AP Chemistry ( MCSEMENICK2015 ) My Courses Course Settings Chemistry: The Central Science, 12e Brown/LeMay/Bursten/Murphy/Woodward
|
|
- Basil Stevens
- 7 years ago
- Views:
Transcription
1 Signed in as Daniel Semenick, Instructor Help Sign Out AP Chemistry ( MCSEMENICK2015 ) My Courses Course Settings Chemistry: The Central Science, 12e Brown/LeMay/Bursten/Murphy/Woodward Instructor Resources etext Study Area Course Home Assignments Roster Gradebook Item Library Chapter 10 Quiz [ Edit ] Overview Summary View Diagnostics View Print View with Answers Chapter 10 Quiz Due: 9:58pm on Thursday, October 30, 2014 You will receive no credit for items you complete after the assignment is due. Grading Policy Go Figure 10.2 Description: A mercury barometer. (a) What happens to h the height of the mercury column, if the atmospheric pressure increases? A mercury barometer. 1 of 16 10/28/14 8:44 PM
2 What happens to h the height of the mercury column, if the atmospheric pressure increases? the height of the mercury column remains the same the height of the mercury column increases the height of the mercury column decreases Chapter 10 Question 17 - Multiple Choice Description: (a) Which one of the following is a valid statement of Avogadro's law? Which one of the following is a valid statement of Avogadro's law? V = constant n PV = constant P = constant T V = constant P V T = constant Problem Description: You have a gas confined to a cylinder with a movable piston. What would happen to the gas pressure inside the cylinder if you do the following? (a) Decrease the volume to one-fourth the original volume while holding the temperature constant. (b)... You have a gas confined to a cylinder with a movable piston. What would happen to the gas pressure inside the 2 of 16 10/28/14 8:44 PM
3 cylinder if you do the following? Decrease the volume to one-fourth the original volume while holding the temperature constant. = 4 = 2 = 4 = 2 = Part B Reduce the temperature (in kelvins) to half its original value while holding the volume constant. = 4 = = = 2 = 2 4 Part C Reduce the amount of gas to one-fourth while keeping the volume and temperature constant. = 4 = 2 = = = of 16 10/28/14 8:44 PM
4 Problem Description: Nitrogen and hydrogen gases react to form ammonia gas as follows: N_2 (g) + 3H_2 (g) rightarrow 2(NH)_3 (g) At a certain temperature and pressure, V_1 of N_2 reacts with V_2 of H_2. (a) If all the N_2 and H_2 are consumed, what volume of... Nitrogen and hydrogen gases react to form ammonia gas as follows: N 2 (g) + 3 H 2 (g) 2 NH 3 (g) At a certain temperature and pressure, 1.1 L of N 2 reacts with 3.3 L of H 2. If all the N 2 and H 2 are consumed, what volume of NH 3, at the same temperature and pressure, will be produced? Express your answer using two significant figures. V = = 2.2 L Chapter 10 Question 10 - Bimodal Description: (a) A sample of a gas originally at 25 C and 1.00 atm pressure in a 2.5 L container is subject to a pressure of 0.85 atm and a temperature of 15 C. The final volume of the gas is L. A sample of a gas originally at 25 C and 1.00 atm pressure in a 2.5 L container is subject to a pressure of 0.85 atm and a temperature of 15 C. The final volume of the gas is L ± Changes in Volume Description: ± Includes Math Remediation. Calculate pressure given the change in volume at constant temperature and molar amount. Calculate temperature given the change in volume at constant pressure and 4 of 16 10/28/14 8:44 PM
5 molar amount. Calculate new molar amount given the change in volume at constant temperature and pressure. The ideal gas law ( PV = nrt ) describes the relationship among pressure P, volume V, temperature T, and molar amount n. When some of these variables are constant, the ideal gas law can be rearranged in different ways to take the following forms where k is a constant: Name Expression Constant Boyle's law PV = nrt = k n and T V nr Charles's law = = k n and P T P V RT Avogadro's law n = = k T and P P A certain amount of chlorine gas was placed inside a cylinder with a movable piston at one end. The initial volume was 3.00 L and the initial pressure of chlorine was 1.50 atm. The piston was pushed down to change the volume to 1.00 L. Calculate the final pressure of the gas if the temperature and number of moles of chlorine remain constant.. Express your answer with the appropriate units. Hint 1. Identify the law that applies to the problem Which gas law applies to this situation? Boyle's law Charles's law Avogadro's law Hint 2. How to set up the equation In this problem, the volume is changing while the amount of gas and the temperature remain the same. Since the product of pressure and volume is constant, we can set up the following equation 5 of 16 10/28/14 8:44 PM
