[melodia]

Hi I've been working on a few different thermochemistry questions in preparation for my finals next week. I was wondering if anyone could shed light on this problem for me:

Calculate the ∆G for the reaction:

H20 (l) ⇋ H+ (aq) +OH- (aq)

at 25 degree C under the following condition:

[H+]=1.0X10^-7 M
[OH-]=1.0X10^-7 M

I used the formula ∆G=-RT*ln(k)

kc being 1.0X10^-14
and got 79907.68671 KJ/mol

The answer in the textbook said the ∆G should equal 0 KJ/mol.

is my kc incorrect?

[melodia]

whoops i ment to type my answer in joules not KJ. It should say 79907 J.