The rate of a reaction quadruples when the temperature changes from 300 to 310 K. The activation energy of this reaction is :
(Assume activation energy and pre-exponential factor are independent of temperature; $l n 2$ =0.693; R = 8.314 J $m o l^{- 1} K^{- 1}$ )

26.8 kJ

m o l^{- 1}

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414.4 kJ

m o l^{- 1}

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107.2 kJ

m o l^{- 1}

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53.6 kJ

m o l^{- 1}

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Solution

The correct option is C 107.2 kJ $m o l^{- 1}$
The rate of the reaction can be written as:

$l n (\frac{K_{2}}{K_{1}}) = \frac{E_{a}}{R} [\frac{1}{T_{1}} - \frac{1}{T_{2}}]$

$l n (\frac{4}{1}) = \frac{E_{a}}{8.314} [\frac{1}{300} - \frac{1}{310}]$

$\Rightarrow E_{a} = 107.2 K J / m o l$

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Similar questions

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:

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)

Q. The rate of a reaction quadruples when the temperature changes from 300 to 310K. What is the activation energy of this reaction?
(Assume activation energy and preexponential factor are independent of temperature ; In 2= 0.693; R= 8.314 J

m o l^{- 1} K^{- 1}

)

The rate of reaction doubles when its temperature changes from 300K to 310 K .activation energy of such a reaction will be (R=8.314 kj/ mol and WG2= 0.031 )

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The rate of a reaction quadruples when the temperature changes from 300 to 310 K. The activation energy of this reaction is : (Assume activation energy and pre-exponential factor are independent of temperature; ln 2=0.693; R = 8.314 J mol−1K−1)

The correct option is C 107.2 kJ mol−1The rate of the reaction can be written as:ln(K2K1)=EaR[1T1−1T2]ln(41)=Ea8.314[1300−1310]⇒Ea=107.2 KJ/mol

The rate of a reaction quadruples when the temperature changes from 300 to 310 K. The activation energy of this reaction is :
(Assume activation energy and pre-exponential factor are independent of temperature; $l n 2$ =0.693; R = 8.314 J $m o l^{- 1} K^{- 1}$ )

The correct option is C 107.2 kJ $m o l^{- 1}$
The rate of the reaction can be written as:

$l n (\frac{K_{2}}{K_{1}}) = \frac{E_{a}}{R} [\frac{1}{T_{1}} - \frac{1}{T_{2}}]$

$l n (\frac{4}{1}) = \frac{E_{a}}{8.314} [\frac{1}{300} - \frac{1}{310}]$

$\Rightarrow E_{a} = 107.2 K J / m o l$