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1 Practice Test Questions: There are a lot of questions. Please feel free to do a problem, skip around and make sure you are doing all types of problems heat exchange, Hess Law problems, specific heat problems, calorimetry problems, and standard enthalpy of formation/reaction questions. 9) Which one of the following is an endothermic process? A) ice melting B) water freezing C) boiling soup D) Hydrochloric acid and barium hydroxide are mixed at 25 C: the temperature increases. E) Both A and C Page Ref: Sec ) Which one of the following is an exothermic process? A) ice melting B) water evaporating C) boiling soup D) condensation of water vapor E) Ammonium thiocyanate and barium hydroxide are mixed at 25 C: the temperature drops. Page Ref: Sec ) Of the following, which one is a state function? A) H B) q C) w D) heat E) none of the above Page Ref: Sec ) Which of the following is a statement of the first law of thermodynamics? A) E k = (1/2) mv 2 B) A negative ΔH corresponds to an exothermic process. C) ΔE = E final - E initial D) Energy lost by the system must be gained by the surroundings. E) 1 cal = J (exactly) Page Ref: Sec ) For a given process at constant pressure, ΔH is negative. This means that the process is 1

2 . A) endothermic B) equithermic C) exothermic D) a state function E) energy Page Ref: Sec ) Which one of the following statements is true? A) Enthalpy is an intensive property. B) The enthalpy change for a reaction is independent of the state of the reactants and products. C) Enthalpy is a state function. D) H is the value of q measured under conditions of constant volume. E) The enthalpy change of a reaction is the reciprocal of the ΔH of the reverse reaction. Page Ref: Sec ) Under what condition(s) is the enthalpy change of a process equal to the amount of heat transferred into or out of the system? A) a only B) b only C) c only D) a and b E) b and c (a) temperature is constant (b) pressure is constant (c) volume is constant Page Ref: Sec ) A sample of calcium carbonate [CaCO3 (s)] absorbs 45.5 J of heat, upon which the temperature of the sample increases from 21.1 C to 28.5 C. If the specific heat of calcium carbonate is 0.82 J/g-K, what is the mass (in grams) of the sample? A) 3.7 B) 5.0 C) 7.5 D) 410 E) 5.0 x ) The temperature of a g sample of calcium carbonate [CaCO3 (s)] increases from 23.6 C to 38.2 C. If the specific heat of calcium carbonate is 0.82 J/g-K, how many joules of heat are absorbed? A) 0.82 B) 5.0 C) 7.5 D) 410 E) 151 2

3 29) An 8.29 g sample of calcium carbonate [CaCO3 (s)] absorbs 50.3 J of heat, upon which the temperature of the sample increases from 21.1 C to 28.5 C. What is the specific heat of calcium carbonate? A).63 B).82 C) 1.1 D) 2.2 E) ) A sample of iron absorbs 67.5 J of heat, upon which the temperature of the sample increases from 21.5 C to 28.5 C. If the specific heat of iron is J/g-K, what is the mass (in grams) of the sample? A) 4.3 B) 11 C) 21 D) 1100 E) 1.1 x ) The temperature of a 35.2 g sample of iron increases from 23.7 C to 29.5 C. If the specific heat of iron is J/g-K, how many joules of heat are absorbed? A) 4.3 B) 92 C) D) 1100 E) 1.1 x ) Which of the following is a statement of Hess's law? A) If a reaction is carried out in a series of steps, the ΔH for the reaction will equal the sum of the enthalpy changes for the individual steps. B) If a reaction is carried out in a series of steps, the ΔH for the reaction will equal the product of the enthalpy changes for the individual steps. C) The ΔH for a process in the forward direction is equal in magnitude and opposite in sign to the ΔH for the process in the reverse direction. D) The ΔH for a process in the forward direction is equal to the ΔH for the process in the reverse direction. E) The ΔH of a reaction depends on the physical states of the reactants and products. Page Ref: Sec

