(C) The rate law for the reaction is given by $\text{Rate} = k[A][B]^2$. Given values are: $k = 5.0 \times 10^{-6} \ mol^{-2} \ L^2 \ s^{-1}$ $[A] = 0

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$2.50 \times 10^{-9} \ mol \ L^{-1} \ s^{-1}$

(C) The rate law for the reaction is given by $\text{Rate} = k[A][B]^2$. Given values are: $k = 5.0 \times 10^{-6} \ mol^{-2} \ L^2 \ s^{-1}$ $[A] = 0.05 \ mol \ L^{-1} = 5 \times 10^{-2} \ mol \ L^{-1}$ $[B] = 0.1 \ mol \ L^{-1} = 1 \times 10^{-1} \ mol \ L^{-1}$ Substituting these values into the rate equation: $\text{Rate} = (5.0 \times 10^{-6}) \times (0.05) \times (0.1)^2$ $\text{Rate} = 5.0 \times 10^{-6} \times 5 \times 10^{-2} \times 1 \times 10^{-2}$ $\text{Rate} = 25 \times 10^{-10} \ mol \ L^{-1} \ s^{-1}$ $\text{Rate} = 2.50 \times 10^{-9} \ mol \ L^{-1} \ s^{-1}$

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

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The rate equation for the reaction $2 A + B \longrightarrow$ products is $\text{rate} = k[A][B]^2$. If $k$ at $T \ K$ is $5.0 \times 10^{-6} \ mol^{-2} \ L^2 \ s^{-1}$,the initial rate of the reaction,when $[A] = 0.05 \ mol \ L^{-1}$ and $[B] = 0.1 \ mol \ L^{-1}$ is:

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A
$1.25 \times 10^{-9} \ mol \ L^{-1} \ s^{-1}$
B
$1.25 \times 10^{-9} \ mol \ L^{-1} \ s^{-1}$
C
$2.50 \times 10^{-9} \ mol \ L^{-1} \ s^{-1}$
D
$2.50 \times 10^{-9} \ mol \ L^{-1} \ s^{-1}$

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

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Select the rate law that corresponds to the data shown for the following reaction $A + B \to C$

$Expt. \ No.$ $[A]$ $[B]$ $Initial \ Rate$

$1$ $0.012$ $0.035$ $0.10$

$2$ $0.024$ $0.070$ $0.80$

$3$ $0.024$ $0.035$ $0.10$

$4$ $0.012$ $0.070$ $0.80$

$Expt. \ No.$	$[A]$	$[B]$	$Initial \ Rate$
$1$	$0.012$	$0.035$	$0.10$
$2$	$0.024$	$0.070$	$0.80$
$3$	$0.024$	$0.035$	$0.10$
$4$	$0.012$	$0.070$	$0.80$

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The rate of a certain reaction is given by, $Rate = k[H^{+}]^n$. The rate increases $100$ times when the $pH$ changes from $3$ to $1$. The order $(n)$ of the reaction is:

EasyWBJEE 2014

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The reaction,$X + 2Y + Z \to N$ occurs by the following mechanism:
$(i)$ $X + Y \rightleftharpoons M$ (very rapid equilibrium)
$(ii)$ $M + Z \to P$ (slow)
$(iii)$ $P + Y \to N$ (very fast)
What is the rate law for this reaction?

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By “the overall order of a reaction”,we mean

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Mechanism of a hypothetical reaction $X_2 + Y_2 \rightarrow 2XY$ is given below:
$(i)$ $X_2 \rightarrow X + X$ (fast)
$(ii)$ $X + Y_2 \rightleftharpoons XY + Y$ (slow)
$(iii)$ $X + Y \rightarrow XY$ (fast)
The overall order of the reaction will be

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The rate equation for the reaction $2 A + B \longrightarrow$ products is $\text{rate} = k[A][B]^2$. If $k$ at $T \ K$ is $5.0 \times 10^{-6} \ mol^{-2} \ L^2 \ s^{-1}$,the initial rate of the reaction,when $[A] = 0.05 \ mol \ L^{-1}$ and $[B] = 0.1 \ mol \ L^{-1}$ is:

Similar Questions

Select the rate law that corresponds to the data shown for the following reaction $A + B \to C$ $Expt. \ No.$ $[A]$ $[B]$ $Initial \ Rate$ $1$ $0.012$ $0.035$ $0.10$ $2$ $0.024$ $0.070$ $0.80$ $3$ $0.024$ $0.035$ $0.10$ $4$ $0.012$ $0.070$ $0.80$

The rate of a certain reaction is given by, $Rate = k[H^{+}]^n$. The rate increases $100$ times when the $pH$ changes from $3$ to $1$. The order $(n)$ of the reaction is:

The reaction,$X + 2Y + Z \to N$ occurs by the following mechanism:$(i)$ $X + Y \rightleftharpoons M$ (very rapid equilibrium)$(ii)$ $M + Z \to P$ (slow)$(iii)$ $P + Y \to N$ (very fast)What is the rate law for this reaction?

By “the overall order of a reaction”,we mean

Mechanism of a hypothetical reaction $X_2 + Y_2 \rightarrow 2XY$ is given below: $(i)$ $X_2 \rightarrow X + X$ (fast) $(ii)$ $X + Y_2 \rightleftharpoons XY + Y$ (slow) $(iii)$ $X + Y \rightarrow XY$ (fast) The overall order of the reaction will be

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Select the rate law that corresponds to the data shown for the following reaction $A + B \to C$

$Expt. \ No.$ $[A]$ $[B]$ $Initial \ Rate$

$1$ $0.012$ $0.035$ $0.10$

$2$ $0.024$ $0.070$ $0.80$

$3$ $0.024$ $0.035$ $0.10$

$4$ $0.012$ $0.070$ $0.80$

The reaction,$X + 2Y + Z \to N$ occurs by the following mechanism:
$(i)$ $X + Y \rightleftharpoons M$ (very rapid equilibrium)
$(ii)$ $M + Z \to P$ (slow)
$(iii)$ $P + Y \to N$ (very fast)
What is the rate law for this reaction?

Mechanism of a hypothetical reaction $X_2 + Y_2 \rightarrow 2XY$ is given below:
$(i)$ $X_2 \rightarrow X + X$ (fast)
$(ii)$ $X + Y_2 \rightleftharpoons XY + Y$ (slow)
$(iii)$ $X + Y \rightarrow XY$ (fast)
The overall order of the reaction will be