For a first order reaction rate constant is 1- 10 -5 s-1 having Ea -1800 kJ-mol - Then the value of ln A at T-600 K is-

Acc. to arrhenius equation k =Ae ^−Ea/RT Rate constant 1× 10^−5s^−1 E_a = 1800 kJ/mol log k = log A− E_a/RT log 1× 10^−5s^−1 = log A− E_a/RT nbsp; nbsp; ...

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Standard XII

Chemistry

Introduction

For a first o...

Question

For a first order reaction rate constant is $1 \times 10^{-} 5 s^{- 1}$ having $E_{a}$ =1800 kJ/mol . Then the value of $l n A$ at T=600 K is:-

151.7

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110.9

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162.4

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193.5

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Solution

The correct option is A 151.7
Acc. to arrhenius equation
$k = A e^{\frac{- E a}{R T}}$
Rate constant $1 \times 10^{- 5} s^{- 1}$
$E_{a} = 1800 k J / m o l$
$l o g k = l o g A - \frac{E_{a}}{R T}$
$l o g 1 \times 10^{- 5} s^{- 1} = l o g A - \frac{E_{a}}{R T}$

$l o g A = l o g (1 \times 10^{- 5} s^{- 1}) + \frac{1800}{1 \times 10^{- 5} \times 600} = 151.7$

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For a first order reaction rate constant is 1×10−5 s−1 having Ea =1800 kJ/mol . Then the value of ln A at T=600 K is:-

The correct option is A 151.7Acc. to arrhenius equation k=Ae−EaRT Rate constant 1×10−5s−1 Ea = 1800 kJ/mol log k=log A−EaRT ​log 1×10−5s−1=log A−EaRT log A=log(1×10−5s−1)+18001×10−5×600=151.7

For a first order reaction rate constant is $1 \times 10^{-} 5 s^{- 1}$ having $E_{a}$ =1800 kJ/mol . Then the value of $l n A$ at T=600 K is:-