The decomposition of a hydrocarbon follows the equation k - 4-5- 1011s-1e-28000- K-T- What will be the value of activation energy-

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Arrhenius Equation

The decomposi...

Question

The decomposition of a hydrocarbon follows the equation $k = (4.5 \times 10^{11} s^{- 1}) e^{- 28000 / K / T}$ . What will be the value of activation energy?

669 k J m o l^{- 1}

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232.79 k J m o l^{- 1}

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4.5 \times 10^{11} k J m o l^{- 1}

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28000 k J m o l^{- 1}

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Solution

The correct option is B $232.79 k J m o l^{- 1}$
Arrhenius equation, $k = A e^{- E_{a} / R T}$

Given equation is
$k = (4.5 \times 10^{11} s^{- 1}) e^{- 28000 K / T}$
Comparing both the equations, we get
$- \frac{E_{a}}{R T} = - \frac{28000 K}{T}$
$E_{a} = 28000 K \times R = 28000 K \times 8.314 J K^{- 1} m o l^{- 1}$
$= 232.79 k J m o l^{- 1}$ .

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The decomposition of hydrocarbon follows the equation $k = (4.5 \times 10^{11} s^{- 1}) e^{- 28000} K / T$ . Calculate the activation energy $E_{a}$

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The decomposition of a hydrocarbon follows the equation k=(4.5×1011s−1)e−28000/K/T. What will be the value of activation energy?

The correct option is B 232.79 kJ mol−1Arrhenius equation, k=Ae−Ea/RTGiven equation isk=(4.5×1011s−1)e−28000 K/TComparing both the equations, we get−EaRT=−28000 KTEa=28000 K×R=28000 K×8.314 J K−1mol−1=232.79 kJ mol−1.

The decomposition of a hydrocarbon follows the equation $k = (4.5 \times 10^{11} s^{- 1}) e^{- 28000 / K / T}$ . What will be the value of activation energy?