If ΔH = 100 kJ and ΔS = 0.2 kJ/K, what is ΔG at 298 K?

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Question: If ΔH = 100 kJ and ΔS = 0.2 kJ/K, what is ΔG at 298 K?

Options:

Correct Answer: 96 kJ

Solution:

ΔG = ΔH - TΔS = 100 kJ - 298 K * 0.2 kJ/K = 100 kJ - 59.6 kJ = 40.4 kJ.

If ΔH = 100 kJ and ΔS = 0.2 kJ/K, what is ΔG at 298 K?

If ΔH = 100 kJ and ΔS = 0.2 kJ/K, what is ΔG at 298 K?

Step 1: Identify the values given in the question. We have ΔH = 100 kJ, ΔS = 0.2 kJ/K, and T = 298 K.
Step 2: Write down the formula for calculating ΔG, which is ΔG = ΔH - TΔS.
Step 3: Calculate TΔS by multiplying T (298 K) by ΔS (0.2 kJ/K). This gives us TΔS = 298 K * 0.2 kJ/K = 59.6 kJ.
Step 4: Substitute the values into the ΔG formula: ΔG = 100 kJ - 59.6 kJ.
Step 5: Perform the subtraction: 100 kJ - 59.6 kJ = 40.4 kJ.
Step 6: Conclude that ΔG = 40.4 kJ.

Gibbs Free Energy – The relationship between enthalpy (ΔH), entropy (ΔS), and temperature (T) to determine the spontaneity of a reaction using the equation ΔG = ΔH - TΔS.
Thermodynamic Variables – Understanding the significance of enthalpy, entropy, and temperature in thermodynamic calculations.