Question

At a certain temperature, the equilibrium constant K for the following reaction is 1.48 × 10⁻⁵ :Br₂(g) + OCI₂(g) = BrOCI(g) + BrCI(g)

Suppose a 13. L reaction vessel is filled with 1.6 mof of Br₂ and 1.6 mol of OCl₂. what the composition of the micture in the vessel at equilibrium?
a. There will be very little Br₂ and OCl₂ Br2 and 1.6 mol of oCl2.
b. There will be very little BroCl and BrcI.
c. Neither of the above is true.

Answer 1

The correct answer is option b. At equilibrium, the composition of the mixture in the reaction vessel will be a mixture of BrOCI and BrCl, with very little Br₂ and OCl₂ remaining.

Step-by-step explanation:

Based on the given information, the equilibrium constant (K) for the reaction Br₂(g) + OCl₂(g) = BrOCI(g) + BrCl(g) is 1.48 x 10⁻⁵ at a certain temperature. The reaction vessel has a volume of 13.0 L and initially contains 1.6 mol of Br₂ and 1.6 mol of OCl₂. To determine the composition of the mixture at equilibrium, we need to compare the initial moles of each reactant and product with the stoichiometric coefficients of the balanced equation.

Since the reaction coefficients are both 1, the moles of BrOCI and BrCl produced will be equal to the moles of Br₂ and OCl₂ used, respectively. Since the volume of the reaction vessel is constant, the concentrations of the reactants and products can be calculated by dividing the number of moles by the volume.

Therefore, at equilibrium, the composition of the mixture in the vessel will be a mixture of BrOCI and BrCl, with very little Br₂ and OCl₂ remaining. Hence, the correct option is b. There will be very little BrOCI and BrCl.