What is the activation energy for a reaction, if its rate doubles when the temperature is raised from $$20oC$$ to $$35oC$$ ? $$R=8.314Jmol$$−$$1K$$−$$1$$

Question

What is the activation energy for a reaction, if its rate doubles when the temperature is raised from $$20oC$$ to $$35oC$$ ? $$R=8.314Jmol$$−$$1K$$−$$1$$

Infinity Learn · Accepted Answer

Given, initial temperature $$T1=20+273=293KFinal$$ temperature, $$T2=35+273=308KR=8.314Jmol$$−$$1K$$−$$1Since$$, rate becomes double on raising temperature $$r2=2r1$$⇒$$r2r1=2As$$ rate constant, k∝r⇒$$k2k1=2From$$ Arrhenius equation, we know that log $$k2k1=$$−$$Ea2.303RT2$$−$$T1T1T2$$                                                      log $$2=Ea2.303$$×$$8.314308$$−$$293293$$×$$308$$                                                   $$0.3010=Ea2.303$$×$$8.31415293$$×$$308$$                                              $$Ea=0.3010$$×$$2.303$$×$$8.314$$×$$293$$×$$30815$$                                                  $$=34673.48Jmol$$−$$1=34.7kJmol$$−$$1$$

What is the activation energy for a reaction, if its rate doubles when the temperature is raised from 20oC to 35oC ? R=8.314Jmol−1K−1

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