Question

The order of the reaction $2A+B+C\to Product$, is found to be $1,2$ and $0$ w.r.t. $A,B$ and $C$ respectively. If the concentration of each reactant is increased by two times, what will be the effect on the rate of the reaction?

Answer 1

Given the reaction is

$2A+B+C⟶Products$

According to question:-

Rate= $K\left[A{]}^1\right[B{]}^2[C{]}^0$ (given) $-\left(i\right)$

where, $K$=Rate constant

& [A], [B], [C] are respectively concentrations of the reactant $A,B$ & $C$.

If concentration of each reactant is increased by two times, then the new rate of reaction is given by:-

$(Rate{)}_{new}$=$K\left[2A{]}^1\right[2B{]}^2[2C{]}^0$

=$2K\left[A\right].4[B{]}^2.2^0[C{]}^0$

=$8K\left[A{]}^1\right[B{]}^2[C{]}^0$ $-\left(ii\right)$

Comparing $\left(i\right)$ and $\left(ii\right)$ we can see that the rate of the reaction is increased by $8$ times.

$\frac{\left(Rate\right)new}{Rate}=\frac{8}{1}$

$\Rightarrow (Rate{)}_{new}=8Rate$