Chemical Forums
Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: kassideys on March 24, 2017, 11:14:16 PM
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Im having trouble with these two problems, any help is greatly appreciated
Consider the following reaction:
C2H4(g)+H2(g)→C2H6(g)
ΔH=−137.5 kJ; ΔS=−120.5 J/K
Calculate ΔG at 25∘C and determine whether the reaction is spontaneous.
Express the free energy change in joules to four significant figures.
Here, I got 256.2 kJ but this is incorrect and I'm not sure what I did wrong after checking my work.
Question 2:
At 25 ∘C the reaction from Part A has a composition as shown in the table below.
Substance Pressure
(atm)
C2H2(g) 4.15
H2(g) 5.35
C2H6(g) 2.25×10−2
What is the free energy change, ΔG, in kilojoules for the reaction under these conditions?
Express your answer numerically in kilojoules.
I have been given T = 298 K and Delta G = -242.1kJ. And I have also been given the formula,
which is Delta G = dG + RT ln Q.
My original Delta G that I calculated was 1016 J. However, this is wrong and I'm not sure where I went wrong.
Thank you, no matter how I do both calculations I keep getting the wrong answer.
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Here, I got 256.2 kJ but this is incorrect and I'm not sure what I did wrong after checking my work.
As long as you have not shown how you arrived at the incorrect answer, we can't point you in the right direction.
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What equation are you using for Part A?