Equilibrium

Consider the following reaction:

4NH₃(g) + 5O₂(g) $$\Longleftrightarrow$$   4NO(g) + 6H₂O(g)

What is the unit of K_c for the equilibrium system?

Consider the following equilibrium:

C(s) + CO₂(g) $$\Longleftrightarrow$$   2CO(g)

The equilibrium mixture contains 0.42 mol dm^-3 of CO₂(g) and 0.82 mol dm^-3 of CO(g) at a certain temperature. What is the equilibrium constant at that temperature?

In Haber process, 0.60 mol dm^-3 of nitrogen is mixed with 1.80 mol dm^-3 of hydrogen in a sealed container at a certain temperature to give ammonia.

N₂(g) + 3H₂(g)   $$\Longleftrightarrow$$  2NH₃(g)

At equilibrium, 30% of the original nitrogen is consumed. What is the value of K_c for this reaction?

Consider the following equilibrium:

Ag⁺(aq) + Cl^-(aq) $$\Longleftrightarrow$$ AgCl(s)       K_c = 5.49 × 10⁹ mol^-2 dm⁶

If the equilibrium concentration of silver ion is 4.13 × 10^-8 mol dm^-3, what is the equilibrium concentration of chloride ion?

In a Haber Process, x mol of N₂(g) and y mol of H₂(g) are introduced into a V dm³ container and allowed to reach equilibrium. At equilibrium, 2z mol of NH₃(g) is found in the reaction mixture. What is the equilibrium constant for the reaction?

Which of the following changes will NOT alter the value of K_c of an equilibrium reaction?

(1)   Change in temperature

(2)   Change in pressure

(3)   Change in concentration

Consider the following equilibrium system at constant pressure:

2SO₂(g) + O₂(g) $$\Longleftrightarrow$$   2SO₃(g)    ΔH = -ve

Which of the following statements is/are correct?

(1)   An increase in temperature favours the backward reaction.

(2)   An increase in concentration of SO₃(g) shifts the equilibrium position to the right.

(3)   An increase in temperature lowers the value of K_c.