Answer
All of these are ways that a catalyst might act to increase the rate of the reaction
Explanation
Arrhenius equation for rate constant is
k = Ae-Ea/RT
where,
A = frequency factor
Ea = Activation energy
R = gas constant , 8.314J/K mol
T = Temperature in K
From this equation we know that , by increasing frequency factor (factor of collisions between molecules) rate constant is increased and by decreasing activation energy rate constant is increased.
By adding catalyst , the reaction path way is changed and because of change in reaction path way activation energy for both forward and reverse rection decreased and freqecy factor also increased.
Therefore,
So, a catalyst increase rate of reaction by w,x,y and z.
Can someone help me? A catalyst can not increase the rate of a reaction W. by...
Which statement below is true only for a homogeneous catalysts? a. A homogeneous catalyst increase the rate of reaction by providing an alternative pathway with a lower activation energy. b. A homogeneous catalyst is a solid substance to which liquid or gaseous reactants will adhere to the surface of the catalyst. c. A homogeneous catalyst is when the catalyst is in the same physical state as the reactant. d. A homogeneous catalyst will eventually be consumed in a chemical reaction.
A catalyst increases the rate of a reaction by providing a different reaction pathway that lowers only the activation energy. raises only the energy of the products. lowers only the energy of the reactants and products. All of these are affected by the presence of a catalyst.
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