The ∆Gº’ of hydrolysis of ATP is –35.7 kJ/mol.
=> Calculate the overall free energy change for the hydrolysis of ATP when [ATP]=3.8 mM, [ADP]=2.0 mM, and [Pi]=4.6 mM at 30 ºC
Reminder: R=8.314 J.mol-1K-1. Use 273.15 for conversion of Celsius to Kelvin.
I got -50.9 kJ/mol right ?
I agree
To calculate the overall free energy change (ΔG) for the hydrolysis of ATP, you can use the equation:
ΔG = ΔGº’ + RT ln ([ADP][Pi]/[ATP])
Given:
ΔGº’ = -35.7 kJ/mol
R = 8.314 J.mol^-1K^-1
T = 30 ºC = 30 + 273.15 = 303.15 K
[ATP] = 3.8 mM = 3.8 x 10^-3 mol/L
[ADP] = 2.0 mM = 2.0 x 10^-3 mol/L
[Pi] = 4.6 mM = 4.6 x 10^-3 mol/L
Let's substitute these values into the equation:
ΔG = -35.7 kJ/mol + (8.314 J.mol^-1K^-1) x (303.15 K) x ln [(2.0 x 10^-3) x (4.6 x 10^-3)] / (3.8 x 10^-3)
Calculating this expression will yield the overall free energy change for the hydrolysis of ATP.
To calculate the overall free energy change (∆G) for the hydrolysis of ATP, we can use the equation:
∆G = ∆Gº’ + RTln(Q)
Where:
∆G is the overall free energy change
∆Gº’ is the standard free energy change at standard conditions (-35.7 kJ/mol in this case)
R is the gas constant (8.314 J/mol·K)
T is the temperature in Kelvin
Q is the reaction quotient, which is calculated using the concentrations of the reactants and products.
Let's calculate Q first:
Q = [ADP] * [Pi] / [ATP]
Given:
[ATP] = 3.8 mM (3.8 x 10^-3 M)
[ADP] = 2.0 mM (2.0 x 10^-3 M)
[Pi] = 4.6 mM (4.6 x 10^-3 M)
Q = (2.0 x 10^-3) * (4.6 x 10^-3) / (3.8 x 10^-3)
Q = 4.6 x 10^-6 / (3.8 x 10^-3)
Q ≈ 1.211 x 10^-3
Now we can calculate ∆G using the equation provided:
∆G = -35.7 kJ/mol + (8.314 J/mol·K) * (30 + 273.15 K) * ln(1.211 x 10^-3)
∆G = -35.7 kJ/mol + (8.314 J/mol·K) * (303.15 K) * ln(1.211 x 10^-3)
∆G ≈ -35.7 kJ/mol + 2.4458 kJ/mol
∆G ≈ -33.2542 kJ/mol
Therefore, the overall free energy change for the hydrolysis of ATP is approximately -33.3 kJ/mol.
So, your calculation of -50.9 kJ/mol is incorrect.