Equilibrium

What is the condition for a chemical system to be at equilibrium?

In the reaction N2(g) + 3H2(g) ⇌ 2NH3(g), if the concentration of NH3 is increased, what will Le Chatelier's principle predict?

For the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), the equilibrium constant Kc is expressed as:

If the equilibrium constant Kc for a reaction is much greater than 1, what does this indicate about the reaction?

Consider the reaction: H2(g) + I2(g) ⇌ 2HI(g), with Kc = 50 at a certain temperature. If initial concentrations are [H2] = 0.1 M, [I2] = 0.1 M, and [HI] = 0 M, what is the direction of the reaction?

In an exothermic reaction at equilibrium, what is the effect of increasing temperature?

The reaction 2NO2(g) ⇌ N2O4(g) has ΔH° = -57 kJ/mol. If pressure is increased, what happens to the equilibrium position?

Derive the relationship between Kp and Kc for the reaction: CO(g) + H2O(g) ⇌ CO2(g) + H2(g).

For the reaction: PCl5(g) ⇌ PCl3(g) + Cl2(g), Kc = 0.02 at 500 K. If initially only PCl5 is present at 0.1 M, what is the equilibrium concentration of PCl5? (Assume x is the amount dissociated)

Which of the following statements about the reaction quotient Q and equilibrium constant K is correct?