For the reaction: A → B

The rate constant at 300 K is k₁ and at 400 K is k₂. If the activation energy Eₐ = 19.9 kJ mol⁻¹, the ratio k₂/k₁ is:

(Given: R = 8.314 J mol⁻¹K⁻¹, log 10 = 1)

(Enter the in

Question

For the reaction: A → B

The rate constant at 300 K is k₁ and at 400 K is k₂. If the activation energy Eₐ = 19.9 kJ mol⁻¹, the ratio k₂/k₁ is:

(Given: R = 8.314 J mol⁻¹K⁻¹, log 10 = 1)

(Enter the integer answer)

Canvas Classes · Accepted Answer

Arrhenius equation (two-temperature form):

9254\log\frac{k2}{k1} = \frac{Ea}{2.303R}\left(\frac{1}{T1} - \frac{1}{T2}ight)9254

9254\frac{1}{300} - \frac{1}{400} = \frac{1}{1200}\,	ext{K}^{-1}9254

9254\log\frac{k2}{k1} = \frac{19900}{2.303 	imes 8.314 	imes 1200} \approx 19254

9254\frac{k2}{k1} = 10^1 = \boxed{10}9254

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