QUESTION Recall the reaction catalyzed by phosphoglucomutase: glucose-1-phosphate <--> glucose-6-phosphate Assume that in liver cells under fed conditions, the G1P concentration = 2.5x10-2 M, and the G6P concentration = 1x10-3 M. Using the equation AG = AGO + RTIN([product)/[reactant]), calculate AG for the reaction, given that: AGO = -7.1 kJ mol1 R = 8.315x10-3 kJ mol-1 K-1 T= 310 K (37°C) In which direction will the reaction proceed spontaneously under these conditions? O +1.2 kl mol1; reverse reaction spontaneous. O -3.5 kl mol-1; forward reaction spontaneous. O -10.7 kl mol"1; forward reaction spontaneous. O -15.4 k) mol; forward reaction spontaneous.
QUESTION Recall the reaction catalyzed by phosphoglucomutase: glucose-1-phosphate <--> glucose-6-phosphate Assume that in liver cells under fed conditions, the G1P concentration = 2.5x10-2 M, and the G6P concentration = 1x10-3 M. Using the equation AG = AGO + RTIN([product)/[reactant]), calculate AG for the reaction, given that: AGO = -7.1 kJ mol1 R = 8.315x10-3 kJ mol-1 K-1 T= 310 K (37°C) In which direction will the reaction proceed spontaneously under these conditions? O +1.2 kl mol1; reverse reaction spontaneous. O -3.5 kl mol-1; forward reaction spontaneous. O -10.7 kl mol"1; forward reaction spontaneous. O -15.4 k) mol; forward reaction spontaneous.
Biochemistry
9th Edition
ISBN:9781319114671
Author:Lubert Stryer, Jeremy M. Berg, John L. Tymoczko, Gregory J. Gatto Jr.
Publisher:Lubert Stryer, Jeremy M. Berg, John L. Tymoczko, Gregory J. Gatto Jr.
Chapter1: Biochemistry: An Evolving Science
Section: Chapter Questions
Problem 1P
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![**Question 28**
Recall the reaction catalyzed by phosphoglucomutase:
\[ \text{glucose-1-phosphate} \rightleftharpoons \text{glucose-6-phosphate} \]
Assume that in liver cells under fed conditions, the G1P concentration = \(2.5 \times 10^{-2}\) M, and the G6P concentration = \(1 \times 10^{-3}\) M. Using the equation \(\Delta G = \Delta G^0 + RT \ln \left( \frac{\text{[product]}}{\text{[reactant]}} \right)\), calculate \(\Delta G\) for the reaction, given that:
\[
\Delta G^0 = -7.1 \, \text{kJ mol}^{-1}
\]
\[
R = 8.315 \times 10^{-3} \, \text{kJ mol}^{-1} \, \text{K}^{-1}
\]
\[
T = 310 \, \text{K} \, (37^\circ \text{C})
\]
In which direction will the reaction proceed spontaneously under these conditions?
- ☐ +1.2 kJ mol⁻¹; reverse reaction spontaneous.
- ☐ -3.5 kJ mol⁻¹; forward reaction spontaneous.
- ☐ -10.7 kJ mol⁻¹; forward reaction spontaneous.
- ☐ -15.4 kJ mol⁻¹; forward reaction spontaneous.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F94d9d6f7-b157-403a-851b-79bd19c538db%2F3dd1ad87-c7e4-4779-8e1a-de7dbaff3427%2Fzge6m5r_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Question 28**
Recall the reaction catalyzed by phosphoglucomutase:
\[ \text{glucose-1-phosphate} \rightleftharpoons \text{glucose-6-phosphate} \]
Assume that in liver cells under fed conditions, the G1P concentration = \(2.5 \times 10^{-2}\) M, and the G6P concentration = \(1 \times 10^{-3}\) M. Using the equation \(\Delta G = \Delta G^0 + RT \ln \left( \frac{\text{[product]}}{\text{[reactant]}} \right)\), calculate \(\Delta G\) for the reaction, given that:
\[
\Delta G^0 = -7.1 \, \text{kJ mol}^{-1}
\]
\[
R = 8.315 \times 10^{-3} \, \text{kJ mol}^{-1} \, \text{K}^{-1}
\]
\[
T = 310 \, \text{K} \, (37^\circ \text{C})
\]
In which direction will the reaction proceed spontaneously under these conditions?
- ☐ +1.2 kJ mol⁻¹; reverse reaction spontaneous.
- ☐ -3.5 kJ mol⁻¹; forward reaction spontaneous.
- ☐ -10.7 kJ mol⁻¹; forward reaction spontaneous.
- ☐ -15.4 kJ mol⁻¹; forward reaction spontaneous.
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