Find the appropriate equilibrium constant (K_P) for the reaction below under the

Question

Find the appropriate equilibrium constant (K_P) for the reaction below under the following conditions. 1/2 SnO_2 (s) + H_2 (g) irreversible H_2O (g) + 1/2 Sn (s) At 650 degree C the equilibrium steam-H_2 mixture was 38% H_2 by volume. At 800 degree C the equilibrium steam-H_2 mixture was 22% H_2 by volume. Would you run this reaction at high or low temperature for the most efficient reduction of Tin (IV)? At 35 degree C, K_C = 1.6 times 10^-5 for the reaction 2 NOCl(g) reversiblearrow 2 NO(g) + Cl_2(g) Calculate the concentrations of all species at equilibrium for each of the following original mixtures 1.0 mole NOCl in a 1.0 L container. 1.00 mol NO and 0.50 mol Cl_2 in a 1.0 L container. 1.00 mol NO and 0.75 mol Cl_2 in a 1.0 L container.

Explanation / Answer

For the reaction

1/2SnO2(s) + H2 (g) <------> H2O (g) + 1/2Sn (l)

Calculate KP

(a) At 6500C, where the equilibrium steam-hydrogen mixture was 38% H2 by volume

Mixture has 38 % by Volume of H2 %

  Volume of H2O = 100 % - 38 % = 62 %

Partial Volume Ratio = Partial Pressure Ratio

KP = [P-H2O] ^2 / [P-H2] ^2

= [62]^2 / [ 38 ]^2

= 2.66

(b) At 8000C, where the equilibrium steam-hydrogen mixture was 22% H2 by volume

Mixture has 22 % by Volume of H2 %

So, volume of H2O = 100 % - 22 % = 78 %

Partial Volume Ratio = Partial Pressure Ratio

Kp = [P-H2O]^2 / [ P-H2 ]^2

= [78]^2 / [ 22 ]^2

= 12.57

(c) I would recommend higher temperature for more efficient reduction of tin (iv).

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