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MHT CET Medical202622 April 2026Morning ShiftChemistryThermodynamics (C)Actual

For a reaction, G ^ = -5.7 kJ mol ⁻¹ at 298 K. Calculate K. ( R = 8.314 J K ⁻¹ mol ⁻¹ )

Options

  1. A1
  2. B10
  3. C10^2
  4. D10^3

Correct answer

B. 10

Step-by-step solution

The relationship between standard Gibbs free energy change and the equilibrium constant is given by: G^ = -2.303 RT K Given: G^ = -5.7 kJ mol ⁻¹ = -5700 J mol ⁻¹ R = 8.314 J K ⁻¹ mol ⁻¹ T = 298 K Substituting the values into the equation: -5700 = -2.303 8.314 298 K -5700 = -5705.8 K K = -5700 -5705.8 1 K = 10^1 = 10 Answer: 10

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