6 and solve it for : (PV ) initial = (PV ) final = = 4.50 Boyle's law describes the inverse relationship between volume and pressure of an ideal gas. When the temperature and amount of a gas remain fixed, an increase in volume results in a lower pressure, and a decrease in volume results in a higher pressure. Part B In an air-conditioned room at 19.0 C, a spherical balloon had the diameter of 50.0 cm. When taken outside on a hot summer day, the balloon expanded to 51.0 cm in diameter. What was the temperature outside in degrees Celsius? Assume that the balloon is a perfect sphere and that the pressure and number of moles of air molecules remains the same. Hint 1. How to approach the problem The pressure and the amount of air inside the balloon remain the same. Therefore this is a Charles's law problem. We can set up the following equation and solve it for T final : V ( = ( T ) V initial T ) final Start by calculating the initial and final volumes from the given diameters. Plug these values into the equation along with initial temperature in kelvins. Solve for the final temperature in kelvins and then convert it to degrees Celsius. Hint 2. Calculate the initial volume of the balloon The diameter of a spherical balloon is 50.0 cm. Calculate the volume of the balloon in liters. Hint 1. Formula for volume of a sphere The formula for the volume of a sphere is 4 V = πr 3 3 where r is the radius of the sphere and π is the constant equal to Hint 2. Conversion factor between cubic centimeters and liters 6 of 16 10/28/14 8:44 PM
7 1 L is equal to 1000 cm 3. V initial = 65.4 Substitute this value for V initial in the appropriate gas law equation. Hint 3. Calculate the final volume of the balloon The diameter of a spherical balloon is 51.0 cm. Calculate the volume of the balloon in liters. Hint 1. Formula for volume of a sphere The formula for the volume of a sphere is 4 V = πr 3 3 where r is the radius of the sphere and π is the constant equal to Hint 2. Conversion factor between cubic centimeters and liters 1 L is equal to 1000 cm 3. V final = 69.5 Substitute this value for V final in the Charles's law equation. 7 of 16 10/28/14 8:44 PM
8 Hint 4. Convert the initial temperature to kelvins The initial temperature of the balloon is 19.0 C. What is the equivalent value on the Kelvin scale? T initial = 292 Substitute this value for V final in the appropriate gas law equation. Hint 5. Calculate the final temperature in kelvins Calculate the outside temperature in kelvins. Hint 1. How to approach the problem The pressure and the amount of air inside the balloon remain the same. Therefore this is a Charles's law problem. We can set up the following equation and solve it for T final : V ( = ( T ) V initial T ) final T final = 310 Now you can convert this value to degrees Celsius. outside temperature = 36.9 Since, at a constant pressure, the volume of an ideal gas is directly proportional to its temperature, the plot of volume versus temperature is a straight line. When temperature is plotted on the Celsius scale, the straight line can be extrapolated to the point where the volume is zero and the temperature is 273 C. Because matter cannot have a negative volume, 273 C must be the lowest possible temperature, absolute zero. 8 of 16 10/28/14 8:44 PM
9 Part C A cylinder with a movable piston contains 2.00 g of helium, He, at room temperature. More helium was added to the cylinder and the volume was adjusted so that the gas pressure remained the same. How many grams of helium were added to the cylinder if the volume was changed from 2.00 L to 2.70 L? (The temperature was held constant.) Hint 1. How to approach the problem The pressure and temperature are held constant, so this is an Avogadro's law problem. We can set up the following equation and solve it for n final : V V ( n ) = ( n ) initial final Start by converting grams to moles and then solving this equation for n final. The number of moles added is the difference between the final and initial molar amounts. Hint 2. Calculate the initial number of moles How many moles are in 2.00 g of helium, He? Hint 1. Find the molar mass of helium What is the molar mass of He? molar mass of He = 4.00 n initial = Hint 3. Calculate the final number of moles A L cylinder contained mol of helium at a certain pressure. After more helium was added to the cylinder, the volume was changed to 2.70 L to keep the pressure the same. Calculate the final number of moles of the gas. 9 of 16 10/28/14 8:44 PM
10 Hint 1. How to approach the problem The pressure and temperature are held constant, so this is an Avogadro's law problem. We can set up the following equation and solve it for n final : V V ( n ) = ( n ) initial final n final = = Now that you know the initial and final numbers of moles, you can calculate the difference and convert it to grams. mass of helium added = = According to Avogadro's law, the volume of an ideal gas is directly proportional to its molar amount. Put another way, the law also says that equal volumes of different gases at the same temperature and pressure contain the same molar amounts. At 0 C and 1 atm (standard conditions), 1 mol of any gas occupies a volume of 22.4 L (standard molar volume). Chapter 10 Question 3 - Short Answer Description: (a) How many molecules are there in 4.00 L of oxygen gas at 500. degree(s) C and 50.0 torr? How many molecules are there in 4.00 L of oxygen gas at 500. C and 50.0 torr? 10 of 16 10/28/14 8:44 PM
11 Chapter 10 Question 23 - Bimodal Description: (a) A mol sample of gas in a 525 ml container has a pressure of 312 torr. The temperature of the gas is C. A mol sample of gas in a 525 ml container has a pressure of 312 torr. The temperature of the gas is C Chapter 10 Question 15 - Algorithmic Description: (a) A sample of gas (1.3 mol) occupies L at 25 C and strings_1 atm. A sample of gas (1.3 mol) occupies L at 25 C and 3.0 atm Chapter 10 Question 26 - Multiple Choice Description: (a) Sodium bicarbonate is reacted with concentrated hydrochloric acid at 25.0 C and 1.50 atm. The reaction of 7.75 kg of bicarbonate with excess hydrochloric acid under these conditions will produce L of CO2. 11 of 16 10/28/14 8:44 PM
12 Sodium bicarbonate is reacted with concentrated hydrochloric acid at 25.0 C and 1.50 atm. The reaction of 7.75 kg of bicarbonate with excess hydrochloric acid under these conditions will produce L of CO x x x x x 10 2 Chapter 10 Question 20 - Multiple Choice Description: (a) The molar volume of a gas at STP is L. The molar volume of a gas at STP is L Chapter 10 Question 21 - Multiple Choice Description: (a) How many moles of gas are there in a 45.0 L container at 25.0 C and mm Hg? How many moles of gas are there in a 45.0 L container at 25.0 C and mm Hg? 12 of 16 10/28/14 8:44 PM
13 Chapter 10 Question 22 - Algorithmic Description: (a) Calcium hydride ((CaH)_2) reacts with water to form hydrogen gas: (CaH)_2(s) + (2H)_2 O (l) rightarrow (Ca(OH))_2 (aq) + (2H)_2 (g) How many grams of (CaH)_2 are needed to generate strings_6 L of H_2 gas at a pressure of strings_7 atm and... Calcium hydride ( CaH 2 ) reacts with water to form hydrogen gas: CaH 2 (s) + 2H 2 O(l) Ca(OH) 2 (aq) + 2H 2 (g) How many grams of CaH 2 are needed to generate 45.0 L of H 2 gas at a pressure of atm and a temperature of 32 C? Chapter 10 Question 28 - Bimodal Description: (a) The molecular weight of a gas is g/mol if 6.7 g of the gas occupies 6.3 L at STP. The molecular weight of a gas is g/mol if 6.7 g of the gas occupies 6.3 L at STP. 13 of 16 10/28/14 8:44 PM
14 27 3.0! ! x 10 3 Chapter 10 Question 26 - Bimodal Description: (a) The density of N2O at 1.53 atm and 45.2 C is g/l. The density of N2O at 1.53 atm and 45.2 C is g/l Chapter 10 Question 60 - Bimodal Description: (a) CO (5.00 g) and CO2 (5.00 g) were placed in a ml container at 50.0 C. The partial pressure of CO in the container was atm. CO (5.00 g) and CO2 (5.00 g) were placed in a ml container at 50.0 C. The partial pressure of CO in the container was atm. 14 of 16 10/28/14 8:44 PM
15 Chapter 10 Question 48 - Bimodal Description: (a) A sample of He gas (3.0 L) at 5.6 atm and 25 C was combined with 4.5 L of Ne gas at 3.6 atm and 25 C at constant temperature in a 9.0 L flask. The total pressure in the flask was atm. Assume the initial pressure in the flask was... A sample of He gas (3.0 L) at 5.6 atm and 25 C was combined with 4.5 L of Ne gas at 3.6 atm and 25 C at constant temperature in a 9.0 L flask. The total pressure in the flask was atm. Assume the initial pressure in the flask was 0.00 atm and the temperature upon mixing was 25 C Problem Description: A mixture of gases contains m_1 of N_2, m_2 of H_2, and m_3 of (NH)_3. The total pressure of the mixture is P. (a) What is the partial pressure of N_2? (b) What is the partial pressure of H_2? (c) What is the partial pressure of (NH)_3? A mixture of gases contains g of N 2, 1.84 g of H 2, and 7.95 g of NH 3. The total pressure of the mixture is 1.75 atm. What is the partial pressure of N 2? 15 of 16 10/28/14 8:44 PM
16 P N2 = = atm Part B What is the partial pressure of H 2? P H2 = = atm Part C What is the partial pressure of NH 3? P NH3 = = atm Copyright 2014 Pearson. All rights reserved. Legal Notice Privacy Policy Permissions Support 16 of 16 10/28/14 8:44 PM
The Gas Laws. Our Atmosphere. Pressure = Units of Pressure. Barometer. Chapter 10
Our Atmosphere The Gas Laws 99% N 2 and O 2 78% N 2 80 70 Nitrogen Chapter 10 21% O 2 1% CO 2 and the Noble Gases 60 50 40 Oxygen 30 20 10 0 Gas Carbon dioxide and Noble Gases Pressure Pressure = Force
More informationGas Laws. The kinetic theory of matter states that particles which make up all types of matter are in constant motion.
