The rate coefficient k for a particular reaction is 1-3- 10-4 M-1 s-1 at 100oC and 1-3- 10-3 M-1 s-1 at 150oC- What is the energy of activation in kJ for this reaction-

The correct option is C 60From Arrhenius equation, ln k _ 2 k _ 1 #160; = E _ a R ( 1 T _ 1 1 T _ 2 ) ln 1.3 × 10^ 3 #160; #160;1.3 × ...

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Standard XII

Chemistry

Arrhenius Equation

The rate coef...

Question

The rate coefficient (k) for a particular reaction is $1.3 \times 10^{- 4} M^{- 1} s^{- 1}$ at $100^{o} C$ and $1.3 \times 10^{- 3} M^{- 1} s^{- 1}$ at $150^{o} C$ . What is the energy of activation $(i n k J)$ for this reaction?

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Solution

The correct option is C 60
From Arrhenius equation,

$ln \frac{k_{2}}{k_{1}} = \frac{E_{a}}{R} (\frac{1}{T_{1}} - \frac{1}{T_{2}})$
$ln \frac{1.3 \times 10^{- 3}}{1.3 \times 10^{- 4}} = \frac{E_{a}}{8.314} (\frac{1}{373} - \frac{1}{423})$
$E_{a} = 60 k J$

Hence, option B is correct.

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The rate coefficient (k) for a particular reaction is 1.3×10−4M−1s−1 at 100oC and 1.3×10−3M−1s−1 at 150oC. What is the energy of activation (in kJ) for this reaction?

The correct option is C 60From Arrhenius equation,lnk2k1=EaR(1T1−1T2)ln1.3×10−31.3×10−4=Ea8.314(1373−1423)Ea=60 kJHence, option B is correct.

The rate coefficient (k) for a particular reaction is $1.3 \times 10^{- 4} M^{- 1} s^{- 1}$ at $100^{o} C$ and $1.3 \times 10^{- 3} M^{- 1} s^{- 1}$ at $150^{o} C$ . What is the energy of activation $(i n k J)$ for this reaction?

The correct option is C 60
From Arrhenius equation,

$ln \frac{k_{2}}{k_{1}} = \frac{E_{a}}{R} (\frac{1}{T_{1}} - \frac{1}{T_{2}})$
$ln \frac{1.3 \times 10^{- 3}}{1.3 \times 10^{- 4}} = \frac{E_{a}}{8.314} (\frac{1}{373} - \frac{1}{423})$
$E_{a} = 60 k J$

Hence, option B is correct.