My Learning Cart

What is the Gibbs free energy change (ΔG) at 298 K for a reaction with ΔH = -100

Practice Questions

Q1
What is the Gibbs free energy change (ΔG) at 298 K for a reaction with ΔH = -100 kJ and ΔS = -200 J/K?
  1. -100 kJ
  2. -200 kJ
  3. 0 kJ
  4. 100 kJ

Questions & Step-by-Step Solutions

What is the Gibbs free energy change (ΔG) at 298 K for a reaction with ΔH = -100 kJ and ΔS = -200 J/K?
  • 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.
No concepts available.
Soulshift Feedback ×

On a scale of 0–10, how likely are you to recommend The Soulshift Academy?

Not likely Very likely