A catalyst increases the rate of chemical reaction by providing an alternative reaction pathway which lowers the activation energy than the reaction pathway in its absence. A catalyst is not consumed and therefore does not appear in the chemical equation for the reaction. A homogenous catalyst is in the same phase as the ractants whilst a heterogeneous catalyst is in a different phase. The complex [Co(NH_(3))_(3)F]^(2+)+H_(2)Oto[Co(NH_(3))_(5)(H_(2)O+F^(-)]^(3+) and Rate =k["complex"]^(a).[H^(+)]^(b) The reaction is acid catalysed , i.e. [H^(+)] does not change during the reaction . Thus, rate =k'["complex"] where, k'=[H^(+)]^(b) The value of activation energy for a chemical reaction primarily depends on

A catalyst increases the rate of chemical reaction by providing an alt

1.	A catalyst increases the rate of chemical reaction by providing an alternative reaction pathway which lowers the activation energy than the reaction pathway in its absence. A catalyst is not consumed and therefore does not appear in the chemical equation for the reaction. A homogenous catalyst is in the same phase as the ractants whilst a heterogeneous catalyst is in a different phase. The complex [Co(NH_(3))_(3)F]^(2+)+H_(2)Oto[Co(NH_(3))_(5)(H_(2)O+F^(-)]^(3+) and Rate =k["complex"]^(a).[H^(+)]^(b) The reaction is acid catalysed , i.e. [H^(+)] does not change during the reaction . Thus, rate =k'["complex"] where, k'=[H^(+)]^(b) The value of activation energy for a chemical reaction primarily depends on
Answer» temperature nature of REACTING species collision frequency concentration of reactants Answer :B