# Given the equation 2A(g) <-> 2B(g) + C(g). At a particular temperature, K = 1.6 ´ 104.A) If you mixed 5.0 mol B, 0.10 mol C, and 0.0010 mol A in a one-liter container, which direction would the reaction initially proceed (left or right)? B) Addition of chemical B to an equilibrium mixture of the above will cause equilibrium to proceed to...  C) At a higher temperature, K = 1.8 ´ 10–5. Placing the equilibrium mixture in an ice bath (thus lowering the temperature) will cause equilibrium to move to the left or right?  D) Raising the pressure by lowering the volume of the container will...

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Given the equation 2A(g) <-> 2B(g) + C(g). At a particular temperature, K = 1.6 ´ 104.

A) If you mixed 5.0 mol B, 0.10 mol C, and 0.0010 mol A in a one-liter container, which direction would the reaction initially proceed (left or right)?

B) Addition of chemical B to an equilibrium mixture of the above will cause equilibrium to proceed to...

C) At a higher temperature, K = 1.8 ´ 10–5. Placing the equilibrium mixture in an ice bath (thus lowering the temperature) will cause equilibrium to move to the left or right?

D) Raising the pressure by lowering the volume of the container will...

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Step 1

Part (A):

Direction of reaction proceeds initially can be determined by comparing the values of equilibrium constant(K) and reaction quotient(Q).

Step 2

Part (B):

According to Le Chatelier’s principle, increasing the concentration of product system shifts the direction of equilibrium in such a way to reverse this change. Therefore, if the concentration of B is increased, system will shift the equilibrium in the direction of left such as to increase the concentration of A . So addition of B will make the equilibrium shifts left.

Step 3

Part (C):

The value of K is very low at higher temperature. It implies that K and temperature is inversely proportional. When the reaction mixture is kept in an ice bath, temperature decreases and hence the value of K increases. It indicates that concentrati...

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### Equilibrium Concepts 