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99 Percentile Qs Bank for JEE MainChemistryChemical Kinetics

For a reversible reaction A B , which one of the following statements is wrong from the given energy profile diagram?

Options

  1. AActivation energy of forward reaction is greater than backward reaction
  2. BThe forward reaction is endothermic
  3. CThe threshold energy is less than that of activation energy
  4. DThe energy of activation of forward reaction is equal to the sum of heat of reaction and the energy of activat

Correct answer

C. The threshold energy is less than that of activation energy

Step-by-step solution

where, E_a= activation energy of forward reaction E_a^ = activation energy of backward reaction The above energy profile diagram shows that E_a>E_a^ The potential energy of the product is greater than that of the reactant, so the reaction is endothermic. aligned & E_a=E_a^ + E & E_t=E_a or E_t>E_a^ aligned

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