Medium
Write the unit of the rate constant for the following reactions:
$1.$ Fourth order
$2.$ Third order
$1.$ Fourth order
$2.$ Third order
(N/A) The general formula for the unit of the rate constant $(k)$ for a reaction of order $n$ is given by:
Unit of $k = (mol \ L^{-1})^{1-n} \ s^{-1}$
$1.$ For a fourth order reaction $(n = 4)$:
Unit of $k = (mol \ L^{-1})^{1-4} \ s^{-1} = (mol \ L^{-1})^{-3} \ s^{-1} = mol^{-3} \ L^3 \ s^{-1}$
$2.$ For a third order reaction $(n = 3)$:
Unit of $k = (mol \ L^{-1})^{1-3} \ s^{-1} = (mol \ L^{-1})^{-2} \ s^{-1} = mol^{-2} \ L^2 \ s^{-1}$
Unit of $k = (mol \ L^{-1})^{1-n} \ s^{-1}$
$1.$ For a fourth order reaction $(n = 4)$:
Unit of $k = (mol \ L^{-1})^{1-4} \ s^{-1} = (mol \ L^{-1})^{-3} \ s^{-1} = mol^{-3} \ L^3 \ s^{-1}$
$2.$ For a third order reaction $(n = 3)$:
Unit of $k = (mol \ L^{-1})^{1-3} \ s^{-1} = (mol \ L^{-1})^{-2} \ s^{-1} = mol^{-2} \ L^2 \ s^{-1}$
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Which of the following is an example of a second-order reaction?
Write the unit of the rate constant for the following reactions:
$1.$ $5/2$ order
$2.$ $n$ order
$1.$ $5/2$ order
$2.$ $n$ order
Easy
View SolutionFor the reaction $N_2O_5 \rightarrow 2NO_2 + \frac{1}{2} O_2$,given that:
$-\frac{d[N_2O_5]}{dt} = K_1[N_2O_5]$,
$\frac{d[NO_2]}{dt} = K_2[N_2O_5]$,
$\frac{d[O_2]}{dt} = K_3[N_2O_5]$
What is the relationship between $K_1$,$K_2$,and $K_3$?
$-\frac{d[N_2O_5]}{dt} = K_1[N_2O_5]$,
$\frac{d[NO_2]}{dt} = K_2[N_2O_5]$,
$\frac{d[O_2]}{dt} = K_3[N_2O_5]$
What is the relationship between $K_1$,$K_2$,and $K_3$?
Difficult
View Solution$(a)$ Write the general reaction and derive the units of the rate constant. $(b)$ Based on that,write the rate constant units for zero,first,and $2^{nd}$ order reactions.
Difficult
View SolutionThe 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:
DifficultAP EAMCET 2022
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