Given the following balanced equation,determine the rate of reaction with respect to [Cl₂].If the rate of Cl₂ loss 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, 2 moles of NO is produced for every 1 mole of Cl₂ consumed. Therefore, the rate of formation of NO must be half of the rate of Cl₂ loss. Thus, the rate of formation of NO is 8.48 × 10^-2 M/s, which is equal to 4.24 × 2.

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