Chemistry: The Molecular Nature of Matter
7th Edition
ISBN: 9781118516461
Author: Neil D. Jespersen, Alison Hyslop
Publisher: WILEY
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Chapter 6, Problem 44RQ
What fundamental fact about
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Chapter 6 Solutions
Chemistry: The Molecular Nature of Matter
Ch. 6 - Prob. 1PECh. 6 - Prob. 2PECh. 6 - When monitoring a reaction, the initial...Ch. 6 - Practice Exercise 6.4
A hall bearing at is...Ch. 6 - Prob. 5PECh. 6 - Silicon, used in computer chips, has a specific...Ch. 6 - Would the explosive reaction of hydrogen and...Ch. 6 - Practice Exercise 6.8
When ammonium nitrate is...Ch. 6 - An exothermic reaction is carried out at a...Ch. 6 - For an exothermic reaction that is conducted under...
Ch. 6 - Since it can be obtained in very high purity,...Ch. 6 - A 1.50 g sample of pure sucrose is burned in a...Ch. 6 - For the Analyzing and Solving Multi-Concept...Ch. 6 - Practice Exercise 6.14
The exact same procedure as...Ch. 6 - The combustion of methane can be represented by...Ch. 6 - Practice Exercise 6.16
What is the thermochemical...Ch. 6 - Two oxides of copper can be made from copper by...Ch. 6 - Consider the following thermochemical...Ch. 6 - Given the following thermochemical equations,...Ch. 6 - Ethanol, C2H5OH, is made industrially by the...Ch. 6 - Practice Exercise 6.21
The heat of combustion, ,...Ch. 6 - Practice Exercise 6.22
n-Octane, , has a standard...Ch. 6 - Write the thermochemical equation that would be...Ch. 6 - Write the thermochemical equation that would be...Ch. 6 - Use heats of formation data from Table 6.2 to...Ch. 6 - Write thermochemical equations corresponding to Hf...Ch. 6 - Calculate H for the following reactions:...Ch. 6 - Give definitions for (a) energy, (b) kinetic...Ch. 6 - Prob. 2RQCh. 6 - Prob. 3RQCh. 6 - 6.4 State the law of conservation of energy....Ch. 6 - 6.5 A pendulum such as a swinging chandelier...Ch. 6 - Prob. 6RQCh. 6 - 6.7 What is meant by the term chemical energy?
Ch. 6 - How does the potential energy change (increase,...Ch. 6 - What is the SI unit of energy? How much energy (in...Ch. 6 - 6.10 Why is hear considered a waste product in a...Ch. 6 - Prob. 11RQCh. 6 - 6.12 How is internal energy related to molecular...Ch. 6 - On a molecular level, how is thermal equilibrium...Ch. 6 - Consider the distribution of molecular kinetic...Ch. 6 - Suppose the temperature of an object is raised...Ch. 6 - A quart of boiling water will cause a more severe...Ch. 6 - Prob. 17RQCh. 6 - What is a state function? Give four examples that...Ch. 6 - How would you determine whether an experimental...Ch. 6 - 6.20 How can the state of a system be specified?
Ch. 6 - 6.21 What do the terms system and surroundings...Ch. 6 - What are the names of the thermal properties whose...Ch. 6 - 6.23 For samples with the same mass, which kind of...Ch. 6 - 6.24 How do heat capacity and specific hear...Ch. 6 - Prob. 25RQCh. 6 - 6.26 Suppose object A has twice the specific heat...Ch. 6 - In a certain chemical reaction, there is a...Ch. 6 - 6.28 What term do we use to describe a reaction...Ch. 6 - 6.29 What term is used to describe a reaction that...Ch. 6 - 6.30 When gasoline burns, it reacts with oxygen in...Ch. 6 - Write the equation that states the first law of...Ch. 6 - How are heat and work defined?Ch. 6 - Devise an example, similar to the one described in...Ch. 6 - 6.34 Why are heat and work not state functions?
