Question

Nitrogen monoxide reacts with chlorine at high temperature according to the equation, 2 NO(g) + Cl2(g) → 2 NOCl(g) In a certain reaction mixture the rate of formation of NOCl(g) was found to be 4.50 x 10‑4 mol L‑1 s‑1. What is the rate of consumption of NO(g)?

Answer 1

Answer:

4.50 × 10⁻⁴ mol L⁻¹ s⁻¹

Explanation:

Step 1: Write the balanced equation

2 NO(g) + Cl₂(g) → 2 NOCl(g)

Step 2: Establish the appropriate molar ratio

The molar ratio of NO(g) to NOCl(g) is 2:2, that is, when 2 moles of NO(g) are consumed, 2 moles of NOCl(g) are formed.

Step 3: Calculate the rate of consumption of NO(g)

The rate of formation of NOCl(g) is 4.50 × 10⁻⁴ mol L⁻¹ s⁻¹. The rate of consumption of NO(g) is:

$\frac{4.50 \times 10^{-4}molNOCl}{L.s} \times \frac{2molNO}{2molNOCl} = \frac{4.50 \times 10^{-4}molNO}{L.s}$