Consider the reaction X Y at 300 K. If H^ and K are 28.40 kJ mol ⁻¹ and 1.8 10⁻⁷ at the same temperature, then the magnitude of S^ for the reaction in J K ⁻¹ mol ⁻¹ is _______. (Nearest integer) (Given: R = 8.3 J K ⁻¹ mol ⁻¹ , 10 = 2.3 , 3

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Consider the reaction X Y at 300 K. If H^ and K are 28.40 kJ mol ⁻¹ and 1.8 10⁻⁷ at the same temperature, then the magnitude of S^ for the reaction in J K ⁻¹ mol ⁻¹ is _______. (Nearest integer) (Given: R = 8.3 J K ⁻¹ mol ⁻¹ , 10 = 2.3 , 3 = 0.48 , 2 = 0.30 )

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Correct answer: 0

The standard Gibbs free energy change is given by: G^ = -RT K = -2.3 RT K First, calculate K : K = (1.8 10⁻⁷) = (18 10⁻⁸) K = 18 - 8 = (2 3^2) - 8 K = 2 + 2 3 - 8 Substituting the given values: K = 0.30 + 2(0.48) - 8 = 0.30 + 0.96 - 8 = 1.26 - 8 = -6.74 Now, calculate G^ : G^ = -2.3 8.3 300 (-6.74) = 38599.98 J mol ⁻¹ Using the relation G^ = H^ - T S^ : 38599.98 = 28400 - 300 S^ 300 S^ = 28400 - 38599.98 = -10199.98 S^ = - 10199.98 300 -34 J K ⁻¹ mol ⁻¹ The magnitude of S^ is 34 . Answer: 34

Consider the reaction X Y at 300 K. If H^ and K are 28.40 kJ mol ⁻¹ and 1.8 10⁻⁷ at the same temperature, then the magnitude of S^ for the reaction in J K ⁻¹ mol ⁻¹ is _______. (Nearest integer) (Given: R = 8.3 J K ⁻¹ mol ⁻¹ , 10 = 2.3 , 3 = 0.48 , 2 = 0.30 )

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