Question

Consider the following reaction at some temperature

N₂(g) + 3 F₂(g) + 2 NF₃(g)

Initially, 8.00 mol of Ny and 8.00 mollof fy are placed in a rigid 2.00 L container, which then react to reach equilibrium. At equilibrium, the concentration of Fz is 0.500 M. Calculate the value of K, the equilibrium constant, for this reaction.

Answer 1

To calculate the equilibrium constant (K) for the given reaction, we need to determine the concentrations of the reactants and products at equilibrium and use their values in the equilibrium constant expression.

Step-by-step explanation:

The equilibrium constant (K) for the given reaction can be calculated using the concentrations of the reactants and products at equilibrium.

First, we need to determine the amount of moles of each substance at equilibrium:

Using the equation for the equilibrium constant:

K = ([NF3]2) / ([N2][F2]3)

Substituting the values into the equation:

K = (0.5002) / ((8.00 - 2x)(8.00 - 3x)3)

Solving for K will give us the equilibrium constant for the reaction.