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19 Nov 2019
Consider the following system at equilibrium where H° = -18.8 kJ, and Kc = 10.5, at 350 K.
2CH2Cl2(g) CH4(g) + CCl4(g)
When 0.25 moles of CH4(g) are removed from the equilibrium system at constant temperature:
the value of Kc
A. increases. B. decreases. C. remains the same.
the value of Qc
A. is greater than Kc. B. is equal to Kc. C. is less than Kc.
the reaction must:
A. run in the forward direction to reestablish equilibrium. B. run in the reverse direction to reestablish equilibrium. C. remain the same. It is already at equilibrium.
the concentration of CCl4 will:
A. increase. B. decrease. C. remain the same.
Consider the following system at equilibrium where H° = -18.8 kJ, and Kc = 10.5, at 350 K.
2CH2Cl2(g) CH4(g) + CCl4(g)
When 0.25 moles of CH4(g) are removed from the equilibrium system at constant temperature:
the value of Kc
A. increases. B. decreases. C. remains the same.
the value of Qc
A. is greater than Kc. B. is equal to Kc. C. is less than Kc.
the reaction must:
A. run in the forward direction to reestablish equilibrium. B. run in the reverse direction to reestablish equilibrium. C. remain the same. It is already at equilibrium.
the concentration of CCl4 will:
A. increase. B. decrease. C. remain the same.
Keith LeannonLv2
17 Nov 2019
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