Given the equation 2A(g) -> 2B(g) + C(g). At a particular temperature, K = 1.6 x 10^4.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 toc. 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...

Question
Asked Feb 18, 2019

Given the equation 2A(g) -> 2B(g) + C(g). At a particular temperature, K = 1.6 x 10^4.
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...

check_circleExpert Solution
Step 1

Equilibrium reaction is the one where the rate of the forward reaction will be equal to the rate of the backward reaction.

Step 2

(a)

The given equilibrium reaction says that 2 moles of A gives 2 moles of B and 1 mole of C.  When 5.0 mol of B, 0.10 mol C, and 0.0010 mol of A is added in one liter container, the concentration of A will be lesser.  Hence, to attain equilibrium according to Le Chatelier's principle, the backward reaction will take place.  Formation of A will be favored.

Step 3

(b)

When chemical B is added to the reaction mixture in equilibrium, the direction of the reaction will shift towards left side.  In other words, the backward reaction ...

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