We talked about this in class today, but I dont know how to do this one. Could someone please help me out? Thank you so much!!!

Question

Given the following balanced equation, determine the rate of reaction with respect to [NOCl]. If the rate of Cl₂ loss is 4.84 × 10²⁻ M/s, what is the rate of formation of NOCl? 2 NO(g) + Cl₂(g) → 2 NOCl(g)

Answer 1

Given the balanced equation 2 NO(g) + Cl₂(g) → 2 NOCl(g)

For every molecule of Cl₂ consumed, 2 molecules of NOCl are generated.

If the rate of Cl₂ loss is 4.84 × 10⁻² M/s, then

the rate of NOCl formation of 2 × (4.84 × 10⁻² M/s) = 9.68 × 10⁻² M/s