For the reaction A + B ⇌ C + D, K_c = 0.60. Calculate the moles of B required to react with 1.8 mol of A to acquire 0.90 mol of C when the reaction is at equilibrium.

A 50.0-g sample of hydrogen fluoride, HF, is introduced to a 3.00-L vessel at 350 K. Equilibrium constant, K_c, at 350 K for the reaction 2 HF(g) ⇌ H₂(g) + F₂(g) is 2.50×10⁻². Determine the total pressure in the vessel at equilibrium.

A 1.00-L reaction vessel containing 13.9 g of P₄ was heated to 578 K. The P₄ dissociated into an equilibrium mixture of P₄ and P₂ with a 6.71 atm total pressure. 

P₄(g) ⇌ 2 P₂(g)

How many kilojoules of heat were released during the dissociation of P₄ to produce the equilibrium mixture?

At 500 K, the equilibrium constant (K_c) for the following reaction is 1.68.

N₂(g) + 2 O₂(g) → N₂O₄(g)

If the reaction is performed in a 1.00 L vessel at 500 K, how much N₂O₄ must be placed in the vessel to contain 0.178 mol of N₂ at equilibrium?

Consider the following hypothetical reaction: 

2 L(g) + M(g) ⇌ 2 N(g)         K_c = 0.85

A 1.00 L flask is charged with 1.50 mol of compound N and allowed to reach equilibrium. The equation derived from the ICE chart is a cubic equation that cannot be solved in closed form. Estimate the equilibrium concentrations of L, M, and N by plotting the cubic equation. [Note: Make sure that the value of x will produce a positive concentration.]

Consider the following reaction 375°C: SO₂(g) + Cl₂(g) ⇌ SO₂Cl₂(g), K_c = 25.9. 

In a reaction vessel, 2.50 M of SO₂(g) and 2.25 M of Cl₂(g) were mixed. Calculate the concentration of all species once equilibrium is reached at 375°C.