Question

Potassium chlorate, kclo3, decomposes according to the reaction: 2kclo3 → 2kcl 3o2 if the rate of decomposition of kclo3 at a certain time is determined to be 2.4 x 10-2 mol s-1, what is the rate of formation of kcl at the same time

Answer 1

$2.4 \times 10^{-2} \; \text{mol} \cdot \text{s}^{-1}$

Explanation

Referring to coefficients of $\text{KClO}_3$ and $\text{KCl}$ the equation, the decomposition of every $2$ moles of potassium chlorate would yield $2$ moles of potassium chloride. At any time in the reaction process the rate of production of $\text{KCl}$ shall equals to the rate at which $\text{KClO}_3$ is being consumed.

The question states that the reaction consumes $2.4 \times 10^{2} \; \text{mol}$ of $\text{KClO}_3$ every single second on average. One would thus expect it to produce the same amount of $\text{KCl}$ in the same period of time. $\text{KCl}$ is thus produced at a rate of $2.4 \times 10^{2} \; \text{mol} \cdot \text{s}^{-1}$