Medium
In the reaction $A + B \to \text{Products}$,the initial concentration of both $A$ and $B$ is $0.1 \, M$. When the concentration decreases to $1.0 \times 10^{-2} \, M$,the half-life period increases by ten times. The rate of the reaction is:
- Aproportional to the first power of concentration
- Bproportional to the second power of concentration
- Cindependent of concentration
- Dproportional to the third power of concentration
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Similar Questions
Mechanism of a hypothetical reaction $X_2 + Y_2 \rightarrow 2XY$ is given below:
$(i)$ $X_2 \rightarrow X + X$ (fast)
$(ii)$ $X + Y_2 \rightleftharpoons XY + Y$ (slow)
$(iii)$ $X + Y \rightarrow XY$ (fast)
The overall order of the reaction will be
$(i)$ $X_2 \rightarrow X + X$ (fast)
$(ii)$ $X + Y_2 \rightleftharpoons XY + Y$ (slow)
$(iii)$ $X + Y \rightarrow XY$ (fast)
The overall order of the reaction will be
Which of the following statements is incorrect?
Easy
View SolutionRate law for a reaction is $r=k[A]^2[B]$. If rate constant is $6.25 \ mol^{-2} \ dm^6 \ s^{-1}$,what is the rate of reaction when $[A]=1 \ mol \ dm^{-3}$ and $[B]=0.2 \ mol \ dm^{-3}$?
For a gaseous reaction $2A + B \rightarrow C + D$,the rate of reaction is given by $Rate = K[A][B]$. If the volume of the container is reduced to $1/4$ of its original volume,what will be the ratio of the new rate to the original rate?
Medium
View SolutionRate of reaction is $r_1 = k[A]^a[B]^b$. If the concentration of $A$ is doubled and $B$ is halved,the new rate is $r_2$. What is the value of $\frac{r_2}{r_1}$?
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