Under the standard state and 260 °C, the solid of ammonia hydroxide NH4OH (s) decomposes explosively on its own into nitrous oxide gas N20 (g) and water gas H20 (g). NH4OH (s) > NH3 (g) + H20 (g) However, NH4OH (S) is stable under the standard state and 25 °C and does not decompose. Based on the above information, which of the following does have the correct signs for the AG° AS°rxn regarding the above reaction at the standard state and 260 °C. AHO rxn and rxn a. AH° XN > 0; ASOrxn < 0; AG°rxn <0 O b. AHO, rxn <0; AS°rxn < 0; AG°rxn < 0 C. AHO, rxn < 0; AS°rxn > 0; AG°rxn> 0 d. AH°rxn> 0; AS°rxn> 0; AGOrxn >0 e. AH°rxn > 0; AS°xn > 0; AG°rxn <0 O f. AH°rxn < 0; AS°rxn > 0; AG°rxn <0

Under the standard state and 260 °C, the solid of ammonia hydroxide NH4OH (s) decomposes explosively on its own into nitrous oxide gas N20 (g) and water gas H20 (g). NH4OH (s) > NH3 (g) + H20 (g) However, NH4OH (S) is stable under the standard state and 25 °C and does not decompose. Based on the above information, which of the following does have the correct signs for the AG° AS°rxn regarding the above reaction at the standard state and 260 °C. AHO rxn and rxn a. AH° XN > 0; ASOrxn < 0; AG°rxn <0 O b. AHO, rxn <0; AS°rxn < 0; AG°rxn < 0 C. AHO, rxn < 0; AS°rxn > 0; AG°rxn> 0 d. AH°rxn> 0; AS°rxn> 0; AGOrxn >0 e. AH°rxn > 0; AS°xn > 0; AG°rxn <0 O f. AH°rxn < 0; AS°rxn > 0; AG°rxn <0

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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The enthalpy change (ΔHrxn) for a certain reaction is 700.0 kJ/mol. The same reaction has an entropy change (ΔSrxn) of 120.0 J/K·mol. Determine the Kelvin temperature above which this reaction is spontaneous.
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For the reaction: 1A(g) + 4B(g) 5 2C(g) + 2D(g) where Kp = 9.483 · 103 %3D the gaseous components are added, each at a partial pressure of 1.238 atm, to a 4.101L vessel at 32.19 °C. Calculate the AG (in kJ) for this reaction under these conditions. 0°C = 273.15 K Ř = 8.314 J/K (molar Universal Gas Constant) %D The answer is given with three numbers after the decimal (do not apply significant figure rules). Example: 25.123
■ The disorder in a solid is greater than that in a liquid. ( ✓ or X ) ■ The tendency of a process to occur naturally is called equilibrium. (✓ or X ) ▪ A spontaneous change happens unidirectional or in one way. For a reverse change to occur, work always has to be done. (✓ or X) ■ For a spontaneous change to occur, time is not a factor. A spontaneous reaction can be a rapid or very slow reaction. (✓or X ) ■ If the system is not in the equilibrium, a spontaneous change is unavoidable. The change will continue until the system reaches the state of equilibrium. (✓or X ) ■ Thermal heat transfers between cold and hot reservoirs in both directions. (✓ or X ) ■ Absolute zero kelvin is attainable. (✓or X)
The chemical reaction 2A(g) + 2B(g) + C(g) → AB2(g) +AC(I) is spontaneous at 300 K and nonspontaneous at 400 K. Which statement is true regarding the reaction? The reaction is exothermic at all temperatures. The reaction is endothermic at all temperatures. The reaction is endothermic at 400 K and exothermic at 300 K. The reaction is exothermic at 400 K and endothermic at 300 K.
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9 =+ For the reaction below AG° = + 33.0 kJ, AH° = + 92.2 kJ, and AS° =+ 198.7 J/K. Estimate the temperature at which this reaction occurs. 2 NH3(g) →N2(g) + 3H2(g) A) 0.464 K B) 166 K C) 298 K D) 464 K A B C
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Which one of the following reactions cannot proceed spontaneously as written at any temperature? Assume that ΔH°rxn does not depend on temperature. A. 2Cl2O(g) → 2Cl2(g) + O2(g) ΔH°rxn = –151 kJ B. 3O2(g) → 2O3(g) ΔH°rxn = +284 kJ C. COCl2(g) → CO(g) + Cl2(g) ΔH°rxn = +112 kJ D. 2C(s) + 2S(s) + O2(g) → 2COS(g) ΔH°rxn = –137 kJ E. N2O4(g) → 2NO2(g) ΔH°rxn = +171 kJ
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AS is positive for which of the following reactions