For the reaction $A + 2B \longrightarrow C$, the reaction rate is doubled if the concentration of $A$ is doubled. The rate is increased by four times when concentrations of both $A$ and $B$ are increased by four times. The order of the reaction is
- A$3$
- B$0$
- C$1$
- D$2$
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Similar Questions
Which of the following statements regarding the order of a reaction is incorrect?
Medium
View SolutionWhat is the order of reaction for $A + B \to C$?
$Observation$ $[A] \ (mol \ L^{-1})$ $[B] \ (mol \ L^{-1})$ $Rate \ (mol \ L^{-1} \ sec^{-1})$ $1$ $0.1$ $0.1$ $2 \times 10^{-3}$ $2$ $0.2$ $0.1$ $4 \times 10^{-3}$ $3$ $0.1$ $0.2$ $8 \times 10^{-3}$
| $Observation$ | $[A] \ (mol \ L^{-1})$ | $[B] \ (mol \ L^{-1})$ | $Rate \ (mol \ L^{-1} \ sec^{-1})$ |
| $1$ | $0.1$ | $0.1$ | $2 \times 10^{-3}$ |
| $2$ | $0.2$ | $0.1$ | $4 \times 10^{-3}$ |
| $3$ | $0.1$ | $0.2$ | $8 \times 10^{-3}$ |
Medium
View SolutionThe rate for the reaction $2 A + B \rightarrow \text{product}$ is $6 \times 10^{-4} \ mol \ dm^{-3} \ s^{-1}$. Calculate the rate constant if the reaction is first order in $A$ and zeroth order in $B$,given $[A] = [B] = 0.3 \ M$.
For the reaction $A + B \to \text{Product}$,the rate of reaction becomes four times when the concentration of $A$ is doubled. If the rate of reaction does not change when the concentration of $B$ is doubled,the rate law for the reaction will be.....
Medium
View SolutionFor the catalytic decomposition of $AB_3$, the half-life period is $4 \, \text{hours}$ at $50 \, \text{mm}$ and $2 \, \text{hours}$ at $100 \, \text{mm}$. What is the order of the reaction?
Medium
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