Question

Given the following balanced equation. Determine the rate of reaction with respect to [Cl2]. If the rate of Cl₂ loss is 4.00x 10-² M/s. What is the rate of formation of NOCl ?

2NO(g) + Cl₂(g) → 2 NCl(g)

Answer 1

The rate of formation of NOCl is twice the rate of Cl₂ loss, which is 8.00x10⁻² M/s given the rate of Cl₂ loss of 4.00x10⁻² M/s.

Step-by-step explanation:

The rate of reaction with respect to [Cl₂] is given, and we can determine the rate of formation of NOCl using the stoichiometric relationships in the balanced chemical equation:

2NO(g) + Cl₂(g) → 2NOCl(g)

Since 2 moles of NOCl are produced for every 1 mole of Cl₂ that reacts, if the rate of Cl₂ loss is 4.00x10⁻² M/s, the rate of formation of NOCl will be twice this value:

Rate of NOCl formation = 2 × (Rate of Cl₂ loss) = 2 × 4.00x10⁻² M/s = 8.00x10⁻² M/s.