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!
can you answer it for 545 K
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
Tried that...not right
If you didn't use 8.314 for R, post your work.
Could you try and answer my other question?
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take spaces out
I don't see anything wrong with what you have done.
where do you get the K1 from?
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.
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.
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