(B) The rate law for the reaction is given by: $\text{Rate} = k[HI]^n$.Using the data from the table:For experiment $1$: $8.80 \times 10^{-10} = k(0.0

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(B) The rate law for the reaction is given by: $\text{Rate} = k[HI]^n$.Using the data from the table:For experiment $1$: $8.80 \times 10^{-10} = k(0.0500)^n$ (Equation $1$)For experiment $2$: $3.52 \times 10^{-9} = k(0.1000)^n$ (Equation $2$)Dividing Equation $2$ by Equation $1$:$\frac{3.52 \times 10^{-9}}{8.80 \times 10^{-10}} = \left(\frac{0.1000}{0.0500}\right)^n$$4 = (2)^n$Since $2^2 = 4$,we find that $n = 2$.Thus,the order of the reaction with respect to $HI$ is $2.0$.

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

Medium

Consider the following gas-phase reaction.
$2HI_{(g)} \longrightarrow H_{2(g)} + I_{2(g)}$
and the following experimental data obtained at $555 \ K$. What is the order of the reaction with respect to $HI_{(g)}$?

$[HI] \ (M)$ Rate $(M \ s^{-1})$

$0.0500$ $8.80 \times 10^{-10}$

$0.1000$ $3.52 \times 10^{-9}$

$0.1500$ $7.92 \times 10^{-9}$

A
$1.0$
B
$2.0$
C
$2.5$
D
$3.0$

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Class 12

Chemistry Questions

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

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$[HI] \ (M)$	Rate $(M \ s^{-1})$
$0.0500$	$8.80 \times 10^{-10}$
$0.1000$	$3.52 \times 10^{-9}$
$0.1500$	$7.92 \times 10^{-9}$

List-$I$ (Order of Reaction)	List-$II$ (Unit of rate constant)
$A$. Zero order	$I$. $mol^{-1} L s^{-1}$
$B$. First order	$II$. $mol^{-2} L^{2} s^{-1}$
$C$. Second order	$III$. $s^{-1}$
$D$. Third order	$IV$. $mol L^{-1} s^{-1}$

Similar Questions

Why is the hydrolysis of an ester slow at the beginning and fast after some time?

An elementary reaction between $A$ and $B$ is a second order reaction. Which of the following rate equations must be correct?

Match List-$I$ with List-$II$:List-$I$ (Order of Reaction)List-$II$ (Unit of rate constant)$A$. Zero order$I$. $mol^{-1} L s^{-1}$$B$. First order$II$. $mol^{-2} L^{2} s^{-1}$$C$. Second order$III$. $s^{-1}$$D$. Third order$IV$. $mol L^{-1} s^{-1}$

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Match List-$I$ with List-$II$:
List-$I$ (Order of Reaction) List-$II$ (Unit of rate constant)
$A$. Zero order $I$. $mol^{-1} L s^{-1}$
$B$. First order $II$. $mol^{-2} L^{2} s^{-1}$
$C$. Second order $III$. $s^{-1}$
$D$. Third order $IV$. $mol L^{-1} s^{-1}$

If a reaction occurs in the following two steps:
$i) \ 2 ClO^{-} \rightarrow ClO_2^{-} + Cl^{-}$
$ii) \ ClO_2^{-} + ClO^{-} \rightarrow ClO_3^{-} + Cl^{-}$
Find the reaction intermediate.