Name Period Gas Laws Kinetic energy is the energy of motion of molecules. Gas state of matter made up of tiny particles (atoms or molecules). Each atom or molecule is very far from other atoms or molecules.
More informationCHEMISTRY GAS LAW S WORKSHEET
Boyle s Law Charles Law Guy-Lassac's Law Combined Gas Law For a given mass of gas at constant temperature, the volume of a gas varies inversely with pressure PV = k The volume of a fixed mass of gas is
More informationCHAPTER 12. Gases and the Kinetic-Molecular Theory
CHAPTER 12 Gases and the Kinetic-Molecular Theory 1 Gases vs. Liquids & Solids Gases Weak interactions between molecules Molecules move rapidly Fast diffusion rates Low densities Easy to compress Liquids
More informationCHEMISTRY. Matter and Change. Section 13.1 Section 13.2 Section 13.3. The Gas Laws The Ideal Gas Law Gas Stoichiometry
CHEMISTRY Matter and Change 13 Table Of Contents Chapter 13: Gases Section 13.1 Section 13.2 Section 13.3 The Gas Laws The Ideal Gas Law Gas Stoichiometry State the relationships among pressure, temperature,
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 informationKinetic Theory of Gases. 6.1 Properties of Gases 6.2 Gas Pressure. Properties That Describe a Gas. Gas Pressure. Learning Check.
Chapter 6 Gases Kinetic Theory of Gases 6.1 Properties of Gases 6.2 Gas Pressure A gas consists of small particles that move rapidly in straight lines. have essentially no attractive (or repulsive) forces.
More informationMULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
Chapter 10 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) A gas at a pressure of 10.0 Pa exerts a force of N on an area of 5.5 m2. A) 1.8 B) 0.55
More informationTemperature. Number of moles. Constant Terms. Pressure. Answers Additional Questions 12.1
Answers Additional Questions 12.1 1. A gas collected over water has a total pressure equal to the pressure of the dry gas plus the pressure of the water vapor. If the partial pressure of water at 25.0
More informationGases. Macroscopic Properties. Petrucci, Harwood and Herring: Chapter 6
Gases Petrucci, Harwood and Herring: Chapter 6 CHEM 1000A 3.0 Gases 1 We will be looking at Macroscopic and Microscopic properties: Macroscopic Properties of bulk gases Observable Pressure, volume, mass,
More informationAS1 MOLES. oxygen molecules have the formula O 2 the relative mass will be 2 x 16 = 32 so the molar mass will be 32g mol -1
Moles 1 MOLES The mole the standard unit of amount of a substance the number of particles in a mole is known as Avogadro s constant (L) Avogadro s constant has a value of 6.023 x 10 23 mol -1. Example
More informationLecture Notes: Gas Laws and Kinetic Molecular Theory (KMT).
CHEM110 Week 9 Notes (Gas Laws) Page 1 of 7 Lecture Notes: Gas Laws and Kinetic Molecular Theory (KMT). Gases Are mostly empty space Occupy containers uniformly and completely Expand infinitely Diffuse
More informationF321 MOLES. Example If 1 atom has a mass of 1.241 x 10-23 g 1 mole of atoms will have a mass of 1.241 x 10-23 g x 6.02 x 10 23 = 7.
Moles 1 MOLES The mole the standard unit of amount of a substance (mol) the number of particles in a mole is known as Avogadro s constant (N A ) Avogadro s constant has a value of 6.02 x 10 23 mol -1.
More informationGases. States of Matter. Molecular Arrangement Solid Small Small Ordered Liquid Unity Unity Local Order Gas High Large Chaotic (random)
Gases States of Matter States of Matter Kinetic E (motion) Potential E(interaction) Distance Between (size) Molecular Arrangement Solid Small Small Ordered Liquid Unity Unity Local Order Gas High Large
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 informationExam 4 Practice Problems false false
Exam 4 Practice Problems 1 1. Which of the following statements is false? a. Condensed states have much higher densities than gases. b. Molecules are very far apart in gases and closer together in liquids
More informationGases and Kinetic-Molecular Theory: Chapter 12. Chapter Outline. Chapter Outline
Gases and Kinetic-Molecular heory: Chapter Chapter Outline Comparison of Solids, Liquids, and Gases Composition of the Atmosphere and Some Common Properties of Gases Pressure Boyle s Law: he Volume-Pressure
More informationGas Laws. vacuum. 760 mm. air pressure. mercury
Gas Laws Some chemical reactions take place in the gas phase and others produce products that are gases. We need a way to measure the quantity of compounds in a given volume of gas and relate that to moles.
