Calculate Kp at 298.15 Kfor the reactions (a), (b), and (c) using AG°f values. Substance AG°F (kJ/mol) NO 86.6 NO2 N20 51.3 104.2 (a) 2NO(g) +0,(g) 2NO, (g

Consider the reaction NH4+(aq) H+(aq)+NH3(aq) Use G f for NH3(aq) at 25C=26.7 kJ/mol and the appropriate tables to calculate (a) G at 25C (b) Ka at 25C

Consider the decomposition of red mercury(II) oxide under standard state conditions.. 2HgO(s,red)2Hg(l)+O2(g) (a) Is the decomposition spontaneous under standard state conditions? (b) Above what temperature does the reaction become spontaneous?

Calculate G at 355 K for each of the reactions in Question 17. State whether the reactions are spontaneous.

Calculate K at 25°C for each of the reactions referred to in Question 32. Assume smallest whole-number coefficients.

For the system 2SO3(g)2SO2(g)+O2(g) K=1.32 at 627. What is the equilibrium constant at 555C?

Consider the reaction CO(g)+H2O(g)CO2(g)+H2(g) Use the appropriate tables to calculate (a) G at 552C (b) K at 552C

For the reaction 2Cu(s)+S(s)Cu2S(s) H and G are negative and S is positive. a At equilibrium, will reactants or products predominate? Why? b Why must the reaction system be heated in order to produce copper(I) sulfide?

The free energy change, G, for a process at constant temperature and pressure is related to Suniv and reflects the spontaneity of the process. How is G related to Suniv? When is a process spontaneous? Nonspontaneous? At equilibrium? G is a composite term composed of H, T, and S. What is the G equation? Give the four possible sign combinations for H and S. What temperatures are required for each sign combination to yield a spontaneous process? If G is positive, what does it say about the reverse process? How does the G = H TS equation reduce when at the melting-point temperature of a solid-to-liquid phase change or at the boiling-point temperature of a liquid-to-gas phase change? What is the sign of G for the solid-to-liquid phase change at temperatures above the freezing point? What is the sign of G for the liquid-to-gas phase change at temperatures below the boiling point?

Given the following data at a certain temperature, 2N2(g)+O2(g)2N2O(g)K=1.2 10 35 N2O4(g)2NO2(g)K=4.6 10 3 12 N2(g)+O2(g)NO2(g)K=4.1 10 9 calculate K for the reaction between one mole of dinitrogen oxide gas and oxygen gas to give dinitrogen tetroxide gas.