Asked by Miguel

Estimate the value of the equilibrium constant at 550 K for each of the following reactions.

1) 2CO(g) + O2(g) <==> 2CO2(g)

2) 2H2S(g) <==> 2H2(g) + S2(g)

Thanks in advance!
Answered by DrBob222
Calculate (from tables) delta Go for each reaction, then delta Go = -RT*lnK.
Answered by Miguel
Tried that...not right
Answered by DrBob222
If you didn't use 8.314 for R, post your work.
Answered by Miguel
It's apparently a different formula since the temperature is not the standard 298 K

Work for the first:

delta G is equal to -514.4 kJ

lnK = 514.4/(0.008314)(550)

lnK = 112.5

e^112.5 = 7.17*10^48 = k

- which Mastering Chemistry says is wrong

Answered by Miguel
I figured it out...

You use the formula

ln(k2/k1) = (delta H)/R * [(1/T1)-(1/T2)]

1) 5.24 * 10^44

2) 8.86 * 10^-13
Answered by Miguel
Could you try and answer my other question?

(ht tp: //ww w. jiskha. com/ display. cgi?id= 1279495858)

take spaces out
Answered by DrBob222
I don't see anything wrong with what you have done.
Answered by kaylan
where do you get the K1 from?
Answered by kaylan
can you answer it for 545 K
Answered by Edward
That formula is used to solve for delta H, not to solve for K. You have to have the 2 temperatures and equilibrium constants to solve for delta H.
Answered by Edward
I take that back. If you solve for K1 at 298 Kelvin, you can plus those values in and solve for K2, as long as you have delta H. T1 is 298 and T2 is 550.
There are no AI answers yet. The ability to request AI answers is coming soon!