The rate of a reaction doubles when its temperature changes form 300 K to 310 K. Activation energy of such a reaction will be $(R = 8.314 J K^{- 1} m o l^{- 1} a n d l o g 2 = 0.301)$

$53.6 k j m o l^{- 1}$

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$48.6 k j m o l^{- 1}$

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$58.5 k j m o l^{- 1}$

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$60.5 k j m o l^{- 1}$

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Solution

The correct option is A
$53.6 k j m o l^{- 1}$

From Arrhenius equation, $l o g \frac{k_{2}}{k_{1}} = \frac{- E_{α}}{2.303 R} (\frac{1}{T_{2}} - \frac{1}{T_{1}})$
Given, $\frac{k_{2}}{k_{1}} = 2 T_{2} = 310 k$
$T_{1} = 300 k$
On putting values,
$\Rightarrow l o g 2 = \frac{- E_{α}}{2.303 \times 8.314} (\frac{1}{310} - \frac{1}{300})$
$\Rightarrow E_{α} = 53598.6 J / m o l = 53.6 k J / m o l$

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The rate of a reaction doubles when its temperature changes form 300 K to 310 K. Activation energy of such a reaction will be $(R = 8.314 J K^{- 1} m o l^{- 1} a n d l o g 2 = 0.301)$

Q. The rate of a reaction doubles when its temperature changes from 300 K to 310 K. Activation energy of such a reaction will be:

(R = 8.314 J K^{- 1} m o l^{- 1}

and

l o g_{10} 2 = 0.301)

Q. The rate of a reaction doubles when its temperature changes from

300 K

310 K

. Activation energy of such a reaction will be:

[R = 8.314 J K^{- 1} m o l^{- 1}

and

log 2 = 0.301]

The rate of a reaction doubles when its temperature changes form 300 K to 310 K. Activation energy of such a reaction will be $(R = 8.314 J K^{- 1} m o l^{- 1} a n d l o g 2 = 0.301)$

The rate of a reaction doubles when its temperature changes from 300 K to 310 K. Activation energy of such a reaction will be:

$(R = 8.314 J K^{- 1} m o l^{- 1} a n d l o g 2 = 0.301)$

(IIT-JEE-2013)

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The rate of a reaction doubles when its temperature changes form 300 K to 310 K. Activation energy of such a reaction will be (R=8.314 JK−1 mol−1 and log 2=0.301)

The correct option is A 53.6 kj mol−1 From Arrhenius equation, logk2k1=−Eα2.303 R(1T2−1T1) Given, k2k1=2 T2=310 k T1=300 k On putting values, ⇒log 2=−Eα2.303×8.314(1310−1300) ⇒Eα=53598.6 J/mol = 53.6kJ/mol

The rate of a reaction doubles when its temperature changes form 300 K to 310 K. Activation energy of such a reaction will be $(R = 8.314 J K^{- 1} m o l^{- 1} a n d l o g 2 = 0.301)$