The standard change in Gibbs free energy is ?G°\\\' = 7.53 kJ/mol. Calculate ?G

Question

The standard change in Gibbs free energy is ?G°' = 7.53 kJ/mol. Calculate ?G for this reaction at 298 K when [dihydroxyacetone phosphate] = 0.100 M and [glyceraldehyde-3-phosphate] = 0.00400 M. The constant R = 8.3145 J/(K·mol)

r the aqueous reaction CH2OH dihydroxyacetone phosphate glyceraldehyde-3-phosphate the standard change in Gibbs free energy is G°-7.53 kJ/mol. Calculate G for this reaction at 298 K when dihydroxyacetone phosphate] = 0.100 M and [glyceraldehyde-3-phosphate] = 0.00400 M. The constant R 8.3145 J/(K-mol) Number k.J/ mol

Explanation / Answer

Given:

Delta G0 = 7.53 kJ/mol = 7.53 E 3 J /mol

[dihydroxyacetone phosphate ] = 0.100 M

[ glyceraldehyde – 3- phosphate] = 0.00400 M

R = 8.314 J / ( K . mol)

We are given the general formula and we apply it for given reaction.

Delta Grxn = Delta G0 + RT ln ( [ glyceraldehyde – 3- phosphate ][dihydroxyacetone phosphate ] )

Lets plug all the given values

Delta Grxn = 7.53 E 3 + ( 8.314 x 298 x ln ( 0.00400/0.100)

Delta Grxn = -444.996 J / mol

So the delt G rxn = - 0.445 kJ /mol

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