Question

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 NOCl?
A) 4.84 x 10-2 M/s.
B) 2.42 x 10-2 M/s.
C) 1.45 x 10-2 M/s.
D) 9.68 x 10-2 M/s.
E) 1.61 x 10-2 M/s.

Answer 1

Answer:

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 10-2 M/s

D) 9.68 x 10-2 M/s

E) 1.61 x 10-2 M/s

D) 9.68 x 10-2 M/s

The correct answer is A) 4.84 x 10-2 M/s.

Explanation:

This question is solved by considering the fact that

The rate of a chemical reaction amount of the reaction that is completed per unit of time. A slow reaction or one that has a low rate of reaction, undergoes a reaction whereby the reacting components or reactants combine with each other to form the products in a long duration of time while in a fast reaction or a reaction that has a high rate of reaction, the molecules combine in short time periods. Fast reactions are known in which the products are formed instantaneously while there are slow reactions that  take several years to complete.

Here we have from the chemical equation

2 NO(g) + Cl2(g) ----> 2 NOCl (g)

that is one mole of Cl2 forms two molecules of NOCl

Hence where the chemical reaction consumes 4.24 × 10-2 moles per second of Cl2 then the amount of NOCl formed = (4.24 × 10-2 ×2)M =8.48 moles of NOCl or the rate of formation of NOCl = 4.84 x 10-2 M/s.