A first order reaction- 2 N 2 O g - 2 N 2 g - O 2 g - has a rate constant of 1-3- 10 -11 s -1 at 270 o C and 4-5- 10 -10 s -1 at 350 o C- What is the activation energy for this reaction-

The correct option is C 120 kJ log( k _ 2 k _ 1 #160;) #160; = E _ a 2.303R [ 1 T _ 1 1 T _ 2 #160;] log( 4.5× 10 ^ 10 1.3× ...

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Arrhenius Equation

A first order...

Question

A first order reaction, $2 N_{2} O (g) ⟶ 2 N_{2} (g) + O_{2} (g)$ , has a rate constant of $1.3 \times 10^{- 11} s^{- 1}$ at $270^{o} C$ and $4.5 \times 10^{- 10} s^{- 1}$ at $350^{o} C$ . What is the activation energy for this reaction?

15 k J

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30 k J

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68 k J

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120 k J

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