Hydrogen can be produced commercially by reforming methanol with steam, depending on the reactionCH3OH(g) + H2O (g) ---> CO2(g) + 3H2(g) a) Find the value of AH0 for this reaction using the data fromAppendix A. b) Determine the AH0 of the reaction using the data in the appendixA. c) Find the AH0 of this reaction at 100 ° C. (Assume that ASO and AH0 do not vary with temperature). Is the reaction spontaneous at 100°C? d) Find the KP value for this reaction at 100 oC.

Using the reaction and information provided below, calculate the value for AG at 15°C. The initial pressure of NO, is 0.003 atm, and the initial pressure of O, is 0.21 atm. 2 N,05 (s) 5 4 No2 (g) + 02 (g) AG;° (kJ/mol) N205 (s) 117.7 NO2 (g) 51.8 O2 (g) 0.

For reaction of A and B: A + B C , rHo = -20 kJ mol-1 and K = 50 at 25C. Calculate K at 100 C.

At -5.92 °C the pressure equilibrium constant K = 5.9 for a certain reaction. P Here are some facts about the reaction: • If the reaction is run at constant pressure, 127. kJ/mol of heat are released. • The constant pressure molar heat capacity C • The net change in moles of gases is -1. = 2.41 J mol -1. K¹. -1 р Yes. ☐ x10 Using these facts, can you calculate K at -27. °C? ○ No. If you said yes, then enter your answer at right. Round it to 2 significant digits. Р If you said no, can you at least decide whether K at -27. °C will be bigger or smaller than K, at −5.92 °C? П Yes, and K, will be р bigger. Yes, and K smaller. will be No. ☑

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