More informationThe Mole. Chapter 10. Dimensional Analysis. The Mole. How much mass is in one atom of carbon-12? Molar Mass of Atoms 3/1/2015
The Mole Chapter 10 1 Objectives Use the mole and molar mass to make conversions among moles, mass, and number of particles Determine the percent composition of the components of a compound Calculate empirical
More informationBoyles Law. At constant temperature the volume occupied by a fixed amount of gas is inversely proportional to the pressure on the gas 1 P = P
Boyles Law At constant temperature the volume occupied by a fixed amount of gas is inversely proportional to the pressure on the gas 1 or k 1 Boyles Law Example ressure olume Initial 2.00 atm 100 cm 3
More informationStoichiometry. 1. The total number of moles represented by 20 grams of calcium carbonate is (1) 1; (2) 2; (3) 0.1; (4) 0.2.
Stoichiometry 1 The total number of moles represented by 20 grams of calcium carbonate is (1) 1; (2) 2; (3) 01; (4) 02 2 A 44 gram sample of a hydrate was heated until the water of hydration was driven
More informationESSAY. Write your answer in the space provided or on a separate sheet of paper.
Test 1 General Chemistry CH116 Summer, 2012 University of Massachusetts, Boston Name ESSAY. Write your answer in the space provided or on a separate sheet of paper. 1) Sodium hydride reacts with excess
More informationAP CHEMISTRY 2009 SCORING GUIDELINES (Form B)
AP CHEMISTRY 2009 SCORING GUIDELINES (Form B) Question 3 (10 points) 2 H 2 O 2 (aq) 2 H 2 O(l) + O 2 (g) The mass of an aqueous solution of H 2 O 2 is 6.951 g. The H 2 O 2 in the solution decomposes completely
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 informationEXPERIMENT 13: THE IDEAL GAS LAW AND THE MOLECULAR WEIGHT OF GASES
Name Section EXPERIMENT 13: THE IDEAL GAS LAW AND THE MOLECULAR WEIGHT OF GASES PRE-LABORATORY QUESTIONS The following preparatory questions should be answered before coming to lab. They are intended to
More informationOther Stoich Calculations A. mole mass (mass mole) calculations. GIVEN mol A x CE mol B. PT g A CE mol A MOLE MASS :
Chem. I Notes Ch. 12, part 2 Using Moles NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics. 1 MOLE = 6.02 x 10 23 representative particles (representative particles
More informationEXPERIMENT 15: Ideal Gas Law: Molecular Weight of a Vapor
EXPERIMENT 15: Ideal Gas Law: Molecular Weight of a Vapor Purpose: In this experiment you will use the ideal gas law to calculate the molecular weight of a volatile liquid compound by measuring the mass,
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 informationMole Notes.notebook. October 29, 2014
1 2 How do chemists count atoms/formula units/molecules? How do we go from the atomic scale to the scale of everyday measurements (macroscopic scale)? The gateway is the mole! But before we get to the
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 informationMolar Mass of Butane
Cautions Butane is toxic and flammable. No OPEN Flames should be used in this experiment. Purpose The purpose of this experiment is to determine the molar mass of butane using Dalton s Law of Partial Pressures
More informationUnit 3 Notepack Chapter 7 Chemical Quantities Qualifier for Test
Unit 3 Notepack Chapter 7 Chemical Quantities Qualifier for Test NAME Section 7.1 The Mole: A Measurement of Matter A. What is a mole? 1. Chemistry is a quantitative science. What does this term mean?
More informationChapter 13 Gases. Review Skills
Chapter 13 Gases t s Monday morning, and Lilia is walking out of the chemistry building, thinking about the introductory lecture on gases that her instructor just presented. Dr. Scanlon challenged the
More informationMULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
General Chemistry PHS 1015 Practice Exam 4 Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Which of the following statements about pressure
More informationCSUS Department of Chemistry Experiment 8 Chem.1A
EXPERIMENT #8 Name: PRE-LABORATORY ASSIGNMENT: Lab Section 1. The alkali metals are so reactive that they react directly with water in the absence of acid. For example, potassium reacts with water as follows:
More informationEXPERIMENT 9 Evaluation of the Universal Gas Constant, R
Outcomes EXPERIMENT 9 Evaluation of the Universal Gas Constant, R After completing this experiment, the student should be able to: 1. Determine universal gas constant using reaction of an acid with a metal.
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 informationDETERMINING THE MOLAR MASS OF CARBON DIOXIDE
DETERMINING THE MOLAR MASS OF CARBON DIOXIDE PURPOSE: The goal of the experiment is to determine the molar mass of carbon dioxide and compare the experimentally determined value to the theoretical value.
