(a)
Interpretation:
For the formation of
Concept introduction:
Standard free energy change:
Standard free energy change is measured by subtracting the product of temperature and standard entropy change from the standard enthalpy change of a system.
(a)
Answer to Problem 18.104QP
The value of standard enthalpy change of formation
Explanation of Solution
To calculate: The value of
The value of standard enthalpy change of formation
(b)
Interpretation:
For the formation of
Concept introduction:
Standard free energy change:
Standard free energy change is measured by subtracting the product of temperature and standard entropy change from the standard enthalpy change of a system.
(b)
Answer to Problem 18.104QP
The value of standard entropy of formation of
Explanation of Solution
To calculate: The value of standard entropy of formation of
The value of standard entropy of formation of
(c)
Interpretation:
For the formation of
Concept introduction:
Standard free energy change:
Standard free energy change is measured by subtracting the product of temperature and standard entropy change from the standard enthalpy change of a system.
(c)
Answer to Problem 18.104QP
The calculated value of
Explanation of Solution
To compare: The calculated value of
Given reaction and information
Calculate the change in enthalpy and entropy
Calculate the value of
The calculated value of
(d)
Interpretation:
For the formation of
Concept introduction:
Standard free energy change:
Standard free energy change is measured by subtracting the product of temperature and standard entropy change from the standard enthalpy change of a system.
(d)
Answer to Problem 18.104QP
The result obtained by the student is not correct because the value of
Explanation of Solution
To check: The result obtained by the student
The correct equation is given by
The equation used by the student is given below
The result obtained by the student is not correct because the value of
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Chapter 18 Solutions
General Chemistry - Standalone book (MindTap Course List)
- Consider the reaction of 2 mol H2(g) at 25C and 1 atm with 1 mol O2(g) at the same temperature and pressure to produce liquid water at these conditions. If this reaction is run in a controlled way to generate work, what is the maximum useful work that can be obtained? How much entropy is produced in this case?arrow_forwardConsider the reaction of 1 mol H2(g) at 25C and 1 atm with 1 mol Br2(l) at the same temperature and pressure to produce gaseous HBr at these conditions. If this reaction is run in a controlled way to generate work, what is the maximum useful work that can be obtained? How much entropy is produced in this case?arrow_forwardFor each of the following processes, identify the systemand the surroundings. Identify those processes that arespontaneous. For each spontaneous process, identify theconstraint that has been removed to enable the process to occur: Ammonium nitrate dissolves in water. Hydrogen and oxygen explode in a closed bomb. A rubber band is rapidly extended by a hangingweight. The gas in a chamber is slowly compressed by aweighted piston. A glass shatters on the floor.arrow_forward
- The molecular scale pictures below show snapshots of a strong acid at three different instants after it is added to water. Place the three pictures in the correct order so that they show the progress of the spontaneous process that takes place as the acid dissolves in the water. Explain your answer in terms of entropyarrow_forwardDetermine the entropy change for the combustion of gaseous propane, C3H8, under the standard conditions to give gaseous carbon dioxide and water.arrow_forwardUse the data in Appendix G to calculate the standard entropy change for H2(g) + CuO(s) H2O() + Cu(s)arrow_forward
- For each process, tell whether the entropy change of the system is positive or negative. (a) A glassblower heats glass (the system) to its softening temperature. (b) A teaspoon of sugar dissolves in a cup of coffee. (The system consists of both sugar and coffee.) (c) Calcium carbonate precipitates out of water in a cave to form stalactites and stalagmites. (Consider only the calcium carbonate to be the system.)arrow_forwardFor the reaction NO(g)+NO2(g)N2O3(g) , use tabulated thermodynamic data to calculate H and S. Then use those values to answer the following questions. (a) Is this reaction spontaneous at 25°C? Explain your answer. (b) If the reaction is not spontaneous at 25°C, will it become spontaneous at higher temperatures or lower temperatures? (c) To show that your prediction is accurate, choose a temperature that corresponds to your prediction in part (b) and calculate G . (Assume that both enthalpy and entropy are independent of temperature.)arrow_forwardDefine the following: a. spontaneous process b. entropy c. positional probability d. system e. surroundings f. universearrow_forward
- What is meant by the standard free-energy change G for a reaction? What is meant by the standard free energy of formation Gf of a substance?arrow_forwardThe decomposition of diamond to graphite [C(diamond) C(graphite)] is thermodynamically favored, but occurs slowly at room temperature. a. Use fG values from Appendix L to calculate rG and Keq for the reaction under standard conditions and 298.15 K. b. Use fH and S values from Appendix L to estimate rG and Keq for the reaction at 1000 K. Assume that enthalpy and entropy values are valid at these temperatures. Does heating shift the equilibrium toward the formation of diamond or graphite? c. Why is the formation of diamond favored at high pressures? d. The phase diagram shows that diamond is thermodynamically favored over graphite at 20,000 atmospheres pressure (about 2 GPa) at room temperature. Why is this conversion actually done at much higher temperatures and pressures?arrow_forward
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