Question

The rate of reaction triples when the temperature changes from 20 ° C to 50 ° C . Calculate the 08 A gas is decomposed according to second order mechanism . For 50 % completion of reaction = 144.7 minutes it takes 50 minutes . The initial concentration of gaseous substance is 1.5 x 102 moles dm3 Calculate the second order rate constant​

Answer 1

Answer:

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Answer 2

Answer:

The Arrhenius equation is,

log10 k_{2}/k_{1} = E_{a}/(R * 2.303) * [(T_{2} - T_{1})/(T_{1}*T_{2})]

Given: k₂ k₁ = 3; R = 8.314 J K ¹ mol¹; T₁ 20 + 273 = 293K

and T2 = 50 + 273 = 323 K

Substituting the given values in the Arrhenius equation, log10 3 = E_{a}/(8.314 * 2.303) * [(323 - 293)/(323 * 293)]

E_{a} = (2.303 * 8.314 * 323 * 293 * 0.477)/30

= 28811.8 J mol-¹ = 28.8118 kJ mol-1

Explanation:

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