Write the unit of the rate constant for the following reactions:
$1.$ $\frac{1}{2}$ order
$2.$ $\frac{3}{2}$ order
$1.$ $\frac{1}{2}$ order
$2.$ $\frac{3}{2}$ order
The general formula for the unit of the rate constant $k$ for a reaction of order $n$ is given by:
Unit $= (mol \ L^{-1})^{1-n} \ s^{-1}$
$1.$ For a reaction of order $n = \frac{1}{2}$:
Unit $= (mol \ L^{-1})^{1 - 1/2} \ s^{-1} = (mol \ L^{-1})^{1/2} \ s^{-1} = mol^{1/2} \ L^{-1/2} \ s^{-1}$
$2.$ For a reaction of order $n = \frac{3}{2}$:
Unit $= (mol \ L^{-1})^{1 - 3/2} \ s^{-1} = (mol \ L^{-1})^{-1/2} \ s^{-1} = mol^{-1/2} \ L^{1/2} \ s^{-1}$
Unit $= (mol \ L^{-1})^{1-n} \ s^{-1}$
$1.$ For a reaction of order $n = \frac{1}{2}$:
Unit $= (mol \ L^{-1})^{1 - 1/2} \ s^{-1} = (mol \ L^{-1})^{1/2} \ s^{-1} = mol^{1/2} \ L^{-1/2} \ s^{-1}$
$2.$ For a reaction of order $n = \frac{3}{2}$:
Unit $= (mol \ L^{-1})^{1 - 3/2} \ s^{-1} = (mol \ L^{-1})^{-1/2} \ s^{-1} = mol^{-1/2} \ L^{1/2} \ s^{-1}$
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Similar Questions
The following data was obtained for the chemical reaction given below at $975 \ K$: $2 NO_{(g)} + 2 H_{2(g)} \rightarrow N_{2(g)} + 2 H_{2}O_{(g)}$
Experiment $[NO] \ (mol \ L^{-1})$ $[H_{2}] \ (mol \ L^{-1})$ Rate $(mol \ L^{-1} \ s^{-1})$ $1$ $8 \times 10^{-5}$ $8 \times 10^{-5}$ $7 \times 10^{-9}$ $2$ $24 \times 10^{-5}$ $8 \times 10^{-5}$ $2.1 \times 10^{-8}$ $3$ $24 \times 10^{-5}$ $32 \times 10^{-5}$ $8.4 \times 10^{-8}$
The order of the reaction with respect to $NO$ is ..... .
| Experiment | $[NO] \ (mol \ L^{-1})$ | $[H_{2}] \ (mol \ L^{-1})$ | Rate $(mol \ L^{-1} \ s^{-1})$ |
| $1$ | $8 \times 10^{-5}$ | $8 \times 10^{-5}$ | $7 \times 10^{-9}$ |
| $2$ | $24 \times 10^{-5}$ | $8 \times 10^{-5}$ | $2.1 \times 10^{-8}$ |
| $3$ | $24 \times 10^{-5}$ | $32 \times 10^{-5}$ | $8.4 \times 10^{-8}$ |
Write the unit of the rate constant for the following reactions:
$1.$ Zero order
$2.$ Second order
$1.$ Zero order
$2.$ Second order
Medium
View SolutionCalculate the order of the reaction with respect to $A$ and $B$ based on the following data:
$[A] \ (mol/L)$ $[B] \ (mol/L)$ Rate $(mol/L \cdot s)$ $0.05$ $0.05$ $1.2 \times 10^{-3}$ $0.10$ $0.05$ $2.4 \times 10^{-3}$ $0.05$ $0.10$ $1.2 \times 10^{-3}$
| $[A] \ (mol/L)$ | $[B] \ (mol/L)$ | Rate $(mol/L \cdot s)$ |
| $0.05$ | $0.05$ | $1.2 \times 10^{-3}$ |
| $0.10$ | $0.05$ | $2.4 \times 10^{-3}$ |
| $0.05$ | $0.10$ | $1.2 \times 10^{-3}$ |
Easy
View SolutionThe dimension of the rate constant for a second-order reaction involves:
Easy
View SolutionFor which type of reactions,order and molecularity have the same value?
Easy
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