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The rate of a reaction double when its temperature changes fro

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The rate of a reaction double when its temperature changes from $300 K$ to $310 K$ . Activation energy of such a reaction will be $(R = 8.314 JK^{- 1} mol^{- 1}$ and $lo g 2 = 0.301$ )

Name: Video solution 1: The rate of a reaction double when its temperature changes from 300 K to 310 K. Activation energy of such a reaction will be (R=8.314JK−1 mol−1 and log2=0.301 )
Uploaded: 2023-01-31T09:47:13.000Z
Duration: 3 min
Description: Video solution 1: The rate of a reaction double when its temperature changes from 300 K to 310 K. Activation energy of such a reaction will be (R=8.314JK−1 mol−1 and log2=0.301 )

53.6 kJ mol^{- 1}

48.6 kJ mol^{- 1}

58.5 kJ mol^{- 1}

60.5 kJ mol^{- 1}

Views: 6,300 students

Updated on: Jan 31, 2023

Book:

Arihant Chemistry JEE Main Chapterwise Solutions (2019-2002) (Arihant)

Exam:

JEE Mains 2013

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Daniel Discussed

The rate of a reaction double when its temperature changes from

300 K

310 K

. Activation energy of such a reaction will be

(R = 8.314 JK^{- 1} mol^{- 1}

and

lo g 2 = 0.301

)

13 mins ago

Discuss this question LIVE

13 mins ago

Text solutionVerified

From Arrhenius equation,

lo g \frac{k _{2}}{k _{1}} = \frac{- E _{a}}{2.303 R} (\frac{1}{T _{2}} - \frac{1}{T _{1}})

Given,

\frac{k _{2}}{k _{1}} = 2; T_{2} = 310 K

T_{1} = 300 K

On putting values,

\Rightarrow lng ρ = \frac{- E _{a}}{2.303 \times 8.314} (\frac{1}{310} - \frac{1}{300})

\Rightarrow E_{a} = 53603.93 J / mol = 53.6 kJ / mol

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Question Text	The rate of a reaction double when its temperature changes from $300 K$ to $310 K$ . Activation energy of such a reaction will be $(R = 8.314 JK^{- 1} mol^{- 1}$ and $lo g 2 = 0.301$ )
Updated On	Jan 31, 2023
Topic	Chemical Kinetics
Subject	Chemistry
Class	Class 12
Answer Type	Text solution:1 Video solution: 2
Upvotes	310
Avg. Video Duration	3 min

The rate of a reaction double when its temperature changes from $300 K$ to $310 K$ . Activation energy of such a reaction will be $(R = 8.314 JK^{- 1} mol^{- 1}$ and $lo g 2 = 0.301$ )

Text solutionVerified

Filo tutor solutions (2)

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The rate of a reaction double when its temperature changes from 300 K to 310 K. Activation energy of such a reaction will be (R=8.314JK−1 mol−1 and log2=0.301 )

Text solutionVerified

Filo tutor solutions (2)

Questions from JEE Mains 2013 - PYQs

Practice questions from Arihant Chemistry JEE Main Chapterwise Solutions (2019-2002) (Arihant)

Practice questions from Chemical Kinetics in the same exam

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The rate of a reaction double when its temperature changes from $300 K$ to $310 K$ . Activation energy of such a reaction will be $(R = 8.314 JK^{- 1} mol^{- 1}$ and $lo g 2 = 0.301$ )