2. For the reaction 2SO2(g) + O2(g) →→2SO3(g), AH and AS° are both negative at 298 K, and the process is spontaneous at 298 K. Which of the following statements must also be true? A. The change in entropy is the driving force of the reaction. B. AG is positive for the reaction at 298 K. The direction of the reaction may be reversed at high temperatures. D. AG is temperature independent. E. At high temperature, AH becomes positive. AH:- AS= AG:-

2. For the reaction 2SO2(g) + O2(g) →→2SO3(g), AH and AS° are both negative at 298 K, and the process is spontaneous at 298 K. Which of the following statements must also be true? A. The change in entropy is the driving force of the reaction. B. AG is positive for the reaction at 298 K. The direction of the reaction may be reversed at high temperatures. D. AG is temperature independent. E. At high temperature, AH becomes positive. AH:- AS= AG:-

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Which substance has the higher entropy? a. a sample of pure silicon (to be used in a computer chip) or a piece of silicon containing a trace of another element such as boron or phosphorus a piece of silicon containing a trace of another element such as boron or phosphorus a sample of pure silicon b. CO2(g) at 0 °C or CO2 (g) at -50 °C O CO2 (g) at –50 °C O CO2 (g) at 0 °C c. I2 (s) or I2 (g) both at room temperature OL (g) OL (s) d. one mole of CO2(g) at 1 bar pressure or one mole of CO2(g) at 0.01 bar pressure (both at 298 K) one mole of CO2(g) at 0.01 bar pressure one mole of CO2(g) at 1 bar pressure
Sublimation is an example of a process for which a. ΔH is negative and ΔS is positive at all temperatures. b. ΔH, ΔS, and ΔG are positive at all temperatures. c. ΔH and ΔS are positive at all temperatures. d. ΔH is positive and ΔS is negative at all temperatures. e. ΔH, ΔS, and ΔG are negative at all temperatures.
3. Entropy changes: Consider samples of 1 mol of N₂(g) at 300K and 1 mol of O₂(g) at 200K. a. The same amount of heat is added to each sample and as a result the entropy of the samples are changed. The entropy of which sample will change more and why did you choose it? b. To have both samples undergo the same entropy change, would more heat need to be added to the N₂ gas or the O₂? Justify your answer. c. Calculate the change in entropy if the temperature of the N₂ is lowered from 300K to 200K. Cp,m = 29.1 J/K mol for N₂.
Which of the following statements is TRUE regarding entropy? a. The entropy of the universe decreases after the occurrence of a spontaneous change. b. The entropy of any substance at temperatures above absolute zero is positive. c. The entropy is zero for a pure, perfect crystal at 0 °C. d.It is possible to determine the standard molar entropy of substances due to the second law of thermodynamics.
In a biochemical reaction, A + B ® C with DG= 30 kJ/mol. Which of the following reactions, if any, might be effectively coupled to this reaction so that it becomes more spontaneous? I. C + D -> B + E Delta G = –40 kJ/mol II. C + D -> B + E Delta G = +40 kJ/mol
Indicate whether each process is spontaneous or nonspontaneous. a. water vapor condensing at 50 °C b. salt crystallizing from an unsaturated solution. c. a cold drink warming up in the hot sun d. carbon dioxide bubbling out of a warm soda e. salt and sand particles separating themselves in a mixture f. all the oxygen in a room condensing at one spot
2. Consider the reaction below. 4NH3(g) + 5O₂ (g) 4NO (g) + 6H₂O (g) a. Using the provided AGf values, calculate AG° for the above reaction at 25 °C. Species AG (kJ/mol) NH3) NO(g) H₂O -16.5 87.6 -228.6 b. Is the reaction spontaneous at 25 °C? c. What is the sign of the change in entropy for the reaction?
Now calculate the change in entropy (delta S) for the following reaction, using the thermodynamic tables P4 (g) + 10 Cl2 (g) → 4 PCl5 (g) a. 1412 J/K b. – 1.50 x 10^2 J/K c. – 856 J/K d. 2510 J/K e. – 113 J/K f. – 1098 J/K g. 3922 J/K h. 856 J/K i. none of these
a. H₂O b. SH- c. S²- BH3 e. NH3 14. At what temperatures will a reaction be spontaneous if A,H=+117 kJ and A,S = -35 J/K? The reaction will be spontaneous at any temperature. b. The reaction will never be spontaneous. c. Temperatures between 12.7 K and 135 K d. All temperatures above 94.1 K e. All temperatures below 94.1 K
Benzene is a liquid under standard conditions. The standard enthalpy and entropy changes for the evaporation of liquid benzene to form benzene vapor are +33.9 kJ/mol and 96.3 J/mol · K, respectively. If liquid benzene is placed in a closed container at 78.85°C, which of the following statements is true? The liquid cannot attain equilibrium with its vapor in a closed container. a. b. The liquid will evaporate completely. Liquid benzene will evaporate until the vapor pressure is 1 bar. d. Liquid benzene will not evaporate. e. Liquid and vapor-phase benzene cannot coexist at temperatures greater than or equal to 78.85°C.
The following reaction is endothermic. 2NH3(g) → N2(g) + 3H2(g) This means the reaction A. will be spontaneous at high temperatures. B. will be spontaneous at low temperatures. C. is not spontaneous at any temperature. D. is spontaneous at all temperatures.
49.For the decomposition of hydrogen peroxide to water and oxygen, H2O2(g) ⟶⟶ H2O(g) + O2(g) ΔΔH° = -106 kJ, and ΔΔS° = +0.0580 kJ/K. In what temperature range is the reaction spontaneous (ΔΔG° < 0)? A. The temperature must be greater than 1.83××103 K B. The temperature must be less than 1.83 ××103 K. C. The temperature must be between 225 K and 1.83 ××103 K. D. ΔΔG° is always less than zero. E. ΔΔG° is never less than zero.