For the reaction PCl3(g) + Cl2(g) PCl5(g) at a particular temperature, Kc = 32.4

Question

For the reaction PCl3(g) + Cl2(g) PCl5(g) at a particular temperature, Kc = 32.4. Suppose a system at that temperature is prepared with: [PCl5] = 0.50 M, [Cl2] = 0.4 M, and [PCl3] = 0.10 M. Which of the following is correct?

a. The reaction will proceed in the direction of forming more PCl5 and Cl2 until equilibrium is reached.

b. The reaction is at equilibrium.

c. The reaction will proceed in the direction of forming more PCl5 until equilibrium is reached.

d. The reaction will proceed in the direction of forming more PCl3 and Cl2 until equilibrium is reached.

e. None of these choices is correct.

Explanation / Answer

PCl3(g) + Cl2(g) <---------> PCl5(g) ; Kc = 32.4

Now, reaction Quotient,Kq = [PCl5]/{[PCl3]*[Cl2]} = (0.5)/{(0.4)*(0.1)} = 12.5

Since, Kq < Kc ; hence forwardward reaction will occur

Hence the correct option is :-

c. The reaction will proceed in the direction of forming more PCl5 until equilibrium is reached.

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