Question

Bromine monochloride is synthesized using the reaction Br₂(g) + Cl₂(g) ⇌ 2brcl(g). The value of Kp for the reaction is 1.1 × 10⁻⁴ at 150 K. A 203.0 L flask initially contains 1.055 kg of Br₂ and 1.065 kg of Cl₂. Calculate the mass of BrCl, in grams, that is present in the reaction mixture at equiLiBrium. Assume ideal gas behavior. Mass of Br is _______. What is the percent yield of BrCl? Percent yield is _______.

Answer 1

To calculate the equilibrium mass of BrCl, the initial moles of Br₂ and Cl₂ are determined and an ICE table is used alongside the equilibrium constant (Kp) to find the moles of BrCl at equilibrium, which is then converted to mass. The percent yield is calculated based on the actual versus theoretical yield.

Step-by-step explanation:

To find the mass of BrCl at equilibrium, we first need to calculate the initial moles of Br₂ and Cl₂ using their respective molar masses. The molar mass of Br₂ (Bromine) is approximately 159.808 g/mol (79.904 × 2) as Bromine's atomic mass is about 79.904. Similarly, the molar mass of Cl₂ (Chlorine) is about 70.906 g/mol (35.453 × 2) as Chlorine's atomic mass is 35.453.

Given the initial masses, we can calculate the initial moles of Br₂ and Cl₂:

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Under the assumption of ideal gas behavior, at equilibrium, the reaction quotient Q must equal the equilibrium constant Kp. So, we can set up an ICE table to find the equilibrium concentrations of the reactants and products.

Using the Kp given (1.1 × 10⁻⁴), we would solve for the changes in concentration (x) for each species and determine the equilibrium mole ratios. From there, we will convert the moles of BrCl back to mass using its molar mass (Bromine + Chlorine).

The percent yield of BrCl is calculated by taking the ratio of the actual amount of BrCl produced over the theoretical maximum amount possible (assuming complete reaction of the limiting reactant) and multiplying by 100%.