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19 Nov 2019
For the reaction below predict the effect of each of the following changes on the equilibrium position. (For each change put an X in the correct column) H_2 (g) + I_2 (g) doubleheadarrow 2HI (g) Delta H = -150 kJ/mol b. Consider the following reaction at 600K: H_2 (g) I_2 doubleheadarrow (g) 2HI (g) A reaction mixture at equilibrium at 600K contains 0.170 bar H_2, 0.120 bar I_2 and 1.26 bar HI. a. Calculate the equilibrium constant (K_p) for this reaction b. A second reaction mixture, also at 600 K contains 0.135 bar of H_2, 0.135 bar I_2 and 1.10 bar of HI. Is the mixture at equilibrium? If the mixture in part b is not at equilibrium, what will be the partial pressures of H_2, I_2 and HI when the reaction mixture reaches equilibrium? d. What will be the total pressure in the flask at equilibrium?
For the reaction below predict the effect of each of the following changes on the equilibrium position. (For each change put an X in the correct column) H_2 (g) + I_2 (g) doubleheadarrow 2HI (g) Delta H = -150 kJ/mol b. Consider the following reaction at 600K: H_2 (g) I_2 doubleheadarrow (g) 2HI (g) A reaction mixture at equilibrium at 600K contains 0.170 bar H_2, 0.120 bar I_2 and 1.26 bar HI. a. Calculate the equilibrium constant (K_p) for this reaction b. A second reaction mixture, also at 600 K contains 0.135 bar of H_2, 0.135 bar I_2 and 1.10 bar of HI. Is the mixture at equilibrium? If the mixture in part b is not at equilibrium, what will be the partial pressures of H_2, I_2 and HI when the reaction mixture reaches equilibrium? d. What will be the total pressure in the flask at equilibrium?
Nestor RutherfordLv2
19 Nov 2019