Consider the following reaction: S P. G \'° = -5,935 J/mol at 37 °C, which means

Question

Consider the following reaction: S P. G'° = -5,935 J/mol at 37 °C, which means that the K'eq = 10. The actual concentrations of S and P were measured in human liver; from these data it was calculated that G' = -10,000 J/mol. In the liver, the ratio of the actual concentration of P to the actual concentration of S must be:
(Hint for this and similar questions to follow: If G' has a negative value, the rx. tends to go to the right in order to approach equilibrium. If G' has a positive value, the rx. tends to go back to the left in order to approach equilibrium. If G' = 0, the rx. is at equilibrium. These questions are surprisingly "easy" to answer if the concept is understood.)

A

greater than 10.

B

equal to 10.

C

less than 10 and greater than 0.

D

equal to 0.

E

less than 0.

A

greater than 10.

B

equal to 10.

C

less than 10 and greater than 0.

D

equal to 0.

E

less than 0.

Explanation / Answer

(A) Greater than 10

Higher is negative value of deltaG higher is the K.

(OR)

deltaG0 = - R T lnK

lnK = 10000 / (8.314 * 298)

K = e4.04

K = 56.8

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