More informationIDEAL AND NON-IDEAL GASES
2/2016 ideal gas 1/8 IDEAL AND NON-IDEAL GASES PURPOSE: To measure how the pressure of a low-density gas varies with temperature, to determine the absolute zero of temperature by making a linear fit to
More informationReview - After School Matter Name: Review - After School Matter Tuesday, April 29, 2008
Name: Review - After School Matter Tuesday, April 29, 2008 1. Figure 1 The graph represents the relationship between temperature and time as heat was added uniformly to a substance starting at a solid
More informationChemistry 110 Lecture Unit 5 Chapter 11-GASES
Chemistry 110 Lecture Unit 5 Chapter 11-GASES I. PROPERITIES OF GASES A. Gases have an indefinite shape. B. Gases have a low density C. Gases are very compressible D. Gases exert pressure equally in all
More informationWhat s in a Mole? Molar Mass
LESSON 10 What s in a Mole? Molar Mass OVERVIEW Key Ideas Lesson Type Lab: Groups of 4 Chemists compare moles of substances rather than masses because moles are a way of counting atoms. When considering
More informationCHEMISTRY II FINAL EXAM REVIEW
Name Period CHEMISTRY II FINAL EXAM REVIEW Final Exam: approximately 75 multiple choice questions Ch 12: Stoichiometry Ch 5 & 6: Electron Configurations & Periodic Properties Ch 7 & 8: Bonding Ch 14: Gas
More informationTHE IDEAL GAS LAW AND KINETIC THEORY
Chapter 14 he Ideal Gas Law and Kinetic heory Chapter 14 HE IDEAL GAS LAW AND KINEIC HEORY REIEW Kinetic molecular theory involves the study of matter, particularly gases, as very small particles in constant
More informationChemistry 13: States of Matter
Chemistry 13: States of Matter Name: Period: Date: Chemistry Content Standard: Gases and Their Properties The kinetic molecular theory describes the motion of atoms and molecules and explains the properties
More informationAppendix D. Reaction Stoichiometry D.1 INTRODUCTION
Appendix D Reaction Stoichiometry D.1 INTRODUCTION In Appendix A, the stoichiometry of elements and compounds was presented. There, the relationships among grams, moles and number of atoms and molecules
More information1.4.6-1.4.8 Gas Laws. Heat and Temperature
1.4.6-1.4.8 Gas Laws Heat and Temperature Often the concepts of heat and temperature are thought to be the same, but they are not. Perhaps the reason the two are incorrectly thought to be the same is because
More informationChemistry 101 Generating Hydrogen Gas
Chemistry 101 Generating Hydrogen Gas Objectives To experimentally verify the molar volume of hydrogen gas at STP To gain experience in collecting gas over water Discussion The molar volume of a gas is
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 informationCHEM 120 Online Chapter 7
CHEM 120 Online Chapter 7 Date: 1. Which of the following statements is not a part of kinetic molecular theory? A) Matter is composed of particles that are in constant motion. B) Particle velocity increases
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 information7. Gases, Liquids, and Solids 7.1 Kinetic Molecular Theory of Matter
7. Gases, Liquids, and Solids 7.1 Kinetic Molecular Theory of Matter Kinetic Molecular Theory of Matter The Kinetic Molecular Theory of Matter is a concept that basically states that matter is composed
More informationDetermining Equivalent Weight by Copper Electrolysis
Purpose The purpose of this experiment is to determine the equivalent mass of copper based on change in the mass of a copper electrode and the volume of hydrogen gas generated during an electrolysis reaction.
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 informationChem 1A Exam 2 Review Problems
Chem 1A Exam 2 Review Problems 1. At 0.967 atm, the height of mercury in a barometer is 0.735 m. If the mercury were replaced with water, what height of water (in meters) would be supported at this pressure?
More informationHEAT UNIT 1.1 KINETIC THEORY OF GASES. 1.1.1 Introduction. 1.1.2 Postulates of Kinetic Theory of Gases
UNIT HEAT. KINETIC THEORY OF GASES.. Introduction Molecules have a diameter of the order of Å and the distance between them in a gas is 0 Å while the interaction distance in solids is very small. R. Clausius
More informationIdeal Gas Law Introduction Lesson Plan Keith Newman Chemistry 511 Final Project 2006/2007
Ideal Gas Law Introduction Lesson Plan Keith Newman Chemistry 511 Final Project 2006/2007 Objectives: Students will be able to solve ideal gas law problems using algebraic ratios. Students will be able
More informationStoichiometry Exploring a Student-Friendly Method of Problem Solving
Stoichiometry Exploring a Student-Friendly Method of Problem Solving Stoichiometry comes in two forms: composition and reaction. If the relationship in question is between the quantities of each element
More informationStoichiometry. 1. The total number of moles represented by 20 grams of calcium carbonate is (1) 1; (2) 2; (3) 0.1; (4) 0.2.
