Given the following balanced equation, determine the rate of reaction with respect to [Cl2]. If the rate of Cl2 loss is 4.00 × 10-2 M/s, what is the rate of formation of NOCl?2 NO(g) + Cl2(g) → 2 NOCl(g)Group of answer choices1.00 × 10-1 M/s4.00 × 10-2 M/s2.00 × 10-2 M/s8.00 × 10-2 M/s7.25 × 10-2 M/s
Question
Given the following balanced equation, determine the rate of reaction with respect to [Cl2]. If the rate of Cl2 loss is 4.00 × 10-2 M/s, what is the rate of formation of NOCl?2 NO(g) + Cl2(g) → 2 NOCl(g)Group of answer choices1.00 × 10-1 M/s4.00 × 10-2 M/s2.00 × 10-2 M/s8.00 × 10-2 M/s7.25 × 10-2 M/s
Solution
The rate of reaction is determined by the stoichiometry of the balanced chemical equation. In this case, the balanced equation shows that 2 moles of NO and 1 mole of Cl2 react to form 2 moles of NOCl.
This means that the rate of loss of Cl2 is equal to the rate of formation of NOCl.
Therefore, if the rate of Cl2 loss is 4.00 × 10^-2 M/s, the rate of formation of NOCl is also 4.00 × 10^-2 M/s.
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