What is the Gibbs free energy change (ΔG) at 298 K for a reaction with ΔH = -100 kJ and ΔS = -200 J/K?

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Q: What is the Gibbs free energy change (ΔG) at 298 K for a reaction with ΔH = -100 kJ and ΔS = -200 J/K?

Solution: ΔG = ΔH - TΔS = -100,000 J - 298(-200) = -100,000 J + 59,600 J = -40,400 J = -40.4 kJ.

Steps: 9

Step 1: Identify the values given in the problem. We have ΔH = -100 kJ and ΔS = -200 J/K.
Step 2: Convert ΔH from kJ to J for consistency. -100 kJ = -100,000 J.
Step 3: Identify the temperature (T) given in the problem, which is 298 K.
Step 4: Calculate TΔS. Multiply the temperature (298 K) by ΔS (-200 J/K): 298 * -200 = -59,600 J.
Step 5: Use the Gibbs free energy formula: ΔG = ΔH - TΔS.
Step 6: Substitute the values into the formula: ΔG = -100,000 J - (-59,600 J).
Step 7: Simplify the equation: ΔG = -100,000 J + 59,600 J.
Step 8: Calculate the final value: ΔG = -40,400 J.
Step 9: Convert ΔG back to kJ: -40,400 J = -40.4 kJ.