The kinetic datas for the reaction - 2A - B2- 2AB are as given below- -A- mol L-1 -B2- mol L-1Rate mol L-2min-1 2 1-0 2-5- 10-3 1-0 1-0 2-5- 10-3 2 2-0 1- 10-2Hence the order of reaction w-r-t A and B2 are respectively-

The correct option is D 0 and 2 No Dependence on #160; [A]→ϑ∝ [A]^0 #160;Quadratic Dependence on #160; #160; [B]→ϑ∝ [B]^2 #160; ...

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Standard XII

Chemistry

Reaction Quotient

The kinetic d...

Question

The kinetic datas for the reaction : $2 A + B_{2} \to 2 A B$ are as given below:
$[A]$
$m o l L^{- 1}$ $[B_{2}]$
$m o l L^{- 1}$ Rate
$m o l L^{- 2} m i n^{- 1}$
$2$ $1.0$ $2.5 \times 10^{- 3}$
$1.0$ $1.0$ $2.5 \times 10^{- 3}$
$2$ $2.0$ $1 \times 10^{- 2}$
Hence the order of reaction w.r.t $A$ and $B_{2}$ are _____ respectively.

0

and

2

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2

and

1

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1

and

2

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2

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Solution

The correct option is D $0$ and $2$
No Dependence on $[A] \to ϑ \propto [A]^{0}$
Quadratic Dependence on $[B] \to ϑ \propto [B]^{2}$
$ϑ = k [A]^{0} [B]^{2} = k [B]^{2}$

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Similar questions

Q. The kinetic datas for the reaction:

2 A + B_{2} \to 2 A B

are as given below:

$[A] m o l L^{- 1}$	$[B_{2}] m o l L^{- 1}$	Rate mol $L^{- 1} m i n^{- 1}$
0.5	1.0	$2.5 \times 10^{- 3}$
1.0	1.0	$5.0 \times 10^{- 3}$
0.5	2.0	$1 \times 10^{- 2}$

Hence the order of reaction with respect to A and

B_{2}

are, respectively:

The kinetic datas for the reaction :

2 A + B_{2} \to 2 A B

arre as given below:

\begin{matrix} [A] (m o l L^{- 1}) & [B_{2}] (m o l L^{- 1}) & R a t e (m o l L^{- 1} m i n^{- 1}) 0.5 & 1.0 & 2.5 \times 10^{- 3} 1.0 & 1.0 & 5.0 \times 10^{- 3} 0.5 & 2.0 & 1 \times 10^{- 2} \end{matrix}

Hence the order of reaction with respect to

A

and

B_{2}

are respectively :

Q. Following data are given for the reaction between

A

and

B

$[A] / m o l L^{- 1}$	$[B] / m o l L^{- 1}$	Initial rate/ $m o l L^{- 1} s^{- 1}$ at $300 K$	$320 K$
$2.5 \times 10^{- 4}$	$3.0 \times 10^{- 5}$	$5.0 \times 10^{- 4}$	$2.0 \times 10^{- 3}$
$5.0 \times 10^{- 4}$	$6.0 \times 10^{- 5}$	$4.0 \times 10^{- 3}$	-
$1.0 \times 10^{- 3}$	$6.0 \times 10^{- 5}$	$1.6 \times 10^{- 2}$	-

The rate constant at

300 K

is:

Q. For the reaction,

2 N O + 2 H_{2} \to N_{2} + 2 H_{2} O

, the following kinetic data were obtained:

Expt. No.	$[H_{2}]$ $(m o l L^{- 1})$	$[N O]$ $(m o l L^{- 1})$	Rate of reaction $(m o l L^{- 1} s^{- 1})$
$1.$	$0.12$	$0.12$	$0.25 \times 10^{- 4}$
$2.$	$0.12$	$0.24$	$1.0 \times 10^{- 4}$
$3.$	$0.24$	$0.24$	$2.0 \times 10^{- 4}$

Determine the rate law and the rate constant.

Q. The experimental data for the reaction

2 A + B_{2} ⟶ 2 A B

, is:

Expt. No.	$[A]$	$[B_{2}]$	Rate $(m o l L^{- 1} s^{- 1})$
$1.$	$0.50$	$0.50$	$1.6 \times 10^{- 4}$
$2.$	$0.50$	$1.00$	$3.2 \times 10^{- 4}$
$3.$	$1.0$	$1.00$	$3.2 \times 10^{- 4}$

The rate equation for the above data is:

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$[A]$ $m o l L^{- 1}$	$[B_{2}]$ $m o l L^{- 1}$	Rate $m o l L^{- 2} m i n^{- 1}$
$2$	$1.0$	$2.5 \times 10^{- 3}$
$1.0$	$1.0$	$2.5 \times 10^{- 3}$
$2$	$2.0$	$1 \times 10^{- 2}$

The kinetic datas for the reaction : 2A+B2→2AB are as given below:[A]molL−1[B2]mol L−1Ratemol L−2min−121.02.5×10−31.01.02.5×10−322.01×10−2Hence the order of reaction w.r.t A and B2 are _____ respectively.

The correct option is D 0 and 2No Dependence on [A]→ϑ∝[A]0 Quadratic Dependence on [B]→ϑ∝[B]2 ϑ=k[A]0[B]2=k[B]2

The correct option is D $0$ and $2$
No Dependence on $[A] \to ϑ \propto [A]^{0}$
Quadratic Dependence on $[B] \to ϑ \propto [B]^{2}$
$ϑ = k [A]^{0} [B]^{2} = k [B]^{2}$