Chemistry: An Atoms First Approach
2nd Edition
ISBN: 9781305079243
Author: Steven S. Zumdahl, Susan A. Zumdahl
Publisher: Cengage Learning
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Chapter 7, Problem 1ALQ
Interpretation Introduction
Interpretation: The metal feels colder than plastic when touch them to be explained.
Concept introduction
Conductivity: Conductivity is a capacity to conduct the
Resistance: Resistance is the quantification of struggling of electric current passed via conductor. In other words, resistance is the ratio of voltage and the electric current flows via the conductor.
Formula
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Chapter 7 Solutions
Chemistry: An Atoms First Approach
Ch. 7 - Define the following terms: potential energy,...Ch. 7 - Consider the following potential energy diagrams...Ch. 7 - What is the first law of thermodynamics? How can a...Ch. 7 - When a gas expands, what is the sign of w? Why?...Ch. 7 - Prob. 5RQCh. 7 - High-quality audio amplifiers generate large...Ch. 7 - Explain how calorimetry works to calculate H or E...Ch. 7 - What is Hesss law? When a reaction is reversed,...Ch. 7 - Define the standard enthalpy of formation. What...Ch. 7 - Prob. 1ALQ
Ch. 7 - Prob. 2ALQCh. 7 - A fire is started in a fireplace by striking a...Ch. 7 - Liquid water turns to ice. Is this process...Ch. 7 - Prob. 5ALQCh. 7 - Prob. 6ALQCh. 7 - Consider 5.5 L of a gas at a pressure of 3.0 atm...Ch. 7 - Explain why oceanfront areas generally have...Ch. 7 - Hesss law is really just another statement of the...Ch. 7 - Prob. 10ALQCh. 7 - Prob. 11QCh. 7 - Prob. 12QCh. 7 - Assuming gasoline is pure C8H18(l), predict the...Ch. 7 - Prob. 14QCh. 7 - The enthalpy change for the reaction...Ch. 7 - For the reaction HgO(s)Hg(l)+12O2(g),H=+90.7KJ: a....Ch. 7 - Prob. 17QCh. 7 - The enthalpy change for a reaction is a state...Ch. 7 - Standard enthalpies of formation are relative...Ch. 7 - The combustion of methane can be represented as...Ch. 7 - Prob. 21QCh. 7 - Prob. 22QCh. 7 - Prob. 23QCh. 7 - Prob. 24QCh. 7 - Prob. 25ECh. 7 - Prob. 26ECh. 7 - Consider the following diagram when answering the...Ch. 7 - Consider the accompanying diagram. Ball A is...Ch. 7 - A gas absorbs 45 kJ of heat and does 29 kJ of...Ch. 7 - A system releases 125 kJ of heat while 104 kJ of...Ch. 7 - Calculate E for each of the following. a. q = 47...Ch. 7 - A system undergoes a process consisting of the...Ch. 7 - If the internal energy of a thermodynamic system...Ch. 7 - Calculate the internal energy change for each of...Ch. 7 - A sample of an ideal gas at 15.0 atm and 10.0 L is...Ch. 7 - Prob. 36ECh. 7 - Consider a mixture of air and gasoline vapor in a...Ch. 7 - As a system increases in volume, it absorbs 52.5 J...Ch. 7 - A balloon filled with 39.1 moles of helium has a...Ch. 7 - Prob. 40ECh. 7 - One of the components of polluted air is NO. It is...Ch. 7 - Prob. 42ECh. 7 - Are the following processes exothermic or...Ch. 7 - Are the following processes exothermic or...Ch. 7 - The overall reaction in a commercial heat pack can...Ch. 7 - Consider the following reaction:...Ch. 7 - Consider the combustion of propane:...Ch. 7 - Consider the following reaction:...Ch. 7 - Prob. 49ECh. 7 - The specific heat capacity of silver is 0.24 J/Cg....Ch. 7 - A 500-g sample of one of the substances listed in...Ch. 7 - Prob. 52ECh. 7 - A 30.0-g sample of water at 280. K is mixed with...Ch. 7 - A biology experiment requires the preparation of a...Ch. 7 - A 5.00-g sample of aluminum pellets (specific heat...Ch. 7 - Hydrogen gives off 120. J/g of energy when burned...Ch. 7 - Prob. 57ECh. 7 - A 110.-g sample of copper (specific heat capacity...Ch. 7 - In a coffee-cup calorimeter, 50.0 mL of 0.100 M...Ch. 7 - In a coffee-cup calorimeter, 100.0 mL of 1.0 M...Ch. 7 - A coffee-cup calorimeter initially contains 125 g...Ch. 7 - In a coffee-cup calorimeter, 1.60 g NH4NO3 is...Ch. 7 - Consider the dissolution of CaCl2:...Ch. 7 - Consider the reaction...Ch. 7 - The heat capacity of a bomb calorimeter was...Ch. 7 - The combustion of 0.1584 g benzoic acid increases...Ch. 7 - The enthalpy of combustion of solid carbon to form...Ch. 7 - Combustion reactions involve reacting a substance...Ch. 7 - Given the following data calculate H for the...Ch. 7 - Given the following data...Ch. 7 - Prob. 71ECh. 7 - Calculate H for the reaction...Ch. 7 - Given the following data...Ch. 7 - Given the following data...Ch. 7 - Give the definition of the standard enthalpy of...Ch. 7 - Write reactions for which the enthalpy change will...Ch. 7 - Prob. 77ECh. 7 - Use the values of Hf in Appendix 4 to calculate H...Ch. 7 - The Ostwald process for the commercial production...Ch. 7 - Calculate H for each of the following reactions...Ch. 7 - The reusable booster rockets of the space shuttle...Ch. 7 - The space shuttle Orbiter utilizes the oxidation...Ch. 7 - Consider the reaction...Ch. 7 - The standard enthalpy of combustion of ethene gas,...Ch. 7 - Water gas is produced from the reaction of steam...Ch. 7 - Prob. 86ECh. 7 - Prob. 87ECh. 7 - Prob. 