For a reaction $2NO_{(g)} + Cl_{2(g)} \rightleftharpoons 2NOCl_{(g)}$,when the concentration of $Cl_2$ is doubled,the rate of reaction becomes two times the original. When the concentration of $NO$ is doubled,the rate becomes four times. What is the order of the reaction?
- A$1$
- B$2$
- C$3$
- D$4$
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$A_{(g)} + 2B_{(g)} \to$ product is an elementary reaction. Which of the following is incorrect?
Medium
View SolutionThe initial rates of decrease of $I_2$ in acetone-iodine reaction catalysed by $H^{+}$ are given in the table.
Experiment Initial $[I_2]$ $(mol \ L^{-1})$ Initial $[H^{+}]$ $(mol \ L^{-1})$ Initial $[CH_3COCH_3]$ $(mol \ L^{-1})$ Initial rate $(mol \ L^{-1} \ s^{-1})$ $1$ $0.01$ $0.1$ $0.1$ $0.096$ $2$ $0.01$ $0.2$ $0.1$ $0.192$ $3$ $0.02$ $0.2$ $0.1$ $0.192$ $4$ $0.01$ $0.2$ $0.2$ $0.384$
The order with respect to $I_2, H^{+}$,acetone and total order of the reaction respectively are:
| Experiment | Initial $[I_2]$ $(mol \ L^{-1})$ | Initial $[H^{+}]$ $(mol \ L^{-1})$ | Initial $[CH_3COCH_3]$ $(mol \ L^{-1})$ | Initial rate $(mol \ L^{-1} \ s^{-1})$ |
| $1$ | $0.01$ | $0.1$ | $0.1$ | $0.096$ |
| $2$ | $0.01$ | $0.2$ | $0.1$ | $0.192$ |
| $3$ | $0.02$ | $0.2$ | $0.1$ | $0.192$ |
| $4$ | $0.01$ | $0.2$ | $0.2$ | $0.384$ |
The order with respect to $I_2, H^{+}$,acetone and total order of the reaction respectively are:
$t_{1/2} =$ constant confirms a first-order reaction. If $a^2 t_{1/2} =$ constant,it confirms that the order of the reaction is ($a =$ initial concentration of reactant).
Medium
View SolutionWrite 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
Easy
View SolutionThe 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 $(mol \ L^{-1} \ s^{-1})$ |
| $1$ | $8 \times 10^{-5}$ | $8 \times 10^{-5}$ | $7 \times 10^{-9}$ |
| $2$ | $24 \times 10^{-5}$ | $8 \times 10^{-5}$ | $2.1 \times 10^{-8}$ |
| $3$ | $24 \times 10^{-5}$ | $32 \times 10^{-5}$ | $8.4 \times 10^{-8}$ |
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