Answer:
The Gibbs free energy is -2997.83 kJ mol-1.
Explanation:
The change in Gibbs free energy of the reaction [tex]\Delta G[/tex] can be calculated using the formula.
[tex]\Delta G = -RTlnK[/tex]
WHere R = Gas constant = 8.314KJ/Kmol
T = the temperature of the reaction in Kelvin = (37.0 + 273) = 310K
K = Raio of molar concentration of the two reactants = 1.6/0.5 = 3.2
Therefore,
[tex]\Delta G = -8.314 \times 310 \times ln (3.2) = -2997.83 kJ mol-1[/tex]
Therefore the Gibbs free energy is -2997.83 kJ mol-1.
The negative sign indicates that the reaction is spontaneous.
The ΔG for the reaction at 37° C = - 2997.83 kJ mol-1.
We can determine the value of ΔG using the formula below
ΔG = - RT*In k
where ; R ( gas constant )= 8.314K J / Kmol
T = Temperature of reaction = 37 + 273 = 310 k
K = Ratio of conc = 1.6 / 0.5 = 3.2
Insert values in equation above
∴ ΔG = - 2997.83 kJ mol-1.
Hence we can conclude that the ΔG for the reaction at 37° C = - 2997.83 kJ mol-1.
learn more : https://brainly.com/question/9179942
