Equilibrium

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

Which of the following represents the expression for the equilibrium constant (Kc) for the reaction: aA + bB ⇌ cC + dD?

For the reaction N2(g) + 3H2(g) ⇌ 2NH3(g), if the equilibrium constant Kc = 4.5 × 10^−5 at a certain temperature, what does this imply about the position of equilibrium?

In the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), increasing the pressure will:

Which of the following changes will NOT affect the value of the equilibrium constant Kc?

For the reaction: PCl5(g) ⇌ PCl3(g) + Cl2(g), the equilibrium constant Kc is 0.02 at a certain temperature. If initially only PCl5 is present, which of the following statements is true at equilibrium?

The reaction 2NO2(g) ⇌ N2O4(g) is exothermic. According to Le Chatelier's principle, what happens to the equilibrium when the temperature is increased?

Given the reaction: H2(g) + I2(g) ⇌ 2HI(g) with Kc = 50 at 448 K, if initial concentrations are [H2] = 0.5 M, [I2] = 0.5 M, and [HI] = 0, what will happen initially?

For the reaction: CO(g) + 2H2(g) ⇌ CH3OH(g), if the equilibrium constant Kc = 1.5 × 10^3, what is the effect of adding more CH3OH at equilibrium?

Derive the relationship between Kp and Kc for the reaction: aA + bB ⇌ cC + dD, where gases are involved.