Imagine that inside a cell the [creatine phosphate] = 3.5 mM, [creatine] = 0.6 mM, and [Pi] = 4.3 mM. Furthermore, imagine that the pH inside the cell is 7.4. Given that ΔG°′ for creatine phosphate hydrolysis is -10.3 kcal/mol, what is the ΔG for creatine phosphate hydrolysis inside the above-described cell, which is at 37 °C? Report your answer in kcal/mol to the nearest tenths. Hint: you might wish to consult the chapter in our text that discusses thermodynamics.
Hydrolysis of creatin phosphate
Creatine phosphate + ADP + H+ Creatine + ATP : Go = -10.3 Kcal/mol
G = Go + RT ln ([products] / [reaction])
R = 1.98 x 10-3 Kcal K-1 mol-1
T = 37 + 273 = 310K
G = -10.3 + 2.303 x 1.98 x 10-3 x 310 log ([0.6] /[3.5] [4.3])
G = -7.7 Kcal/mol
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