Given the following balanced equation,determine the rate of reaction with respect to [Cl₂].If the rate of disappearance of Cl₂ is 4.24 × 10^-2 M/s,what is the rate of formation of NO? 2 NO(g)+ Cl₂(g)→ 2 NOCl(g)

Question

Quizplus · Accepted Answer

According to the balanced equation, for every 2 moles of Cl₂ reacted, 2 moles of NOCl is formed. Therefore, the rate of formation of NOCl is also 4.24 × 10^-2 M/s. Rate of formation of NO = (1/2) x Rate of formation of NOCl = (1/2) x 4.24 × 10^-2 M/s = 2.12 × 10^-2 M/s. Therefore, the best choice is D.

Given the Following Balanced Equation,determine the Rate of Reaction with Respect