A mixture with [N_2O_4] = 0.90 and [NO_2J = 0.1M is at equilibrium at follows: N

Question

A mixture with [N_2O_4] = 0.90 and [NO_2J = 0.1M is at equilibrium at follows: N_2O_4(g) 2NO_2(g) What is the value of K_c for the reaction? The value of K_p for the following reaction equilibrium at 1.1 Times 10^-1 at 600 degree C. 2SO_3(g) 2SO_2(g) + O_2(g) What is the value of k_C for the reaction? (R = 0.08206 Latm/mol K) K_p for the following reaction equilibrium at 425.4 degree C us 54.5. H_2(g) + I_2(g) 2HI(g)g If the partial pressures in a mixture was found to be pH = 0.75 atm. pI_2 = 0.75 atm. and determine whether the mixture is at equilibrium or not. If the mixture is not at equilibrium, tell the direction of the shift, and calculate the equilibrium partial pressures of H_2, I_2- and HI. The value of K_p is 0.113 at 25 degree C for the following equilibrium If the total pressure is = 8.0 atm. what are the partial pressures of N204 and N_2O_4? Predict the effect of each of the following changes on the equilibrium increasing pressure by decreasing volume at constant temperature decreasing pressure by increasing volume at constant temperature removing some CO from the mixture increasing temperature at constant pressure adding a catalyst.

Explanation / Answer

A mixture with [N_2O_4] = 0.90 and [NO_2J = 0.1M is at equilibrium at follows: N

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