4 34) For which one of the following reactions is ΔH rxn equal to the heat of formation of the product? A) N 2 (g) + 3H 2 (g) 2NH 3 (g) B) (1/2) N 2 (g) + O 2 (g) NO 2 (g) C) 6C (s) + 6H (g) C 6 H 6 (l) D) P (g) + 4H (g) + Br (g) PH 4 Br (l) E) 12C (g) + 11H 2 (g) + 11O (g) C 6 H 22 O 11 (g) 35) Of the following, ΔH f is not zero for. A) O 2 (g) B) C (graphite) C) N 2 (g) D) F 2 (s) E) Cl 2 (g) 36) Of the following, ΔH f is not zero for. A) Sc (g) B) Si (s) C) P4 (s, white) D) Br 2 (l) E) Ca (s) 40) For which one of the following equations is ΔH rxn equal to ΔH f for the product? A) Xe (g) + 2 F 2 (g) XeF 4 (g) B) CH 4 (g) + 2 Cl 2 (g) CH 2 Cl 2 (l) + 2HCl (g) C) N 2 (g) + O 3 (g) N 2 O 3 (g) D) 2CO (g) + O 2 (g) 2CO 2 (g) E) C (diamond) + O 2 (g) CO 2 (g) 45) With reference to enthalpy changes, the term standard conditions means. (a) P = 1 atm (b) some common temperature, usually 298 K (c) V = 1 L A) a only B) b only C) c only D) a and c E) a and b 4

5 5.2 Bimodal Questions 1) Calculate the kinetic energy in J of an electron moving at m/s. The mass of an electron is g. A) B) C) D) E) Answer: C Diff: 2 Page Ref: Sec ) Calculate the kinetic energy in joules of an automobile weighing 2135 lb and traveling at 55 mph. A) B) C) D) E) Answer: B Diff: 3 Page Ref: Sec ) Calculate the kinetic energy in joules of an automobile weighing 4345 lb and traveling at 75 mph. A) 5.5 x 105 B) C) D) E) Answer: C Diff: 3 Page Ref: Sec ) The kinetic energy of a 7.3 kg steel ball traveling at 18.0 m/s is J. A) B) 66 C) D) E) 7.3 Answer: A Diff: 2 Page Ref: Sec

6 15) The value of ΔH for the reaction below is -72 kj. kj of heat are released when 80.9 grams of HBr is formed in this reaction. H 2 (g) + Br 2 (g) 2HBr (g) A) 144 B) 72 C) 0.44 D) 36 E) -72 Page Ref: Sec ) The value of ΔH for the reaction below is -126 kj. kj are released when 2.00 mol of NaOH is formed in the reaction? 2 Na 2 O 2 (s) + 2 H 2 O (l) 4NaOH (s) + O 2 (g) A) 252 B) 63 C) 3.9 D) 7.8 E) -126 Page Ref: Sec ) The enthalpy change for the following reaction is kj: 2 H 2 (g) + O 2 (g) 2 H 2 O (g) Therefore, the enthalpy change for the following reaction is kj: 4 H 2 (g) + 2 O 2 (g) 4 H 2 O (g) A) B) C) D) E) Page Ref: Sec

7 35) ΔH for the reaction IF 5 (g) IF 3 (g) + F 2 (g) is kj, give the data below. IF (g) + F 2 (g) IF 3 (g) ΔH = -390 kj IF (g) + 2 F 2 (g) IF 5 (g) ΔH = -745 kj A) +355 B) C) D) +35 E) -35 Page Ref: Sec ) Given the following reactions Fe 2 O 3 (s) + 3CO (s) 2Fe (s) + 3CO 2 (g) 3Fe (s) + 4CO 2 (s) 4CO (g) + Fe 3 O 4 (s) ΔH = kj ΔH = kj the enthalpy of the reaction of Fe 2 O 3 with CO 3 Fe 2 O 3 (s) + CO (g) CO 2 (g) + 2 Fe 3 O 4 (s) A) B) 40.5 C) D) -109 E) +109 Page Ref: Sec ) Given the following reactions N 2 (g) + 2 O 2 (g) 2NO 2 (g) ΔH = 66.4 kj 2NO (g) + O 2 (g) 2NO 2 (g) ΔH = kj the enthalpy of the reaction of the nitrogen to produce nitric oxide N 2 (g) + O 2 (g) 2NO (g) A) B) C) 47.8 D) 90.3 E) Page Ref: Sec

