Problem: Part DGiven that the rate constant is 4.0×10−4 M-1 s-1 at 25.0 °C and that the rate constant is 2.6×10−3 M-1 s-1 at 42.4 °C, what is the activation energy in kilojoules per mole? Note that the value of the constant R is R = 8.3145 J/mol • K).Express your answer numerically in kilojoules per mole using three significant figures.

FREE Expert Solution

Two-point form of the Arrhenius Equation:

$\overline{){\mathbf{ln}}\frac{{\mathbf{k}}_{\mathbf{2}}}{{\mathbf{k}}_{\mathbf{1}}}{\mathbf{=}}{\mathbf{-}}\frac{{\mathbf{E}}_{\mathbf{a}}}{\mathbf{R}}\mathbf{\left[}\frac{\mathbf{1}}{{\mathbf{T}}_{\mathbf{2}}}\mathbf{-}\frac{\mathbf{1}}{{\mathbf{T}}_{\mathbf{1}}}\mathbf{\right]}}$

T1 = 25 ˚C + 273.15 = 298.15 K

T2 = 42.4 ˚C + 273.15 = 315.55 K

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Problem Details

Part D

Given that the rate constant is 4.0×10−4 M-1 s-1 at 25.0 °C and that the rate constant is 2.6×10−3 M-1 s-1 at 42.4 °C, what is the activation energy in kilojoules per mole? Note that the value of the constant R is R = 8.3145 J/mol • K).

Express your answer numerically in kilojoules per mole using three significant figures.

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