When the concentration of A in the reaction $A + B$ $\rightleftharpoons$ $AB$ is doubled, the rate of reaction will be
When the concentration of A in the reaction $A + B$ $\rightleftharpoons$ $AB$ is doubled, the rate of reaction will be
- A
Doubled
- B
Decreased by half
- C
Unchanged
- D
Increased by four times
Similar Questions
If the concentration of the reactants is increased, the rate of reaction
If the concentration of the reactants is increased, the rate of reaction
Half life of a reaction is found to be inversely proportional to the cube of its initial concentration. The order of reaction is
Half life of a reaction is found to be inversely proportional to the cube of its initial concentration. The order of reaction is
The experimental data for reaction
$2A + B_2 \longrightarrow 2AB$
Exp.
$[A]$
$[B_2]$
Rate $(mol\,L^{-1}\,S^{-1})$
$1$
$0.50$
$0.50$
$1.6 \times {10^{ - 4}}$
$2$
$0.50$
$1.00$
$3.2 \times {10^{ - 4}}$
$3$
$1.00$
$1.00$
$3.2 \times {10^{ - 4}}$
The rate law
The experimental data for reaction
$2A + B_2 \longrightarrow 2AB$
| Exp. | $[A]$ | $[B_2]$ | Rate $(mol\,L^{-1}\,S^{-1})$ |
| $1$ | $0.50$ | $0.50$ | $1.6 \times {10^{ - 4}}$ |
| $2$ | $0.50$ | $1.00$ | $3.2 \times {10^{ - 4}}$ |
| $3$ | $1.00$ | $1.00$ | $3.2 \times {10^{ - 4}}$ |
The rate law
Which one of the following statements for the order of a reaction is incorrect?
Which one of the following statements for the order of a reaction is incorrect?
- [AIPMT 2011]
Write differential rate expression of following reaction and give its order of reaction :
$H _{2} O _{2}+ I ^{-} \rightarrow H _{2} O + IO ^{-}$
$H _{2} O _{2}+ IO ^{-} \rightarrow H _{2} O + I ^{-}+ O _{2}$
Write differential rate expression of following reaction and give its order of reaction :
$H _{2} O _{2}+ I ^{-} \rightarrow H _{2} O + IO ^{-}$
$H _{2} O _{2}+ IO ^{-} \rightarrow H _{2} O + I ^{-}+ O _{2}$