4.000 mol chlorine and 2.000 mol bromine were placed in a 50.0 L container and kept at 293 K until equilibrium was achieved for the reaction:
Br₂(l) + Cl₂(g) ⇌ 2 BrCl(g)
At the point of equilibrium there were 82.63 g of Br₂(l) .Determine the total pressure in the 50.0 L container at equilibrium.

Question

Quizplus · Accepted Answer

To find the total pressure, first calculate the moles of Br2 at equilibrium using its mass (82.63 g) and molar mass (159.808 g/mol), which gives approximately 0.517 mol of Br2. The change in moles of Br2 from initial to equilibrium is 2.000 - 0.517 = 1.483 mol, which means 1.483 mol of Cl2 reacted, and 2 * 1.483 = 2.966 mol of BrCl was formed. The total moles of gas at equilibrium is 4.000 - 1.483 + 2.966 = 5.483 mol. Using the ideal gas law (PV=nRT) with R = 0.0821 L·atm/mol·K and T = 293 K, the total pressure is calculated as (5.483 mol * 0.0821 L·atm/mol·K * 293 K) / 50.0 L = 2.64 atm.

4000 Mol Chlorine and 2