Chemical Kinetics

Which one of the given statement for order of reaction is not correct?

The equation

k = $\left(6.5*10^{12}{s}^{-1}\right)e^{-26000K/T}$  

Is followed for the decomposition of compound A. The activation energy for the reaction is________ kJ mol^-1 [nearest integer]        (Given : R = 8.314 JK^-1 mol^-1)

For a reaction P → Q, the Ea for the forward reaction and backward reaction is 15KJ/mol and 5KJ/mol, respectively, potential energy of P is 8KJ/mol, then the heat of reaction (in kJ) is:

What is the difference between reaction rate and rate constant?

Can the order and molecularity of a reaction be the same?

What is reaction kinetics?

For the first order reaction A → 2B, 1 mole of reactant A gives 0.2 moles of B after 100 minutes. The half life of the reaction is _____ min. (Round off to the Nearest Integer).
[Use : ln2 = 0.69, ln 10 = 2.3 Properties of logarithms : ln x? = y ln x; ln(x/y) = lnx – lny ]

Given below are two statements: one is labelled as Assertion A and the other is labelled as Reason R:
Assertion A: A reaction can have zero activation energy.
Reason R: The minimum extra amount of energy absorbed by reactant molecules so that their energy becomes equal to threshold value, is called activation energy.

In the light of the above statements, choose the correct answer from the options given below:

For a certain reaction, the rate = k[A]²[B]. When the initial concentration of A is tripled keeping concentration of B constant, the initial rate would

The number of molecules with energy greater than the threshold energy for a reaction increases five fold by a rise of temperature from 27°C to 42°C. Its energy of activation in J/mol is (Take in 5 = 1.6094; R = 8.314 J mol⁻¹ K⁻¹)