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BITSAT2018ChemistryChemical KineticsActual

The rate of a reaction triples when temperature changes from 20 0 C to 50 0 C . The energy of activation for the reaction is R = 8 . 314 JK - 1 mol - 1

Options

  1. A181 . 327   J   mol - 1
  2. B428 . 141   J   mol - 1
  3. C32 . 4321 kJmol - 1
  4. D28 . 8118 kJmol - 1

Correct answer

D. 28 . 8118 kJmol - 1

Step-by-step solution

Arrhenius equation is given by, log 10 K 2 K 1 = E a 2 . 303 × R T 2 - T 1 T 1 T 2 Given, K 2 K 1 = 3 ; R = - 8 . 314   JK - 1 mol - 1 T 1 = 20 + 273 = 293   K and T 2 = 50 + 273 = 323   K Substituting the given values in Arrhenius equation, log 10 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 kJmol - 1

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