For the reaction ATP + H2O ⇔ ADP + phosphate, ΔG° = -30.5 kJ/mol. Very high...
For the reaction ATP + H2O ⇔ ADP + phosphate, ΔG° = -30.5 kJ/mol. Very high concentrations of ADP and phosphate (such that Q>>K) would likely have which of the following effects (explain your thinking):
a. ΔG would be less negative than ΔG°, because conditions would disfavor the formation of more ADP
b. ΔG would be more negative than ΔG°, because conditions would favor the formation of more ADP
c. ΔG° and ΔG are unrelated in this case, because conditions are non-standard
d. ΔG would be equal to ΔG°
Homework Answers
Negative value of ∆G° =-30.5 kJ/mol , indicate that reaction is spontaneous , and would favour formation of product (ADP and phosphate).
Hence, correct option is : (b) where ∆G would be more negative than ∆G°.
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For the reaction ATP + H2O ⇔ ADP + phosphate, ΔG° = -30.5
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