Stoichiometry 1 The total number of moles represented by 20 grams of calcium carbonate is (1) 1; (2) 2; (3) 01; (4) 02 2 A 44 gram sample of a hydrate was heated until the water of hydration was driven
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 information= 800 kg/m 3 (note that old units cancel out) 4.184 J 1000 g = 4184 J/kg o C
Units and Dimensions Basic properties such as length, mass, time and temperature that can be measured are called dimensions. Any quantity that can be measured has a value and a unit associated with it.
More informationSolution. Practice Exercise. Concept Exercise
Example Exercise 9.1 Atomic Mass and Avogadro s Number Refer to the atomic masses in the periodic table inside the front cover of this textbook. State the mass of Avogadro s number of atoms for each of
More informationDescription of the Mole Concept:
Description of the Mole Concept: Suppose you were sent into the store to buy 36 eggs. When you picked them up you would get 3 boxes, each containing 12 eggs. You just used a mathematical device, called
More informationStoichiometry V = 9.98 L CO2. 34.0 ml H 2 SO 4 soln 6.0 mol H 2 SO. 1000 ml H 2 SO 4 soln. 2 mol CO = 0.408 mol CO 2 1 mol H 2 SO 4
Stoichiometry We cannot count molecules so instead we weigh them; however, it is etremely inconvenient to weigh gases. So, when adding gases to a reaction how do we measure the amount of gas? We use the
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 informationName Date Class CHEMICAL QUANTITIES. SECTION 10.1 THE MOLE: A MEASUREMENT OF MATTER (pages 287 296)
Name Date Class 10 CHEMICAL QUANTITIES SECTION 10.1 THE MOLE: A MEASUREMENT OF MATTER (pages 287 296) This section defines the mole and explains how the mole is used to measure matter. It also teaches
More informationChapter 8: Gases and Gas Laws.
133 Chapter 8: Gases and Gas Laws. The first substances to be produced and studied in high purity were gases. Gases are more difficult to handle and manipulate than solids and liquids, since any minor
More informationName Class Date. In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question.
Assessment Chapter Test A Chapter: States of Matter In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question. 1. The kinetic-molecular
More informationDATE PERFORMED: DATE DUE:
Sample lab report The first page is the cover page for the report. Title: Experiment #12 Determination of the Atomic Mass of Zinc ( p 117, Hunt and Block) YOUR NAME: PARTNER(S) NAME: DATE PERFORMED: DATE
More informationMULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
Exam Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Given: 4 NO2(g) + O2(g) 2 N2O5(g) ΔH = -110.2 kj find ΔH for N2O5(g) 2 NO2(g) + 1/2 O2(g).
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 informationTHE KINETIC THEORY OF GASES
Chapter 19: THE KINETIC THEORY OF GASES 1. Evidence that a gas consists mostly of empty space is the fact that: A. the density of a gas becomes much greater when it is liquefied B. gases exert pressure
More informationCHAPTER 8: CHEMICAL COMPOSITION
CHAPTER 8: CHEMICAL COMPOSITION Active Learning: 1-4, 6-8, 12, 18-25; End-of-Chapter Problems: 3-4, 9-82, 84-85, 87-92, 94-104, 107-109, 111, 113, 119, 125-126 8.2 ATOMIC MASSES: COUNTING ATOMS BY WEIGHING
More informationThe Mole Concept and Atoms
Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Chapter 4 24 September 2013 Calculations and the Chemical Equation The Mole Concept and Atoms Atoms are exceedingly
More informationCHEM 105 HOUR EXAM III 28-OCT-99. = -163 kj/mole determine H f 0 for Ni(CO) 4 (g) = -260 kj/mole determine H f 0 for Cr(CO) 6 (g)
CHEM 15 HOUR EXAM III 28-OCT-99 NAME (please print) 1. a. given: Ni (s) + 4 CO (g) = Ni(CO) 4 (g) H Rxn = -163 k/mole determine H f for Ni(CO) 4 (g) b. given: Cr (s) + 6 CO (g) = Cr(CO) 6 (g) H Rxn = -26
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 informationCP Chemistry Review for Stoichiometry Test
CP Chemistry Review for Stoichiometry Test Stoichiometry Problems (one given reactant): 1. Make sure you have a balanced chemical equation 2. Convert to moles of the known substance. (Use the periodic
More informationCHEM 36 General Chemistry EXAM #1 February 13, 2002
CHEM 36 General Chemistry EXAM #1 February 13, 2002 Name: Serkey, Anne INSTRUCTIONS: Read through the entire exam before you begin. Answer all of the questions. For questions involving calculations, show
More informationMultiple Choice questions (one answer correct)
Mole Concept Multiple Choice questions (one answer correct) (1) Avogadro s number represents the number of atoms in (a) 12g of C 12 (b) 320g of sulphur (c) 32g of oxygen (d) 12.7g of iodine (2) The number
More informationUnit 2: Quantities in Chemistry
