If the equilibrium concentrations found in the reaction: 2A(g) + B(g) doublehead

Question

If the equilibrium concentrations found in the reaction: 2A(g) + B(g) doubleheadarrow 2C(g) Are [A] = 0.30 M [B] = 0.10 M and [C] = 0.20 M calculate the value of Kc. 0.23 6.7 4.4 3.3 The value of Kp for the reaction 2NO_2(g) doubleheadarrow N_2O_4(g) is 1.52 at 319K. What is the value of Kp at this temperature for the reaction N_2O_4(g) doubleheadarrow 2NO_2(g)? -1.52 5.74 times 10^-4 0.658 1.23 For the gaseous system, 2H_2S + 3O_2 doubleheadarrow 2H_2O + SO_2 how is K_p related to K_c at a given temperature? less than greater than equal to unrelated to Which change will increase the quantity of product in the following reaction? 2SO_2(g) + O_2 doubleheadarrow 2SO_3(g) delta H degree = -198kJ An increase in temperature a decrease in pressure A decrease in volume of container adding a catalyst

Explanation / Answer

14.

Kc = [products]^p / [reactants]^r

then

Kc = [C]^2 / [A]^2[B]

Kc = (0.2^2) ((0.3^2)(0.1)) = 4.44

Kc = 4.44, which favours products

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