Chemical Forums
Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: cormbreb on May 12, 2022, 01:55:20 PM
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I'm preparing for my gen chem 2 final, and I'm unable to get in touch with anyone who normally can help me so I figured I would ask here. I'm just stuck on what to do with this.
What is the equilibrium constant for the reaction below at 298K?
The ∆G° for the reaction below is -10.36 kJ/mol.
2A (g) + 2B (g) ⇌ C (g) + 2D (g)
I keep getting an answer choice that is available but isn't correct. I got it by plugging in the info given to the ∆G° = -RT(lnK) equation and solving for K. (I'm getting 1.004 as my answer.)
I used 8.314 as my R and 298K as T.
The answer key say it's actually 65.37, but I don't know how to arrive at that value.
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Check the units of R and ΔG°.
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I finally figured it out while you were writing I think. Two key errors were made: I hadn't converted R by multiplying x 1000 and I had not switched the sign of ΔG° to a positive.
OOF. Thanks!
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R should be divided by 1000, to put it into kJ, or ΔG° can be multiplied by 1000, to put it into Joules. One way or the other, the units must match. The sign is also important, as you implied.