the standard state free energy of hydrolysis of acetyl phosphat is G= -42.3 kJ/mol. Calculate the free energy change for the acetyl phosphate hydrolysis in a solution of 2mM acetate, 2 mM phospate and 3 nM acetyl phospahte.
To calculate the free energy change for the hydrolysis of acetyl phosphate in the given solution, we can use the equation:
ΔG' = ΔG° + RT * ln ([C][D]/[A][B])
where:
ΔG' is the standard state free energy change,
ΔG° is the standard state free energy of hydrolysis (-42.3 kJ/mol in this case),
R is the gas constant (8.314 J/(mol*K)),
T is the temperature in Kelvin,
ln is the natural logarithm,
[C], [D], [A], and [B] are the concentrations of the reactants and products, respectively.
We need to convert the concentration of acetyl phosphate from nM to M by dividing by 10^9 and multiply by 1000 to convert to mM:
[A] = 3 nM = 3 × 10^-9 M = 3 × 10^-6 mM
Now we can substitute the values into the equation and solve for ΔG':
ΔG' = -42.3 kJ/mol + (8.314 J/(mol*K)) * T * ln ((2 mM) * (2 mM) / (3 × 10^-6 mM) * (2 mM))
Note: The temperature (T) should be specified in Kelvin.
Please provide the temperature (T) value in Kelvin so I can complete the calculation.
To calculate the free energy change for the hydrolysis reaction of acetyl phosphate in the given solution, you need to use the equation:
ΔG = ΔG° + RTln(Q)
Here:
ΔG is the free energy change
ΔG° is the standard state free energy change (-42.3 kJ/mol)
R is the gas constant (8.314 J/(mol·K) or 0.008314 kJ/(mol·K))
T is the temperature (in Kelvin)
ln(Q) is the natural logarithm of the reaction quotient, Q
First, convert the given temperature to Kelvin if necessary.
Next, calculate the reaction quotient, Q, using the concentrations of reactants and products. The reaction is:
Acetyl Phosphate (2mM) + H2O = Acetate (2mM) + Phosphate
Q = [acetate] * [phosphate] / [acetyl phosphate]
Substitute the given concentrations into the equation and calculate Q.
Finally, substitute the values of ΔG°, R, T, and ln(Q) into the equation ΔG = ΔG° + RTln(Q) to find the free energy change, ΔG, in kJ/mol.