Nitrogen monoxide reacts with chlorine at high temperature, according to the equation: 2NO(g)+ Cl₂(g)$\rarr$ 2NOCl(g)In a certain reaction mixture, the rate of formation of NOCl(g)was 4.50 × 10^-⁴ mol L^-¹ s^-¹. What was the rate of consumption of NO(g)?

Question

Quizplus · Accepted Answer

From the stoichiometry of the reaction, we can see that 2 moles of NO react to form 2 moles of NOCl. Therefore, the rate of consumption of NO is half the rate of formation of NOCl, which is 4.50 × 10^-⁴ mol L^-¹ s^-¹ / 2 = 2.25 × 10^-⁴ mol L^-¹ s^-¹.

Nitrogen Monoxide Reacts with Chlorine at High Temperature, According to the Equation