A catalyst alters the rate of a chemical reaction by:
Shifting the equilibrium towards product formation.
Increasing the concentration of reactants.
Changing the activation energy of the reaction.
Altering the enthalpy change of the reaction.
Related Questions
Which of the following is an example for heterogeneous catalysis reaction?
Hydrolysis of ester in presence of acid
Hydrolysis of ester in presence of base
Haber-Bosch process
Decomposition of hydrogen peroxide in presence of Iodide ion
A catalyst alters the rate of a chemical reaction by:
Shifting the equilibrium towards product formation.
Increasing the concentration of reactants.
Changing the activation energy of the reaction.
Altering the enthalpy change of the reaction.
Which acts as poison for Pd-charcoal in Lindlar’s catalyst?
Lead
Quinoline
Palladium
Calcium Carbonate
A catalyst
Lowers the activation energy
Changes the rate constant
Changes the product
Itself destroys in the reaction
An example of homogeneous catalysis is
Hydrogenation of ethene using nickel
Manufacture of ammonia by Haber's process
Destruction of ozone by chlorine radicals
Hydrolysis of sucrose using acid
In a chemical reaction, catalyst
Decrease the energy of activation
Increases the energy of activation
Does not change energy of activation
None of the above
A catalyst for a reversible reaction is a substance that :
Supplies energy to the reaction
Decreases the time to reach equilibrium
Increases the equilibrium concentration of the products
Change the equilibrium constant of the reaction
Catalyst used in Haber’s process is
Nickel powder
Iron and molybdenum powder
Black lead
Iodine
In the titration between oxalic acid and acidified potassium permanganate, the manganous salt formed during the reaction catalyses the reaction. The manganous salt acts as :
A promoter
A positive catalyst
An autocatalyst
None of these
In Haber’s process for manufacture of ammonia, the reaction is usually carried at about . If a temperature of about was used then
A catalyst would be of no use at all at this temperature
The rate of formation of ammonia would be too slow
No ammonia would be formed at all
The percentage of ammonia in the equilibrium mixture would be too low
