(A) The rate of reaction is given by the expression: $-\frac{d[N_2]}{dt} = -\frac{1}{3} \frac{d[H_2]}{dt} = \frac{1}{2} \frac{d[NH_3]}{dt}$.Given that

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$4.44 \times 10^{-3} \ mol \ dm^{-3} \ s^{-1}$

(A) The rate of reaction is given by the expression: $-\frac{d[N_2]}{dt} = -\frac{1}{3} \frac{d[H_2]}{dt} = \frac{1}{2} \frac{d[NH_3]}{dt}$.Given that the rate of disappearance of $N_2$ is $-\frac{d[N_2]}{dt} = 2.22 \times 10^{-3} \ mol \ dm^{-3} \ s^{-1}$.From the stoichiometric relationship,we have: $\frac{d[NH_3]}{dt} = 2 \times (-\frac{d[N_2]}{dt})$.Substituting the given value: $\frac{d[NH_3]}{dt} = 2 \times (2.22 \times 10^{-3} \ mol \ dm^{-3} \ s^{-1}) = 4.44 \times 10^{-3} \ mol \ dm^{-3} \ s^{-1}$.

Class 12 Chemistry Chemical Kinetics Rate of a reaction

Easy

For the reaction $N_{2(g)} + 3H_{2(g)} \rightarrow 2NH_{3(g)}$,the rate of disappearance of $N_{2(g)}$ is $2.22 \times 10^{-3} \ mol \ dm^{-3} \ s^{-1}$. What is the rate of appearance of $NH_{3(g)}$?

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A
$4.44 \times 10^{-3} \ mol \ dm^{-3} \ s^{-1}$
B
$1.11 \times 10^{-3} \ mol \ dm^{-3} \ s^{-1}$
C
$2.22 \times 10^{-3} \ mol \ dm^{-3} \ s^{-1}$
D
$3.33 \times 10^{-3} \ mol \ dm^{-3} \ s^{-1}$

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For the reaction $N_{2(g)} + 3 H_{2(g)} \rightarrow 2 NH_{3(g)}$,what is the relation between $\frac{d[N_2]}{dt}$ and $\frac{d[H_2]}{dt}$?

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If the first order reaction involves gaseous reactants and gaseous products,the units of its rate are:

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For the reaction $N_2 + 3H_2 \to 2NH_3$,if $\frac{\Delta [NH_3]}{\Delta t} = 2 \times 10^{-4} \ mol \ L^{-1} s^{-1}$,the value of $\frac{-\Delta [H_2]}{\Delta t}$ would be

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In a reaction,$n_1A + n_2B \to m_1C + m_2D$,$5 \ M$ of reactant $A$ are allowed to react with $3 \ M$ of reactant $B$. After $5 \ sec$,the concentration of $A$ was found to be $4 \ M$. What are the rate of decomposition of $A$ and the rate of formation of $D$,respectively?

Difficult

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In a pseudo first order hydrolysis of ester in water,the following results were obtained:

$t \ (s)$ $0$ $30$ $60$ $90$

$[\text{Ester}] \ (mol \ L^{-1})$ $0.55$ $0.31$ $0.17$ $0.085$

What will be the average rate of reaction between the time interval $30 \ s$ to $60 \ s$?

Medium

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$t \ (s)$	$0$	$30$	$60$	$90$
$[\text{Ester}] \ (mol \ L^{-1})$	$0.55$	$0.31$	$0.17$	$0.085$

For the reaction $N_{2(g)} + 3H_{2(g)} \rightarrow 2NH_{3(g)}$,the rate of disappearance of $N_{2(g)}$ is $2.22 \times 10^{-3} \ mol \ dm^{-3} \ s^{-1}$. What is the rate of appearance of $NH_{3(g)}$?

Similar Questions

For the reaction $N_{2(g)} + 3 H_{2(g)} \rightarrow 2 NH_{3(g)}$,what is the relation between $\frac{d[N_2]}{dt}$ and $\frac{d[H_2]}{dt}$?

If the first order reaction involves gaseous reactants and gaseous products,the units of its rate are:

For the reaction $N_2 + 3H_2 \to 2NH_3$,if $\frac{\Delta [NH_3]}{\Delta t} = 2 \times 10^{-4} \ mol \ L^{-1} s^{-1}$,the value of $\frac{-\Delta [H_2]}{\Delta t}$ would be

In a reaction,$n_1A + n_2B \to m_1C + m_2D$,$5 \ M$ of reactant $A$ are allowed to react with $3 \ M$ of reactant $B$. After $5 \ sec$,the concentration of $A$ was found to be $4 \ M$. What are the rate of decomposition of $A$ and the rate of formation of $D$,respectively?

In a pseudo first order hydrolysis of ester in water,the following results were obtained: $t \ (s)$ $0$ $30$ $60$ $90$ $[\text{Ester}] \ (mol \ L^{-1})$ $0.55$ $0.31$ $0.17$ $0.085$ What will be the average rate of reaction between the time interval $30 \ s$ to $60 \ s$?

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In a pseudo first order hydrolysis of ester in water,the following results were obtained:

$t \ (s)$ $0$ $30$ $60$ $90$

$[\text{Ester}] \ (mol \ L^{-1})$ $0.55$ $0.31$ $0.17$ $0.085$

What will be the average rate of reaction between the time interval $30 \ s$ to $60 \ s$?