88ECh. 7 - Some automobiles and buses have been equipped to...Ch. 7 - The complete combustion of acetylene, C2H2(g),...Ch. 7 - Prob. 91AECh. 7 - One way to lose weight is to exercise! Walking...Ch. 7 - Three gas-phase reactions were run in a...Ch. 7 - Nitrogen gas reacts with hydrogen gas to form...Ch. 7 - Combustion of table sugar produces CO2(g) and H2O(...Ch. 7 - Prob. 96AECh. 7 - Consider the following cyclic process carried out...Ch. 7 - Calculate H for the reaction...Ch. 7 - The enthalpy of neutralization for the reaction of...Ch. 7 - Prob. 100AECh. 7 - If a student performs an endothermic reaction in a...Ch. 7 - In a bomb calorimeter, the reaction vessel is...Ch. 7 - The bomb calorimeter in Exercise 102 is filled...Ch. 7 - Prob. 104AECh. 7 - Consider the following equations:...Ch. 7 - Prob. 106AECh. 7 - At 298 K, the standard enthalpies of formation for...Ch. 7 - Prob. 108AECh. 7 - A sample of nickel is heated to 99.8C and placed...Ch. 7 - Quinone is an important type of molecule that is...Ch. 7 - Calculate H for each of the following reactions,...Ch. 7 - Compare your answers from parts a and b of...Ch. 7 - Compare your answer from Exercise 72 of Chapter 3...Ch. 7 - Consider a balloon filled with helium at the...Ch. 7 - Prob. 115CWPCh. 7 - Prob. 116CWPCh. 7 - Prob. 117CWPCh. 7 - A swimming pool, 10.0 m by 4.0 m, is filled with...Ch. 7 - Prob. 119CWPCh. 7 - Calculate H for the reaction...Ch. 7 - Which of the following substances have an enthalpy...Ch. 7 - Consider 2.00 moles of an ideal gas that are taken...Ch. 7 - For the process H2O(l)H2O(g) at 298 K and 1.0 atm,...Ch. 7 - The sun supplies energy at a rate of about 1.0...Ch. 7 - Prob. 125CPCh. 7 - The standard enthalpies of formation for S(g),...Ch. 7 - Use the following standard enthalpies of formation...Ch. 7 - The standard enthalpy of formation for N2H4(g) is...Ch. 7 - The standard enthalpy of formation for NO(g) is...Ch. 7 - A piece of chocolate cake contains about 400...Ch. 7 - You have a l.00-mole sample of water at 30.C and...Ch. 7 - A 500.0-g sample of an element at 195C is dropped...Ch. 7 - A cubic piece of uranium metal (specific heat...Ch. 7 - On Easter Sunday, April 3, 1983, nitric acid...Ch. 7 - Using data from Chapter 2, calculate the change in...Ch. 7 - In Exercise 89 in Chapter 3, the Lewis structures...Ch. 7 - A gaseous hydrocarbon reacts completely with...
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- If 125 J of heat energy is applied to a block of silver weighing 29.3 g, by how many degrees will the temperature of the silver increase? (See Table 10.1.)arrow_forwardIf 14.5 kJ of heat were added to 485 g of liquid water, how much would its temperature increase?arrow_forwardThe enthalpy change when 1 mol methane (CH4) is burned is 890 kJ. It takes 44.0 kJ to vaporize 1 mol water. What mass of methane must be burned to provide the heat needed to vaporize 1.00 g water?arrow_forward
- How much heat is evolved when 1255 g of water condensesto a liquid at 100°C?arrow_forwardThe temperature of the cooling water as it leaves the hot engine of an automobile is 240 F. After it passes through the radiator it has a temperature of 175 F. Calculate the amount of heat transferred from the engine to the surroundings by one gallon of water with a specific heat of 4.184 J/g oC.arrow_forward9.45 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_forward
- What quantity of heat energy would have to be applied to a 25.1 -g block of iron in order to raise the temperature of the iron sample by 17.5 °C? (See Table 10.1.)arrow_forwardCopper is used in building the integrated circuits, chips, and printed circuit boards for computers. When 228 J of heat are absorbed by 125 g of copper at 22.38C, the temperature rises to 27.12C. What is the specific heat of copper?arrow_forwardA piece of unknown substance weighs 44.7 g and requires 2110 J to increase its temperature from 23.2 °C to 89.6 °C. (a) What is the specific heat of the substance? (b) If it is one of the substances found in Table 5.1, what is its likely identity?arrow_forward
- A 110.-g sample of copper (specific heat capacity = 0.20 J/C g) is heated to 82.4C and then placed in a container of water at 22.3C. The final temperature of the water and copper is 24.9C. What is the mass of the water in the container, assuming that all the heat lost by the copper is gained by the water?arrow_forwardThe specific heat of copper metal was determined by putting a piece of the metal weighing 35.4 g in hot water. The quantity of heat absorbed by the metal was calculated to be 47.0 J from the temperature drop of the water. What was the specific heat of the metal if the temperature of the metal rose 3.45C?arrow_forwardA piece of lead of mass 121.6 g was heated by an electrical coil. From the resistance of the coil, the current, and the Time the current flowed, it was calculated that 235 J of heat was added to the lead. The temperature of the lead rose from 20.4C to 35.5C. What is the specific heat of the lead?arrow_forward
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