Write the unit of the rate constant for the following reactions:
$1.$ $5/2$ order
$2.$ $n$ order
$1.$ $5/2$ order
$2.$ $n$ order
(N/A) The general formula for the unit of the rate constant $(k)$ for a reaction of order $n$ is given by:
$k = (\text{concentration})^{1-n} \times (\text{time})^{-1}$
Using molarity $(M = \text{mol L}^{-1})$ and time in seconds $(s)$:
$1.$ For $n = 5/2$:
Unit $= (\text{mol L}^{-1})^{1 - 5/2} \times s^{-1} = (\text{mol L}^{-1})^{-3/2} \times s^{-1} = \text{mol}^{-3/2} \text{L}^{3/2} \text{s}^{-1}$
$2.$ For $n$ order:
Unit $= (\text{mol L}^{-1})^{1-n} \text{s}^{-1}$
$k = (\text{concentration})^{1-n} \times (\text{time})^{-1}$
Using molarity $(M = \text{mol L}^{-1})$ and time in seconds $(s)$:
$1.$ For $n = 5/2$:
Unit $= (\text{mol L}^{-1})^{1 - 5/2} \times s^{-1} = (\text{mol L}^{-1})^{-3/2} \times s^{-1} = \text{mol}^{-3/2} \text{L}^{3/2} \text{s}^{-1}$
$2.$ For $n$ order:
Unit $= (\text{mol L}^{-1})^{1-n} \text{s}^{-1}$
Explore More
Similar Questions
Write the differential rate expression for the following reaction and determine its order of reaction:
$H_{2}O_{2} + I^{-} \rightarrow H_{2}O + IO^{-}$
$H_{2}O_{2} + IO^{-} \rightarrow H_{2}O + I^{-} + O_{2}$
$H_{2}O_{2} + I^{-} \rightarrow H_{2}O + IO^{-}$
$H_{2}O_{2} + IO^{-} \rightarrow H_{2}O + I^{-} + O_{2}$
Medium
View SolutionWrite the differential rate expression for the following reactions and determine their order of reaction:
$1. CHCl_3 + Cl_2 \rightarrow CCl_4 + HCl$
$2. CH_3COOC_2H_5 + H_2O \rightarrow CH_3COOH + C_2H_5OH$
$1. CHCl_3 + Cl_2 \rightarrow CCl_4 + HCl$
$2. CH_3COOC_2H_5 + H_2O \rightarrow CH_3COOH + C_2H_5OH$
Medium
View SolutionFor an $n^{th}$ order reaction where $n < 1$,what is the expression for the time required for $100\%$ completion $(t_{100\%})$?
Difficult
View SolutionWhat will be the unit of the rate constant for the following reaction?
$C_2H_{4(g)} + H_{2(g)} \rightarrow C_2H_{6(g)}$
$C_2H_{4(g)} + H_{2(g)} \rightarrow C_2H_{6(g)}$
The rate law for the reaction $A + B \rightarrow C$ at $25^{\circ} C$ is given by $\text{rate} = k[A][B]^2$. Calculate the rate of reaction if the rate constant at the same temperature is $6.25 \ mol^{-2} \ dm^6 \ s^{-1}$ where $[A] = 1 \ M$ and $[B] = 0.2 \ M$.
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