Ch. 6 - When we measure the heat of combustion of glucose,...Ch. 6 - Consider the reaction...Ch. 6 - How is enthalpy defined?Ch. 6 - What is the sign of H for an endothermic change?Ch. 6 - 6.39 If the enthalpy of a system increases by 100...Ch. 6 - If a system containing gases expands and pushes...Ch. 6 - 6.41 Why do standard reference values for...Ch. 6 - What distinguishes a thermochemical equation from...Ch. 6 - Why are fractional coefficients permitted in a...Ch. 6 - 6.44 What fundamental fact about makes Hess’s law...Ch. 6 - 6.45 What two conditions must be met by a...Ch. 6 - Describe what must be done with the standard...Ch. 6 - What two additional thermochemical equations are...Ch. 6 - Peptides, small parts of proteins, contain...Ch. 6 - If a car increases its speed from 30 mph to 60...Ch. 6 - 6.50 If the mass of a truck is doubled—for...Ch. 6 - 6.51 What is the kinetic energy, in joules, of a...Ch. 6 - What is the kinetic energy, in joules, of a...Ch. 6 - How much heat, in joules and in calories, must be...Ch. 6 - 6.54 How much heat, in joules and calories, is...Ch. 6 - How many grams of water can be heated from...Ch. 6 - 6.56 How many grams of copper can be cooled from ...Ch. 6 - A 50.0 g piece of a metal at 100.0C was plunged...Ch. 6 - 6.58 A sample of copper was heated to and then...Ch. 6 - 6.59 Calculate the molar heat capacity of iron in...Ch. 6 - 6.60 What is the molar heat capacity of ethyl...Ch. 6 - A vat of 4.54 kg of water underwent a decrease in...Ch. 6 - A container filled with 2.46 kg of water underwent...Ch. 6 - 6.63 Nitric acid neutralizes potassium hydroxide....Ch. 6 - In the reaction between formic acid (HCHO2) and...Ch. 6 - 6.65 A 1.000 mol sample of propane, a gas used for...Ch. 6 - Toluene, C7H8, is used in the manufacture of...Ch. 6 - If a system does 4$ J of work and receives 28 J of...Ch. 6 - If a system has 48 J of work done on it and...Ch. 6 - An automobile engine converts heat into work via a...Ch. 6 - Chargers for cell phones get warm while they are...Ch. 6 - If the engine in Problem 6.69 absorbs 250 joules...Ch. 6 - If a battery can release 535 J of energy and 455 J...Ch. 6 - Ammonia reacts with oxygen as follows:...Ch. 6 - One thermochemical equation for the reaction of...Ch. 6 - Magnesium bums in air to produce a bright light...Ch. 6 - Methanol is the fuel in canned heat containers...Ch. 6 - Methane burns with oxygen to produce carbon...Ch. 6 - Methanol, as described in Problem 6.76, is used to...Ch. 6 - *6.79 Construct an enthalpy diagram that shows the...Ch. 6 - *6.80 Construct an enthalpy diagram for the...Ch. 6 - Show how the equations...Ch. 6 - 6.82 We can generate hydrogen chloride by heating...Ch. 6 - Calculate H in kilojoules for the following...Ch. 6 - Calcium hydroxide reacts with hydrochloric acid by...Ch. 6 - Given the following thermochemical equations,...Ch. 6 - 6.86 Given the following thermochemical...Ch. 6 - Given the following thermochemical equations,...Ch. 6 - Given the following thermochemical equations,...Ch. 6 - Which of the following thermochemical equations...Ch. 6 - Which of the following thermochemical equations...Ch. 6 - Write the thermochcmical equations, including...Ch. 6 - Write the thermochemical equations, including...Ch. 6 - Using data in Table 6.2, calculate H in kilojoules...Ch. 6 - 6.94 Using data in Table 6.2, calculate in...Ch. 6 - The value for the standard heat of combustion, H...Ch. 6 - The thermochemical equation for the combustion of...Ch. 6 - 6.97 Look at the list of substances in Table 6.1....Ch. 6 - *6.98 A dilute solution of hydrochloric acid with...Ch. 6 - A 2.00 kg piece of granite with a specific heat of...Ch. 6 - In the recovery of iron from iron ore, the...Ch. 6 - Use the results of Problem 6.100 and the data in...Ch. 6 - 6.102 The amino acid glycine, , is one of the...Ch. 6 - The value of Hf for HBr(g) was first evaluated...Ch. 6 - Acetylene, C2H2, is a gas commonly burned in...Ch. 6 - The reaction for the metabolism of sucrose,...Ch. 6 - Consider the following