Consider the following system at equilibrium where Delta HÂ° = 108 kJ, and Kc = 1.29Ã—10-2, at...

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Chemistry

Consider the following system at equilibrium where Delta HÂ° =108 kJ, and K_c =1.29Ã—10^-2, at 600K.

COCl₂(g) <--->CO(g)+Â Â Cl₂(g)Â Â

If the VOLUME of the equilibrium system issuddenlyÂ Â increased at constanttemperature:
The value of K_c A. increases.
B. decreases.
C. remains the same.
The value of Q_c A. is greater than K_c.
B. is equal to K_c.
C. is less than K_c.
The reaction must: A. run in the forward direction to reestablishequilibrium.
B. run in the reverse direction to reestablishequilibrium.
C. remain the same. It is already at equilibrium.
The number of moles ofCl₂will: A. increase.
B. decrease.
C. remain the same.

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4.4 Ratings (593 Votes)

SolutionAs ideal gas equation PVnRTSo v n where V volume of gas n no of molee of gasPpressure of gasNo of moles in reactant side 1No of moles in product side 2i option C value of Kc willremains the same as according to Le Chateilers principle See Answer

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The value of K_c		A. increases.
		B. decreases.
		C. remains the same.

The value of Q_c		A. is greater than K_c.
		B. is equal to K_c.
		C. is less than K_c.

The reaction must:		A. run in the forward direction to reestablishequilibrium.
		B. run in the reverse direction to reestablishequilibrium.
		C. remain the same. It is already at equilibrium.

The number of moles ofCl₂will:		A. increase.
		B. decrease.
		C. remain the same.