Final answer:
Given that the rate of Cl2 loss is 4.60 × 10^-2 M/s, and according to the balanced equation, two moles of NOCl are formed for every mole of Cl2 consumed. Thus, the rate of NOCl formation is 9.20 × 10^-2 M/s.
Step-by-step explanation:
The rate of reaction with respect to Cl2 can be determined using the balanced equation. In the equation 2NO(g) + Cl2(g) → 2NOCl(g), the stoichiometric coefficient of Cl2 is 1. Therefore, the rate of reaction with respect to Cl2 is equal to the rate of Cl2 loss, which is given as 4.60 × 10^-2 M/s.
To find the rate of formation of NOCl, we need to use the stoichiometric coefficients. From the balanced equation, we can see that 2 mol of NOCl is formed for every 1 mol of Cl2 reacted. Therefore, the rate of formation of NOCl is half the rate of Cl2 loss, which is 2.30 × 10^-2 M/s.
To explain the question: "Given the following balanced equation, determine the rate of reaction with respect to [Cl2]. If the rate of Cl2 loss is 4.60 × 10^-2 M/s, what is the rate of formation of NOCl? 2NO(g) + Cl2(g) → 2NOCl(g)", we need to use the stoichiometric coefficients from the balanced chemical equation to find the relationship between the rates of consumption and formation of the substances involved.
According to the balanced equation, for every mole of Cl2 consumed, two moles of NOCl are formed. Therefore, if the rate of Cl2 loss is 4.60 × 10^-2 M/s, the rate of NOCl formation is twice that of Cl2 loss. The rate of formation of NOCl is therefore 9.20 × 10^-2 M/s.