Question

For a specific reaction with ΔH = -111.4 kJ/mol and ΔS = -25.0 J/(mol·K), answer the following:

Determine ΔG for this reaction at 298 K (in kJ).

Answer 1

To find ΔG at 298 K for the reaction with ΔH = -111.4 kJ/mol and ΔS = -25.0 J/(mol·K), convert ΔS to kJ, plug the values into ΔG = ΔH - TΔS, and calculate to get ΔG = -103.95 kJ/mol.

Step-by-step explanation:

To calculate the change in Gibbs free energy (ΔG) at 298 K for a reaction with a given change in enthalpy (ΔH) of -111.4 kJ/mol and change in entropy (ΔS) of -25.0 J/(mol·K), we use the Gibbs free energy equation:

ΔG = ΔH - TΔS

First, we need to convert ΔS from J to kJ:

ΔS = -25.0 J/(mol·K) × (1 kJ/1000 J) = -0.025 kJ/(mol·K)

Now, plug the values into the Gibbs free energy equation:

ΔG = -111.4 kJ/mol - (298 K)(-0.025 kJ/(mol·K))

Calculate the value:

ΔG = -111.4 kJ/mol + 7.45 kJ/mol = -103.95 kJ/mol