Mass, Moles, & Molar Mass Relative quantities of isotopes in a natural occurring element (%) E.g. Carbon has 2 isotopes C-12 and C-13. Of Carbon s two isotopes, there is 98.9% C-12 and 11.1% C-13. Find
More informationChemical Composition. Introductory Chemistry: A Foundation FOURTH EDITION. Atomic Masses. Atomic Masses. Atomic Masses. Chapter 8
Introductory Chemistry: A Foundation FOURTH EDITION by Steven S. Zumdahl University of Illinois Chemical Composition Chapter 8 1 2 Atomic Masses Balanced equation tells us the relative numbers of molecules
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 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 informationBalance the following equation: KClO 3 + C 12 H 22 O 11 KCl + CO 2 + H 2 O
Balance the following equation: KClO 3 + C 12 H 22 O 11 KCl + CO 2 + H 2 O Ans: 8 KClO 3 + C 12 H 22 O 11 8 KCl + 12 CO 2 + 11 H 2 O 3.2 Chemical Symbols at Different levels Chemical symbols represent
More informationPHYS-2010: General Physics I Course Lecture Notes Section XIII
PHYS-2010: General Physics I Course Lecture Notes Section XIII Dr. Donald G. Luttermoser East Tennessee State University Edition 2.5 Abstract These class notes are designed for use of the instructor and
More informationFormulas, Equations and Moles
Chapter 3 Formulas, Equations and Moles Interpreting Chemical Equations You can interpret a balanced chemical equation in many ways. On a microscopic level, two molecules of H 2 react with one molecule
More informationEXPERIMENT 12: Empirical Formula of a Compound
EXPERIMENT 12: Empirical Formula of a Compound INTRODUCTION Chemical formulas indicate the composition of compounds. A formula that gives only the simplest ratio of the relative number of atoms in a compound
More informationExperiment 3 Limiting Reactants
3-1 Experiment 3 Limiting Reactants Introduction: Most chemical reactions require two or more reactants. Typically, one of the reactants is used up before the other, at which time the reaction stops. The
More informationChemistry 151 Final Exam
Chemistry 151 Final Exam Name: SSN: Exam Rules & Guidelines Show your work. No credit will be given for an answer unless your work is shown. Indicate your answer with a box or a circle. All paperwork must
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 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 informationChemistry 212 VAPOR PRESSURE OF WATER LEARNING OBJECTIVES
Chemistry 212 VAPOR PRESSURE OF WATER LEARNING OBJECTIVES The learning objectives of this experiment are to explore the relationship between the temperature and vapor pressure of water. determine the molar
More informationPage 2. Base your answers to questions 7 through 9 on this phase diagram
1. The normal boiling point of water is often depressed at high altitudes. Which of the following explains this phenomenon? t high altitudes, the lower atmospheric pressure equals the equilibrium water
More informationChapter 10. Can You... 1. draw the Lewis structure for a given covalently bonded molecule?
Chapter 10 Can You... 1. draw the Lewis structure for a given covalently bonded molecule? e.g. SF 6 and CH 3 Cl 2. identify and count the number of non-bonding and bonding domains within a given covalently
More informationProblem Set 3 Solutions
Chemistry 360 Dr Jean M Standard Problem Set 3 Solutions 1 (a) One mole of an ideal gas at 98 K is expanded reversibly and isothermally from 10 L to 10 L Determine the amount of work in Joules We start
More informationName Date Class CHEMICAL QUANTITIES. SECTION 10.1 THE MOLE: A MEASUREMENT OF MATTER (pages 287 296)
10 CHEMICAL QUANTITIES SECTION 10.1 THE MOLE: A MEASUREMENT OF MATTER (pages 287 296) This section defines the mole and explains how the mole is used to measure matter. It also teaches you how to calculate
More informationTemperature Measure of KE At the same temperature, heavier molecules have less speed Absolute Zero -273 o C 0 K
Temperature Measure of KE At the same temperature, heavier molecules have less speed Absolute Zero -273 o C 0 K Kinetic Molecular Theory of Gases 1. Large number of atoms/molecules in random motion 2.
More informationChapter 3. Mass Relationships in Chemical Reactions
Chapter 3 Mass Relationships in Chemical Reactions This chapter uses the concepts of conservation of mass to assist the student in gaining an understanding of chemical changes. Upon completion of Chapter
More information2. ATOMIC, MOLECULAR AND EQUIVALENT MASSES
2. ATOMIC, MOLECULAR AND EQUIVALENT MASSES INTRODUCTION: EQUIVALENT WEIGHT Since hydrogen is the lightest of all elements, it was chosen as a standard for determination of equivalent weights. On this basis,
More informationThe Molar Mass of a Gas
The Molar Mass of a Gas Goals The purpose of this experiment is to determine the number of grams per mole of a gas by measuring the pressure, volume, temperature, and mass of a sample. Terms to Know Molar
More information