Question

For a particular reaction, ΔH=−111. 4 kJ/mol and ΔS=−25. 0 J/(mol·K). Required: Calculate ΔG for this reaction at 298 K. (in KJ).

Answer 1

The standard free energy change (ΔG) for the reaction at 298 K is calculated using the Gibbs free energy equation ΔG = ΔH - TΔS, resulting in -103.95 kJ/mol.

Step-by-step explanation:

To calculate the standard free energy change (ΔG) for a reaction at a given temperature, you can use the Gibbs free energy equation: ΔG = ΔH - TΔS. In this equation, ΔH represents the enthalpy change, ΔS represents the entropy change, and T is the temperature in Kelvin.

For this reaction, we have been provided with ΔH = -111.4 kJ/mol and ΔS = -25.0 J/(mol·K). To find ΔG at 298 K, we will perform the following calculation:

ΔG = ΔH - TΔS
ΔG = (-111.4 kJ/mol) - (298 K) * (-25.0 J/(mol·K) * (1 kJ/1000 J))
ΔG = -111.4 kJ/mol - (298 K * -0.025 kJ/(mol·K))
ΔG = -111.4 kJ/mol + 7.45 kJ/mol
ΔG = -103.95 kJ/mol

Therefore, the standard free energy change (ΔG) for the reaction at 298 K is -103.95 kJ/mol.