Answer :
(A) The value of
is, 7.37 kJ/mol
(B) The value of
is, -4.03 kJ/mol
(C) The value of Q for the reaction is, 1.39
Explanation :
The given balanced chemical reaction is,

The expression for reaction quotient will be :
![Q=\frac{[F6P]}{[G6P]}](https://tex.z-dn.net/?f=Q%3D%5Cfrac%7B%5BF6P%5D%7D%7B%5BG6P%5D%7D)
Given:
![Q=\frac{[F6P]}{[G6P]}=10.0](https://tex.z-dn.net/?f=Q%3D%5Cfrac%7B%5BF6P%5D%7D%7B%5BG6P%5D%7D%3D10.0)
k = 0.510
First we have to calculate the
for the reaction.



<u>Part A:</u>
Now we have to calculate the value of
.
The formula used for
is:
............(1)
where,
= Gibbs free energy for the reaction = ?
= standard Gibbs free energy = 1.67 kJ/mol
R = gas constant = 
T = temperature = 298 K
Q = reaction quotient = 10.0
Now put all the given values in the above formula 1, we get:


Thus, the value of
is, 7.37 kJ/mol
<u>Part B:</u>
Now we have to calculate the value of
.
The formula used for
is:
............(1)
where,
= Gibbs free energy for the reaction = ?
= standard Gibbs free energy = 1.67 kJ/mol
R = gas constant = 
T = temperature = 298 K
Q = reaction quotient = 0.100
Now put all the given values in the above formula 1, we get:


Thus, the value of
is, -4.03 kJ/mol
<u>Part C:</u>
Now we have to calculate the value of Q.
The formula used for
is:
............(1)
where,
= Gibbs free energy for the reaction = 2.50 kJ/mol
= standard Gibbs free energy = 1.67 kJ/mol
R = gas constant = 
T = temperature = 298 K
Q = reaction quotient = ?
Now put all the given values in the above formula 1, we get:


Thus, the value of Q for the reaction is, 1.39