Question

Multiple Choice 1 point Consider the following equilibrium reaction: CO (g) + Cl$_2$(g) $\rightleftharpoons$ COCI$_2$ (g) After 45 seconds, [CO] = 0.045 M, [Cl$_2$] = 0.026 M, and [COCl$_2$] = 1.4 M. Is the reaction at equilibrium? If not, which way will the reaction proceed to reach equilibrium? Hint: K = 1.2 x 10$^3$ at 668 K The reaction will proceed to the right because Q < K. The reaction will proceed to the right because Q > K. The reaction will proceed to the left because Q < K. The reaction will is at equilibrium because Q = K. The reaction will proceed to the left because Q > K.

          Multiple Choice 1 point
Consider the following equilibrium reaction:
CO (g) + Cl$_2$(g) $\rightleftharpoons$ COCI$_2$ (g)
After 45 seconds, [CO] = 0.045 M, [Cl$_2$] = 0.026 M, and [COCl$_2$] = 1.4 M.
Is the reaction at equilibrium?
If not, which way will the reaction proceed to reach equilibrium?
Hint: K = 1.2 x 10$^3$ at 668 K
The reaction will proceed to the right because Q < K.
The reaction will proceed to the right because Q > K.
The reaction will proceed to the left because Q < K.
The reaction will is at equilibrium because Q = K.
The reaction will proceed to the left because Q > K.

Multiple Choice 1 point
Consider the following equilibrium reaction:
CO (g) + Cl2(g) ⇌ COCI2 (g)
After 45 seconds, [CO] = 0.045 M, [Cl2] = 0.026 M, and [COCl2] = 1.4 M.
Is the reaction at equilibrium?
If not, which way will the reaction proceed to reach equilibrium?
Hint: K = 1.2 x 10^3 at 668 K
The reaction will proceed to the right because Q < K.
The reaction will proceed to the right because Q > K.
The reaction will proceed to the left because Q < K.
The reaction will is at equilibrium because Q = K.
The reaction will proceed to the left because Q > K.

Added by Bradley D.

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