(B) The concentration of sucrose decreases from $0.4 \ M$ to $0.2 \ M$ in $1 \ hour$. This means the half-life $(t_{1/2})$ is $1 \ hour$.When the conc

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(B) The concentration of sucrose decreases from $0.4 \ M$ to $0.2 \ M$ in $1 \ hour$. This means the half-life $(t_{1/2})$ is $1 \ hour$.When the concentration is further reduced from $0.2 \ M$ to $0.1 \ M$,it takes another $1 \ hour$ (total $2 \ hours$).Since the half-life is independent of the initial concentration,the reaction follows first-order kinetics.Therefore,the order of the reaction is $1$.

Class 12 Chemistry Chemical Kinetics Rate law , Rate constant , Order of Reaction and Molecularity

Easy

In the presence of $HCl$,sucrose gets hydrolysed into glucose and fructose. The concentration of sucrose was found to reduce from $0.4 \ M$ to $0.2 \ M$ in $1 \ hour$ and to $0.1 \ M$ in $2 \ hours$. The order of the reaction is:

A
$0$
B
$1$
C
$2$
D
None of these

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

For the reaction $A + B \rightarrow \text{Product}$,the order with respect to $A$ is $1$ and with respect to $B$ is $1/2$. When the concentrations of both $A$ and $B$ are increased by a factor of $4$,the rate of reaction increases by a factor of .......

Medium

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The possible mechanism for the reaction $2NO + Br_2 \to 2NOBr$ is:
$NO + Br_2 \rightleftharpoons NOBr_2$ (Fast)
$NOBr_2 + NO \to 2NOBr$ (Slow)
The rate law expression is:

Medium

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For a reaction,$A + 2B \longrightarrow C$,the rate is given by $+\frac{d[C]}{dt} = k[A][B]$. Hence,the order of the reaction is:

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$A_2 + 2 \, B \to 2 \, AB$

$[A_2]$ $[B]$ $-d[A_2]/dt$

$0.1$ $0.2$ $1 \times 10^{-2} \, M \, s^{-1}$

$0.2$ $0.2$ $2 \times 10^{-2} \, M \, s^{-1}$

$0.2$ $0.4$ $8 \times 10^{-2} \, M \, s^{-1}$

The order of reaction with respect to $A_2$ and $B$ are respectively:

$[A_2]$	$[B]$	$-d[A_2]/dt$
$0.1$	$0.2$	$1 \times 10^{-2} \, M \, s^{-1}$
$0.2$	$0.2$	$2 \times 10^{-2} \, M \, s^{-1}$
$0.2$	$0.4$	$8 \times 10^{-2} \, M \, s^{-1}$

Medium

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The half-life of a reaction is found to be inversely proportional to the cube of its initial concentration. The order of the reaction is:

Easy

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In the presence of $HCl$,sucrose gets hydrolysed into glucose and fructose. The concentration of sucrose was found to reduce from $0.4 \ M$ to $0.2 \ M$ in $1 \ hour$ and to $0.1 \ M$ in $2 \ hours$. The order of the reaction is:

Similar Questions

For the reaction $A + B \rightarrow \text{Product}$,the order with respect to $A$ is $1$ and with respect to $B$ is $1/2$. When the concentrations of both $A$ and $B$ are increased by a factor of $4$,the rate of reaction increases by a factor of .......

The possible mechanism for the reaction $2NO + Br_2 \to 2NOBr$ is:$NO + Br_2 \rightleftharpoons NOBr_2$ (Fast)$NOBr_2 + NO \to 2NOBr$ (Slow)The rate law expression is:

For a reaction,$A + 2B \longrightarrow C$,the rate is given by $+\frac{d[C]}{dt} = k[A][B]$. Hence,the order of the reaction is:

$A_2 + 2 \, B \to 2 \, AB$ $[A_2]$ $[B]$ $-d[A_2]/dt$ $0.1$ $0.2$ $1 \times 10^{-2} \, M \, s^{-1}$ $0.2$ $0.2$ $2 \times 10^{-2} \, M \, s^{-1}$ $0.2$ $0.4$ $8 \times 10^{-2} \, M \, s^{-1}$ The order of reaction with respect to $A_2$ and $B$ are respectively:

The half-life of a reaction is found to be inversely proportional to the cube of its initial concentration. The order of the reaction is:

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The possible mechanism for the reaction $2NO + Br_2 \to 2NOBr$ is:
$NO + Br_2 \rightleftharpoons NOBr_2$ (Fast)
$NOBr_2 + NO \to 2NOBr$ (Slow)
The rate law expression is:

$A_2 + 2 \, B \to 2 \, AB$

$[A_2]$ $[B]$ $-d[A_2]/dt$

$0.1$ $0.2$ $1 \times 10^{-2} \, M \, s^{-1}$

$0.2$ $0.2$ $2 \times 10^{-2} \, M \, s^{-1}$

$0.2$ $0.4$ $8 \times 10^{-2} \, M \, s^{-1}$

The order of reaction with respect to $A_2$ and $B$ are respectively: