For the reaction CH3OH(g)←→CO(g) + 2H2(g),

Question

a. Determine ΔHo and ΔSo for the reaction at 298K
b. Determine the entropy change for the surroundings assuming that they are at 298 K. What does this result tell you?
c. Calculate ΔGo at 298 from tabulated ΔG𝑓𝑜 values. Is it consistent with your result from b?
d. Assuming that ΔHo and ΔSoremain relatively constant at different temperatures, calculate ΔGoat 28 oC and 228 oC.
e. From you answer from c, would it be wiser to conduct the experiment at higher or lower temperatures if you wished the reaction to produce hydrogen gas.
f. At what temperature is the reaction at equilibrium?

Answer 1

Long question. How much do you already know how to do? Exactly what do you not understand. Regarding a part, what keeps you from looking up the values for dHo and dSo? Same for dGo for c.

Answer 2

I pretty much understand nothing

Answer 3

That doesn't help much. We need to know what to focus on to provide the best meaningful help.

So look up the values of dHo and dSo.
dHorxn = (n*dH formation products) - (n*dHo formation reactants.
dSorxn = (n*dSo formation products) - (n*dSo formation reactants)

dSsurr = -dH/T

Look up dGo and calculate dGorxn the same way you did dHorxn and dSorxn above.

d. dG = dH - TdS

e. Use the information above.

f. Set dG = 0 and solve for T.
Post your work if you get stuck and PLEASE explain what you don't understand.