1.

if the activation energy of a reaction is 80.9 × 10^3 j/mol . calculate the fraction of molecules at 427°C , which have enough energy to react to form the products​

Answer»

if the activation energy of a reaction is 80.9 × 10^3 j/mol . CALCULATE the FRACTION of molecules at 427°C , which have enough energy to react to form the products

solution : according to Arrhenius's activation energy FORMULA,

\bf{A=e^{-\frac{E_a}{RT}}}

where A is fraction of molecules which have enough energy to react to form of the product, Ea is activation energy and T is TEMPERATURE in Kelvin.

here, T = 427°C = 427 + 273 = 700K

Ea = 80.9 × 10³ = 80900 J/mol

and R = 25/3 J/mol.K

now, A = e^{-\frac{80900}{\frac{25}{3}\times700}}

= e^{-13.8685}

= 9.48390025e-7

≈ 9.5 × 10^-7

hence, 9.5 × 10^-7 is the answer.


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