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MHT CET202620 April 2026Morning ShiftChemistryChemical EquilibriumActual

Calculate G^ for reaction, CH _ 4(g) + H _ 2(g) C ₂ H _ 6(g) ( K_p = 2 10¹⁷ , R = 8.314 JK ⁻¹ mol ⁻¹ )

Options

  1. A-64.695 kJ mol ⁻¹
  2. B-98.716 kJ mol ⁻¹
  3. C-44.08 kJ mol ⁻¹
  4. D-58.78 kJ mol ⁻¹

Correct answer

B. -98.716 kJ mol ⁻¹

Step-by-step solution

The standard Gibbs free energy change is related to the equilibrium constant by the equation: G^ = -RT K_p = -2.303 RT K_p Assuming standard temperature T = 298 K and substituting the given values: G^ = -2.303 8.314 298 (2 10¹⁷) G^ = -5705.84 ( 2 + 17 10) G^ = -5705.84 (0.3010 + 17) G^ = -5705.84 17.3010 G^ = -98716 J mol ⁻¹ G^ = -98.716 kJ mol ⁻¹ Answer: -98.716 kJ mol ⁻¹

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