Consider the following reaction where Kc-1.20x10-2 at 500 K. PClsg) Cl()+ Ch(g)

Question

Consider the following reaction where Kc-1.20x10-2 at 500 K. PClsg) Cl()+ Ch(g) A reaction mixture was found to contain 0.136 moles of PCl5(8), 5.38x102 moles of PClz(g), and 4.14x102 moles of CI20g), in a 1.00 liter container Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Qc equals The reaction A. must run in the forward direction to reach equilibrium. B. must run in the reverse direction to reach equilibrium C. is at equilibrium.

Explanation / Answer

since volume of container 1 L, concentration will be same as number of moles

Qc = [PCl3][Cl2]/[PCl5]
= (5.38*10^-2)*(4.14*10^-2)/(0.136)
= 1.64*10^-2

Since Qc is not equal to Kc, is not at equilibrium

Qc is greater than Kc, so it must proceed in backward direction
Answer: B

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