8 40) Given the following reactions CaCO 3 (s) CaO (s) + CO 2 (g) ΔH = kj C (s, graphite) + O 2 (g) CO 2 (g) ΔH = kj the enthalpy of the reaction CaCO 3 (s) CaO (s) + C (s, graphite) + O 2 (g) A) B) C) D) E) Page Ref: Sec ) The value of ΔH for the reaction below is -186 kj. H 2 (g) + Cl 2 (g) 2HCl (g) The value of ΔH f for HCl (g) is kj/mol. A) B) C) D) -186 E) ) Given the data in the table below, ΔH rxn for the reaction Ca(OH) H 3 AsO 4 Ca(H 2 AsO 4 ) H 2 O A) B) C) D) E)

9 48) Given the data in the table below, ΔH rxn for the reaction 4NH 3 (g) + 5 O 2 (g) 4NO (g) + 6 H 2 O (l) A) B) -150 C) D) E) The ΔH f of O 2 (g) is needed for the calculation. Answer: A Diff: 3 49) Given the data in the table below, ΔH rxn for the reaction C 2 H 5 OH (l) + O 2 (g) CH 3 CO 2 H (l) + H 2 O (l) A) B) C) D) E) The value of ΔH f of O 2 (g) is required for the calculation. Answer: D Diff: 3 9

10 50) Given the data in the table below, ΔH rxn for the reaction 3NO 2 (g) + H 2 O (l) 2HNO 3 (aq) + NO (g) A) 64 B) 140 C) -140 D) -508 E) ) Given the data in the table below, ΔH rxn for the reaction 2 Ag 2 S (s) + O 2 (g) 2 Ag 2 O (s) + 2S (s) A) -1.6 B) +1.6 C) -3.2 D) +3.2 E) The ΔH f of S (s) and of O2 (g) are needed for the calculation. 10

11 55) Given the data in the table below, ΔH rxn for the reaction Ag 2 O (s) + H 2 S (g) Ag 2 S (s) + H 2 O (l) A) -267 B) -370 C) -202 D) -308 E) More data are needed to complete the calculation. 56) Given the data in the table below, ΔH rxn for the reaction 2SO 2 (g) + O 2 (g) 2SO 3 (g) A) -99 B) 99 C) -198 D) 198 E) The ΔH f of O2 (g) is needed for the calculation. 11

12 10) The combustion of titanium with oxygen produces titanium dioxide: Ti (s) + O 2 (g) TiO 2 (s) When g of titanium is combusted in a bomb calorimeter, the temperature of the calorimeter increases from C to C. In a separate experiment, the heat capacity of the calorimeter is measured to be 9.84 kj/k. The heat of reaction for the combustion of a mole of Ti in this calorimeter is kj/mol. A) 14.3 B) 19.6 C) -311 D) E) ) The specific heat capacity of solid copper metal is J/g-K. How many joules of heat are needed to raise the temperature of a 1.55-kg block of copper from 33.0 C to 77.5 C? A) B) 26.6 C) D) E) ) A 50.0-g sample of liquid water at 25.0 C is mixed with 29.0 g of water at 45.0 C. The final temperature of the water is C. A) 102 B) 27.6 C) 35.0 D) 142 E) ) What is the enthalpy change (in kj) of a chemical reaction that raises the temperature of ml of solution having a density of 1.25 g/ml by 7.80 C? (The specific heat of the solution is 3.74 joules/gram-k.) A) B) C) 8.20 D) E)

13 5.4 Short Answer Questions 2) Given the equation H2O (l) H2O (g) ΔHrxn = 40.7 kj at 100 C Calculate the mass of liquid water (in grams) at 100. C that can converted to vapor by absorbing J of heat. Answer: grams Diff: 3 3) Given the equation H2O (l) H2O (g) ΔHrxn = 40.7 kj at 100 C Calculate the heat required to convert 3.00 grams of liquid water at 100. C to vapor. 4) When grams of NaOH is dissolved in grams of water, the temperature of the solution increases from C to C. The amount of heat absorbed by the water is? (The specific heat of water is 4.18 J/g- C.) 13

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