Question

Calculate ∆Grxn at 298 K under the conditions shown below for the following reaction. SO3(g) + H2O(g) → H2SO4(l) ∆G°= -90.5 kJ

P(SO3) = 0.20 atm, P(H2O) = 0.88 atm. Please show me as much work as possible

Answer 1

The change in the free energy of the reaction is -4.3 kJ/mol.

Understanding the thermodynamics of chemical reactions and biological processes requires an understanding of the concept of free energy change, which is essential for predicting whether a reaction will happen spontaneously and revealing the ideal circumstances for it to occur.

The change in free energy, often denoted as ΔG (delta G), is a thermodynamic concept that represents the energy available to do work in a chemical reaction.

We know that;

K = 1/(0.2) * (0.88)

K = 5.7

Then;

∆G°= - RTlnK

∆G°= -(8.314 * 298 * ln(5.7))

= -4.3 kJ/mol