What is rate law ? Give a relation between rate of reaction and concentration of reactants.
What is rate law ? Give a relation between rate of reaction and concentration of reactants.
Rate of reaction depends upon the experimental conditions such as concentration of reactants (pressure in case of gases), temperature and catalyst. The rate of a chemical reaction at a given temperature may depend on the concentration of one or more reactants and products.
The representation of rate of reaction in terms of concentration of the reactants is known as rate law. It is also called as rate equation or rate expression.
The rate of a reaction decreases with the passage of time as the concentration of reactants decrease. Conversely rate generally increase when reactant concentrations increase.
$\therefore$ Rate of reaction $\propto$ Concentration of reactants
So, rate of a reaction depends upon the concentration of reactants.
Similar Questions
The results given in the below table were obtained during kinetic studies of the following reaction:
$2 A + B \longrightarrow C + D$
Experiment
$[ A ] / molL ^{-1}$
$[ B ] / molL ^{-1}$
Initial $rate/molL$ $^{-1}$ $\min ^{-1}$
$I$
$0.1$
$0.1$
$6.00 \times 10^{-3}$
$II$
$0.1$
$0.2$
$2.40 \times 10^{-2}$
$III$
$0.2$
$0.1$
$1.20 \times 10^{-2}$
$IV$
$X$
$0.2$
$7.20 \times 10^{-2}$
$V$
$0.3$
$Y$
$2.88 \times 10^{-1}$
$X$ and $Y$ in the given table are respectively :
The results given in the below table were obtained during kinetic studies of the following reaction:
$2 A + B \longrightarrow C + D$
| Experiment | $[ A ] / molL ^{-1}$ | $[ B ] / molL ^{-1}$ | Initial $rate/molL$ $^{-1}$ $\min ^{-1}$ |
| $I$ | $0.1$ | $0.1$ | $6.00 \times 10^{-3}$ |
| $II$ | $0.1$ | $0.2$ | $2.40 \times 10^{-2}$ |
| $III$ | $0.2$ | $0.1$ | $1.20 \times 10^{-2}$ |
| $IV$ | $X$ | $0.2$ | $7.20 \times 10^{-2}$ |
| $V$ | $0.3$ | $Y$ | $2.88 \times 10^{-1}$ |
$X$ and $Y$ in the given table are respectively :
- [JEE MAIN 2020]
Consider the reaction, $2A + B \rightarrow$ products. When concentration of $B$ alone was doubled, the half-life did not change. When the concentration of $A$ alone was doubled, the rate increased by two times. The unit of rate constant for this reaction is
Consider the reaction, $2A + B \rightarrow$ products. When concentration of $B$ alone was doubled, the half-life did not change. When the concentration of $A$ alone was doubled, the rate increased by two times. The unit of rate constant for this reaction is
- [AIEEE 2007]
The unit of rate constant of second order reaction is usually expressed as
The unit of rate constant of second order reaction is usually expressed as
If the rate expression for a chemical reaction is given by Rate $ = k{[A]^m}{[B]^n}$
If the rate expression for a chemical reaction is given by Rate $ = k{[A]^m}{[B]^n}$
If $‘a’ $ is the initial concentration and $ ‘n’ $ is the order of the reaction and the half life period is $ ‘T’,$ then
If $‘a’ $ is the initial concentration and $ ‘n’ $ is the order of the reaction and the half life period is $ ‘T’,$ then