thermochemical...Ch. 6 - 6.107 Chlorofluoromethanes (CFMs) are carbon...Ch. 6 - Prob. 108RQCh. 6 - Suppose a truck with a mass of 14.0 tons...Ch. 6 - How much work must be done to form one mole of CH4...Ch. 6 - A cold -15C piece of copper metal weighing 7.38 g...Ch. 6 - Both Na2CO3 and NaHCO3 can be used to neutralize...Ch. 6 - *6.113 When 4.56 g of a solid mixture composed of ...Ch. 6 - Using the results from Analyzing and Solving...Ch. 6 - *6.115 For ethanol, , which is mixed with gasoline...Ch. 6 - Both calcium and potassium react with water to...Ch. 6 - 6.117 As a routine safety procedure, acids and...Ch. 6 - In an experiment, 95.0 mL of 0.225 M silver...Ch. 6 - 6.119 Growing wheat and converting it into bread...Ch. 6 - Suppose we compress a spring, tie it up tightly,...Ch. 6 - Prob. 121RQCh. 6 - Why do we usually use H rather than E when we...Ch. 6 - Prob. 123RQCh. 6 - 6.124 Find the heats of formation of some...Ch. 6 - Prob. 125RQ
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- Compounds with carboncarbon double bonds, such as ethylene, C2H4, add hydrogen in a reaction called hydrogenation. C2H4(g)+H2(g)C2H6(g) Calculate the enthalpy change for this reaction, using the following combustion data: C2H4(g)+3O2(g)2CO2(g)+2H2O(l);H=1411kJC2H6(g)+72O2(g)2CO2(g)+3H2O(l);H=1560kJH2(g)+12O2(g)H2O(l);H=286kJarrow_forwardHydrazine, N2H4, is a colorless liquid used as a rocket fuel. What is the enthalpy change for the process in which hydrazine is formed from its elements? N2(g)+2H2(g)N2H4(l) Use the following reactions and enthalpy changes: N2H4(l)+O2(g)N2(g)+2H2O(l);H=622.2kJH2(g)+12O2(g)H2O(l);H=285.8kJarrow_forwardWhen 2.50 g of methane burns in oxygen, 125 kJ of heat is produced. What is the enthalpy of combustion per mole of methane under these conditions?arrow_forward
- You discover that you cannot carry out a particular reaction for which you would like the enthalpy change. Does this mean that you will be unable to obtain this enthalpy change? Explain.arrow_forwardDefine heat. What are its units? How does it differ from energy?arrow_forwardA 0.470-g sample of magnesium reacts with 200 g dilute HCl in a coffee-cup calorimeter to form MgCl2(aq) and H2(g). The temperature increases by 10.9 C as the magnesium reacts. Assume that the mixture has the same specific heat as water and a mass of 200 g. (a) Calculate the enthalpy change for the reaction. Is the process exothermic or endothermic? (b) Write the chemical equation and evaluate H.arrow_forward
- 9.45 What happens to the temperature of a material as it undergoes an endothermic phase change? If heat is added, how can the temperature behave in this manner?arrow_forwardThe first step in the preparation of lead from its ore (galena, PbS) consists of roasting the ore. PbS(s)+32O2(g)SO2(g)+PbO(s) Calculate the standard enthalpy change for this reaction, using enthalpies of formation (see Appendix C).arrow_forwardThe equation for the fermentation of glucose to alcohol and carbon dioxide is: C6H12O6(aq) 2C2H5OH(aq) + 2CO2(g) The enthalpy change for the reaction is 67 kJ. Is this reaction exothermic or endothermic? Is energy, in the form of heat, absorbed or evolved as the reaction occurs?arrow_forward
- What mass of acetylene, C2H2(g), must be burned to produce 3420 kJ of heat, given that its enthalpy of combustion is 1301 kJ/mol? Compare this with the answer to Exercise 5.91 and determine which substance produces more heat per gram.arrow_forward9.73 Without looking up any numerical data or doing calculations, predict whether the enthalpy change for each of the following reactions should he positive, negative, or zero. (a) H2O(l)H2O(s) (b) N2(g)2N(g) (c) CH4(g)+2O2(g)CO2(g)+2H2O(l) (d) CO2(s)CO2(g)arrow_forward9.74 Without looking up any numerical data or doing calculations, predict whether the following enthalpy changes should he positive, negative, or zero. (a) Hf for H2(g) (b) Hf for O(g) (c) Hfusion for H2O (d) Hcombusion for C3H8(g)arrow_forward
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