Chemical Kineti...

A first order reaction is given as $$A\rightarrow$$ products. Its integrated equation is:

In the first order reaction, 75% of the reactant gets disappeared in 1.386 h. The rate constant of the reaction is:

The first order integrated rate equation is:

Assertion: Reactions happen faster at higher temperatures.
Reason: As temperatures increase, there is also an increase in the number of collisions with the required activation energy for a reaction to occur.

The minimum energy required for molecules to react and form compounds can be defined as :

The time required for $$100\%$$ completion of zero order reaction is:

In a reaction, the potential energy of the reactants is 40 kJ/mol, the potential energy of the products is 10 kJ/mol and the potential energy of the activated complex is 55 kJ/mol. What is the activation energy for the reverse reaction?

How an increase in concentration is related to number of collisions?

The addition of a catalyst to a reaction changes which of the following?