Question

For the reaction below, an analysis of an equilibrium mixture isperformed at a certain temperature.

N2(g) + 3Cl2(g) reverse reaction arrow 2NCl3(g)

It is found that [NCl3(g)] = 1.9 multiplied by 10-1M, [N2(g)] = 1.4 multiplied by 10-3M, and [Cl2(g)] = 4.3 multiplied by 10-4M. Calculate K for the reaction at thistemperature.

Answer 1

k = 3.2 x 10¹¹

Step-by-step explanation:

The equilbrium taking place is:

• N₂(g) + 3Cl₂(g) ↔ 2NCl₃(g)

And the expression for the equilbrium constant k is

• k = [NCl₃]² / ( [N₂] * [Cl₂]³)

We are given all the required data from the problem, so now we solve for k:

• k = (1.9x10⁻¹)² / ( (1.4x10⁻³) * (4.3x10⁻⁴)³ )

• k = 3.2 x 10¹¹