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Consider the following system at equilibrium where delta H° = 87.9 kJ/mol, and Kc = 1.20×10-2,...

Consider the following system at equilibrium where delta H° = 87.9 kJ/mol, and Kc = 1.20×10-2, at 500 K.

PCl5(g) ⇌ PCl3(g) + Cl2(g)

When 0.15 moles of PCl5(g) are removed from the equilibrium system at constant temperature:

Answer the following:

The value of Kc _________ (possible answers: increases, decreases, or remains the same)

The value of Qc _________(possible answers: is greater than, is equal to, or is less than) Kc.

The reaction must (choose a, b, or c from below)
a. run in the forward direction to restablish equilibrium.
b. run in the reverse direction to restablish equilibrium.
c. remain the same. It is already at equilibrium.



The concentration of PCl3will _________ (possible answers: increase, decrease, or remain the same.

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Answer #1

The value of Kcremains the same

The value of Qcis greater than Kc

The reaction must (b.) run in the reverse direction to restablish equilibrium.

The concentration of PCl3 will decrease

Explanation

Value of equilibrium constant Kc does not depend upon concentration of reactants and products. Value of Kc depends upon temperature.

When PCl5 is removed from the system, amount of reactants decrease. To achieve equilibrium again, system will run in reverse direction to produce PCl5 from PCl3 and Cl2

Therefore, concentration of PCl3 decreases

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