# Chemistry

posted by Heidi

Find the equilibrium constant for the following reaction:

D-Glucose (aq) <-> 2L (+) lactic acid (aq)

ΔG ° for D-Glucose= -914.5kJ/mol
ΔG ° for lactic acid = -538.8kJ/mol

Would I just use the ΔG° =-RTlnK?

1. Heidi

Temperature is at 25C, I forgot to add that!

2. DrBob222

Yes, but first you must find dGo for the reaction. That is dGorxn = (n*dGo products) - (n*dGo reactants). Remember to use 8.314 for R.

3. Heidi

d as in derivative? How would I factor in the 2L though? That's also throwing me off.

4. Heidi

d=difference. Wow, okay- makes more sense now.

5. Heidi

I was thinking this entire time 2L meant two liters. My professor just didn't put a space between the 2 and the L. L has nothing to do with the two, it has to do with the compound itself.

6. DrBob222

The 2 is n in the work I provided; i.e.,
dGorxn = (1*dGo products) - (2*dGo reactants. And yes, I don't know how to write a delta sign so dGo means delta Go. The capital D refers D glucose and capital L to L lactose.

7. Heidi

Thank you! I would've been able to handle this problem without any help if I had realized it 2=n instead of 2L.

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