Medium
For a hypothetical reaction $A + B \rightarrow C$,the following data is provided from three different experiments:
$1$. $[A] = 0.01 \ M$,$[B] = 0.01 \ M$ - Rate of reaction $= 1.0 \times 10^{-4} \ M \ s^{-1}$.
$2$. $[A] = 0.01 \ M$,$[B] = 0.03 \ M$ - Rate of reaction $= 9.0 \times 10^{-4} \ M \ s^{-1}$.
$3$. $[A] = 0.03 \ M$,$[B] = 0.03 \ M$ - Rate of reaction $= 2.70 \times 10^{-3} \ M \ s^{-1}$.
Determine the rate law.
$1$. $[A] = 0.01 \ M$,$[B] = 0.01 \ M$ - Rate of reaction $= 1.0 \times 10^{-4} \ M \ s^{-1}$.
$2$. $[A] = 0.01 \ M$,$[B] = 0.03 \ M$ - Rate of reaction $= 9.0 \times 10^{-4} \ M \ s^{-1}$.
$3$. $[A] = 0.03 \ M$,$[B] = 0.03 \ M$ - Rate of reaction $= 2.70 \times 10^{-3} \ M \ s^{-1}$.
Determine the rate law.
- A$r = K[A]^2 [B]$
- B$r = K[A] [B]^2$
- C$r = K[A] [B]$
- DNone of these
Explore More
Similar Questions
Consider the following gas-phase reaction.
$2HI_{(g)} \longrightarrow H_{2(g)} + I_{2(g)}$
and the following experimental data obtained at $555 \ K$. What is the order of the reaction with respect to $HI_{(g)}$?
$[HI] \ (M)$ Rate $(M \ s^{-1})$ $0.0500$ $8.80 \times 10^{-10}$ $0.1000$ $3.52 \times 10^{-9}$ $0.1500$ $7.92 \times 10^{-9}$
$2HI_{(g)} \longrightarrow H_{2(g)} + I_{2(g)}$
and the following experimental data obtained at $555 \ K$. What is the order of the reaction with respect to $HI_{(g)}$?
| $[HI] \ (M)$ | Rate $(M \ s^{-1})$ |
| $0.0500$ | $8.80 \times 10^{-10}$ |
| $0.1000$ | $3.52 \times 10^{-9}$ |
| $0.1500$ | $7.92 \times 10^{-9}$ |
Medium
View SolutionFor a reaction $A + B \to \text{Products}$,the rate law is: $\text{Rate} = k[A][B]^{3/2}$. Can the reaction be an elementary reaction? Explain.
Easy
View SolutionFor a certain reaction,the rate $= k[A]^2[B]$. When the initial concentration of $A$ is tripled keeping the concentration of $B$ constant,the initial rate would:
MediumNEET 2023
View Solution$A_2 + 2 \, B \to 2 \, AB$
$[A_2]$ $[B]$ $-d[A_2]/dt$ $0.1$ $0.2$ $1 \times 10^{-2} \, M \, s^{-1}$ $0.2$ $0.2$ $2 \times 10^{-2} \, M \, s^{-1}$ $0.2$ $0.4$ $8 \times 10^{-2} \, M \, s^{-1}$
The order of reaction with respect to $A_2$ and $B$ are respectively:
| $[A_2]$ | $[B]$ | $-d[A_2]/dt$ |
|---|---|---|
| $0.1$ | $0.2$ | $1 \times 10^{-2} \, M \, s^{-1}$ |
| $0.2$ | $0.2$ | $2 \times 10^{-2} \, M \, s^{-1}$ |
| $0.2$ | $0.4$ | $8 \times 10^{-2} \, M \, s^{-1}$ |
The order of reaction with respect to $A_2$ and $B$ are respectively:
Medium
View SolutionWhich of the following statements is $NOT$ true for a reaction having rate law $r=k[H_2][I_2]$?
Vedclass 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