Medium
For three reactions of first,second,and third order,the rate constants are numerically equal. If the concentration of the reactant is the same and greater than $1 \ M$,which of the following is true for the rates of these three reactions?
- A$r_1 = r_2 = r_3$
- B$r_1 > r_2 > r_3$
- C$r_1 < r_2 < r_3$
- DAll of these
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Similar Questions
For an $n^{th}$ order reaction where $n < 1$,what is the expression for the time required for $100\%$ completion $(t_{100\%})$?
Difficult
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:
Which among the following is a false statement?
Easy
View SolutionFor a reaction of order $n$,the unit of the rate constant is :
For conversion of compound $A \rightarrow B$,the rate constant of the reaction was found to be $4.6 \times 10^{-5} \ L \ mol^{-1} \ s^{-1}$. The order of the reaction is $..........$
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