONS AND REACTING MASSES AND VOLUMES The meaning of stoichiometric coefficients: 2 H 2 (g) + O 2 (g) 2 H 2 O(l) number of reacting particles 2 molecules of hydrogen react with 1 molecule
More information