Answer:
The value of delta G is -52.4 KJ/mol.
Explanation:
In the given question, the ATP's hydrolysis reaction is given as:
ATP (aq) + H2O (l) = ADP (aq) + HPO4^2-
The Q or the reaction quotient of the reaction will be as follows:
Q = [ADP] [HPO4^2-] / [ATP]
The delta G or the Gibb's free energy is determined by using the formula, delta Grxn = ΔG°rxn + RTlnQ
Here R is the gas constant, T is the temperature and ΔG°rxn is the Gibb's free energy.
Based on the given question, the values of [ATP] is 5.0 mM, [ADP] is 0.20 mM and [HPO4^2-] is 5.0 mM, now putting the values in the equation we get:
Q = [0.20 mM] [5.0 mM] / [5.0 mM]
= 0.20 mM or 0.20 * 10^-3 M
The temperature or T given is 37 degree C, which in Kelvin will be 273 + 37 = 310 K, the value of R will be 8.314 JK^-1mol^-1 and value of ΔG°rxn will be -30.5 kJ/mol. Now substituting the values we get,
ΔGrxn = ΔG°rxn + RTlnQ
= (-30.5kJ/mol) + (8.314 * 10^-3 kJ/K/mol) (310K) ln (0.20 * 10^-3)
= -52.4kJ/mol
