Medium
The rate law for the reaction $A + B \rightarrow \text{product}$ is $\text{rate} = k[A][B]$. When will the rate of reaction increase by a factor of $2$?
- A$[A]$ and $[B]$ both are doubled
- B$[A]$ is doubled and $[B]$ is kept constant
- C$[B]$ is doubled and $[A]$ is halved
- D$[A]$ is kept constant and $[B]$ is halved
Explore More
Similar Questions
For a reaction,$A + B \rightarrow$ products,the rate of the reaction at various concentrations is given below. The rate law for the above reaction is:
Expt. no. $[A]$ $[B]$ Rate $(\text{mol} \ \text{dm}^{-3} \ \text{s}^{-1})$ $1$ $0.2$ $0.2$ $2$ $2$ $0.2$ $0.4$ $4$ $3$ $0.6$ $0.4$ $36$
| Expt. no. | $[A]$ | $[B]$ | Rate $(\text{mol} \ \text{dm}^{-3} \ \text{s}^{-1})$ |
|---|---|---|---|
| $1$ | $0.2$ | $0.2$ | $2$ |
| $2$ | $0.2$ | $0.4$ | $4$ |
| $3$ | $0.6$ | $0.4$ | $36$ |
For a reaction $A$ $\xrightarrow{K_1} B$ $\xrightarrow{K_2} C$. If the rate of formation of $B$ is set to be zero,then the concentration of $B$ is given by:
In a reaction involving hydrolysis of an organic chloride in the presence of a large excess of water,$RCl + H_2O \to ROH + HCl$.
Medium
View SolutionWhat is the order of the following reaction: $2H_2O_2(l) \rightarrow 2H_2O(l) + O_2(g)$, given that the rate law is $\text{rate} = k[H_2O_2]^1$?
The rate equation for the reaction $2A + B \to C$ is found to be: $\text{rate} = k[A][B]$. The correct statement in relation to this reaction is that the
MediumAIEEE 2004
View SolutionVedclass Products
For Students
Vedclass Test Series
Mock tests in real JEE/NEET style with performance analysis. 5-day free trial.
Start Free TrialFor Teachers
Exam Paper Generator
Generate Set A/B/C/D exam papers from 7.5L+ questions in 2 minutes. 3 chapters free.
Try FreeFor Institutes
Online Exam Module
Live online exams with unlimited students, 360° analytics & white-label branding.
See Demo