Assume that the reaction: CO(g) + H2O(g) CO2(g) + H2(g) occurs in an ideal mixture of ideal gases. At 500. K, Kp = 3.11. At this temperature, ΔG° equals: A 0 kJ B -5.47 kJ C -3.74 D -7.47 kJ E -4.72 kJ

53. Please show the process of cancelling out the function of ln. thank you

For the reaction:  ½F2(g)F(g), a reaction mixture initially contains 1.5 atm of F2(g) and 1.5 atm of F(g) in their standard states. If Kp = 12 at this temperature, which statement is true?               Q < K, and the reaction proceeds towards the products.     Q > K, and the reaction proceeds towards the reactants.     Q = K, and the reaction is at equilibrium.     Q < K, and the reaction proceeds towards the reactants.

Given Consider the Kp of the reaction C(s)  + CO2(g) <=> 2CO(g), with ∆H° of the reaction is -426 kJ. What is the effect of decreasing the reaction temperature to 298 K on the amount of CO gas produced?

Consider the following reaction, the equilibrium constant for this reaction at 298 K is 0.113: 2NO2(g) ⇌ N2O4(g) A) You have a system with 5.00 atm of NO2 and 7.00 atm of N2O4 is this reaction at equilibrium? Calculate Q tosupport your answer.B) Which way will the reaction proceed to reach equilibrium? C) Using the value of K, calculate the value for ΔG°.

What is the ΔG of a reaction if ΔH is 129.2 kJ and ΔS is 324.1 J/K when the reaction takes place at 316.9 K?     102800 kJ     26.49 kJ     231.9 kJ     -102600 kJ     -129.2 kJ

7. What is ΔG° at 500.0 K for the following reaction?  You need to show your works. Zn(s) + H2O(g) →ZnO(s) + H2(g) Substance ΔH°f (kJ/mol) at 298 K S° (J/(mol∙K)) at 298 K Zn(s) 0 41.6 H2O(g) –241.8 188.7 ZnO(s) –350.5 43.7 H2(g) 0 130.6 A. 92.0 kJ B. –136.7 kJ C. –80.7 kJ D. –92.0 kJ E. 80.7 kJ

At what temperature in Kelvin does the reaction shown below reach equilibrium under standard state conditions. Report your answer to the correct sig figs. 2 NO(g) + O2(g) → 2 NO2(g) NO(g) Ozlg) NO2(g) AH°F 90.3 33.2 (kJ/mol S° 210.8 205.0 240.1 (J/K-mol) Temperature in Kelvin =

Ag(+aq) + Cl-(aq) AgCl(s) ∆H = +112 kJIf ions are colorless, and AgCl is whiteWill the reaction appear “colorless” or “white” if:a) Some of the AgCl (s) is removed?b) The pressure is decreased?c) The temperature is raised?

∆Gº for the reaction, H2(g)+Br2(g)⇄2HBr(g), is -33.3 kJ. Which statement below is true?   To make this reaction go forward, 33.3 kJ must be added.   This reaction is non-spontaneous.   This reaction is spontaneous.   This reaction cannot be at equilibrium.