Given the following balanced equation, determine the rate of reaction with respect to [Cl2]. If the rate of Cl2 loss is 4.44 * 10-2 M/s, what is the rate of formation of NOCl?2 NO (g) + Cl2 (g) → 2 NOCl (g) 1.11 * 10-1 M/s2.22 * 10-2 M/s8.88 * 10-2 M/s1.61 * 10-2 M/s4.44 * 10-2 M/s

8.88 x 10⁻² M/s

Explanation:

The rate of reaction for:

NO (g) + Cl₂ (g) ⇒ 2NOCl (g)

is rate = - ΔNO/Δt = - ΔCl2/Δt = 1/2 ΔNOCl/Δt

so ΔNOCl/Δt = 2 ΔCl2/Δt = 2 x 4.44 * 10⁻² M/s = 8.88 x 10⁻² M/s

In general given a reaction

aA + bB ⇒ cC + dD

rate = - 1/a ΔA/Δt = - 1/b ΔB/Δt = 1/c ΔC/Δt = 1/d ΔD/Δt