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!
11 answers
Calculate (from tables) delta Go for each reaction, then delta Go = -RT*lnK.
Tried that...not right
If you didn't use 8.314 for R, post your work.
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
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
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
You use the formula
ln(k2/k1) = (delta H)/R * [(1/T1)-(1/T2)]
1) 5.24 * 10^44
2) 8.86 * 10^-13
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?
can you answer it for 545 K
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.
3 answers