In a reaction, if the enthalpy change (ΔH) is -100 kJ and the entropy change (ΔS

In a reaction, if the enthalpy change (ΔH) is -100 kJ and the entropy change (ΔS) is 200 J/K, what is the Gibbs free energy change (ΔG) at 298 K?

In a reaction, if the enthalpy change (ΔH) is -100 kJ and the entropy change (ΔS) is 200 J/K, what is the Gibbs free energy change (ΔG) at 298 K?

Step 1: Identify the values given in the problem. We have ΔH = -100 kJ and ΔS = 200 J/K.
Step 2: Convert ΔS from J/K to kJ/K because ΔH is in kJ. Since 1 kJ = 1000 J, we convert 200 J/K to kJ/K: 200 J/K = 0.2 kJ/K.
Step 3: Identify the temperature (T) given in the problem, which is 298 K.
Step 4: Use the Gibbs free energy formula: ΔG = ΔH - TΔS.
Step 5: Substitute the values into the formula: ΔG = -100 kJ - (298 K * 0.2 kJ/K).
Step 6: Calculate TΔS: 298 K * 0.2 kJ/K = 59.6 kJ.
Step 7: Substitute this value back into the equation: ΔG = -100 kJ - 59.6 kJ.
Step 8: Perform the final calculation: ΔG = -100 kJ - 59.6 kJ = -159.6 kJ.

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