For #1, I suspect they expect you to calculate dGo which you get from dGo = dHo - TdSo from tables. However, most tables have dGo already tabulated and you need not go through the dH-TdS part.
Then dGo = -RTlnK should get it.
#2.
I'll look at 2 later.
My question is ..can anyone explain how to do problem #2? I feel lost. :( And could you also explain why? Problem#1, is that a regular dG = dH - TdS problem? Then using Go = -RTlnK to find K? Im just afraid if there are other seps to it..
1. The combustion of butane has the following balanced equation:
2 C4H10(g) + 13 O2(g) ----> 8 CO2(g) + 10 H2O(l)
a) Calculate the value of dG for the combustion of C4H10(g).
b) Calculate the equilibrium constant K at 500°C for the combustion of butane.
2. The following reaction is nonspontaneous under standard conditions:
Cd(s) + Fe^2+ ---> Fe(s) + Cd^2+
a) Calculate the temperature(s) at which this reaction would be spontaneous. The dS° of this reaction is 40.0 J/K. (Use at least 3 sig figs in your calculations).
b) Calculate the concentration of Cd^2+ needed for a cell that contains 1.00 M Fe^2+ to be spontaneous.
c) Explain why a higher/lower concentration of cadmium ion makes the reaction spontaneous. Your answer should use a concept about/related to equilibrium.
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3 answers