Problem: Given the following balanced equation, determine the rate of reaction with respect to [NOCl]. If the rate of Cl2 loss is 4.84 x 10-2 M/s, what is the rate of formation of NOCl?2 NO(g) + Cl2(g) → 2 NOCl(g)A) 4.84 x 10-2 M/sB) 2.42 x 10-2 M/sC) 1.45 x 10-1 M/sD) 9.68 x 10-2 M/sE) 1.61 x 10-2 M/s

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Given the following balanced equation, determine the rate of reaction with respect to [NOCl]. If the rate of Cl2 loss is 4.84 x 10-2 M/s, what is the rate of formation of NOCl?

2 NO(g) + Cl2(g) → 2 NOCl(g)

A) 4.84 x 10-2 M/s

B) 2.42 x 10-2 M/s

C) 1.45 x 10-1 M/s

D) 9.68 x 10-2 M/s

E) 1.61 x 10-2 M/s