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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The dimension of the rate constant for a second-order reaction involves:
Easy
View SolutionFor the reaction $2A + 2B \rightarrow 2C + D$,if $r = k[A]^2[B]^0$,then the rate of reaction is:
For the reaction $A_2 + B_2 \to 2AB$,the experimental data is given below. Determine the order of the reaction.
Experiment No. $[A_2] \text{ (M)}$ $[B_2] \text{ (M)}$ Rate $(M \cdot s^{-1})$ $1$ $0.1$ $0.1$ $1.6 \times 10^{-4}$ $2$ $0.1$ $0.2$ $3.2 \times 10^{-4}$ $3$ $0.2$ $0.1$ $3.2 \times 10^{-4}$
| Experiment No. | $[A_2] \text{ (M)}$ | $[B_2] \text{ (M)}$ | Rate $(M \cdot s^{-1})$ |
| $1$ | $0.1$ | $0.1$ | $1.6 \times 10^{-4}$ |
| $2$ | $0.1$ | $0.2$ | $3.2 \times 10^{-4}$ |
| $3$ | $0.2$ | $0.1$ | $3.2 \times 10^{-4}$ |
Medium
View SolutionFor the reaction $2A + 2B \rightarrow 2C + D$,the rate law is expressed as $\text{rate} = k[A]^2[B]$. Calculate the rate constant if the rate of reaction is $0.24 \ mol \ dm^{-3} \ s^{-1}$ where $[A] = 0.5 \ M$ and $[B] = 0.2 \ M$.
Which function of $[X]$ plotted against time will give a straight line for a second order reaction? $X \to \text{Product}$
Medium
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