For a first order reaction A ⟶ B the rate constant is x min⁻¹. If the initial concentration of A is 0.01M, the concentration of A after one hour is given by the expression.

The addition of a catalyst during a chemical reaction alters which of the following quantities?

Consider the following statements:
(i) increase in concentration of the reactant increases the rate of a zero order reaction.
(ii) rate constant k is equal to collision frequency A if E_a = 0
(iii) rate constant k is equal to collision frequency A if E_a = ∞
(iv) a plot of ln (k) vs T is a straight line.
(v) a plot of ln (k) vs \(\left( \frac { 1 }{ T } \right) \) is a straight line with a positive slope.
Correct statements are

Which of the following statement is not correct?

For an exothermic chemical process occurring in 2 steps as
(i) A +B ⟶ X (slow) ;
(ii) X ⟶  AB (fast)
The progress of the reaction can be best described by (x- intermediate).

During a chemical reaction, the concentration of reaction  _____.

The half life period of a first order reaction is 10 minutes. Then its rate constant is  _____.

If the activation energy is high then the rate of the reaction is  _____.

Rate law cannot be determined from balanced chemical equation if ______.

The value of rate constant of a pseudo first order reaction______.

By the order of reaction we mean _______.

For a reaction 2A + B ⟶ 3C, express the rate of reaction in terms of formation of the product _______.

The minimum energy that all colliding molecules must possess so as to make the collisions more effective and successful is_______.

The time required for 50% completion of the reaction is known as _______.

If [A] is the concentration of A at any time t and [A_o] is the concentration at t = 0, then for the first order reaction, the rate equation can be written as ______.

Define average rate and instantaneous rate.

What is an elementary reaction? Give the differences between order and molecularity of a reaction.

Describe the graphical representation of first order reaction.

The rate law for a reaction of A, B and C has been found to be rate = k[A]²[B][L]^3/2 How would the rate of reaction change when
(i) Concentration of [L] is quadrupled
(ii) Concentration of both [A] and [B] are doubled
(iii) Concentration of [A] is halved
(iv) Concentration of [A] is reduced to \(\left(\frac{1}{3}\right)\) and concentration of [L] is quadrupled.

What is the study of chemical kinetics used for?

Why is instantaneous rate preferred over average rate?

The decomposition reaction of ammonia gas on platinum surface has a rate constant R = 2.5 x 10^-4mol L^-1. What is the order of the reaction.

How does the value of rate constant vary with reactant constant.

Consider the oxidation of nitric oxide to form NO₂
2NO_(g) + O_2(g) ➝2NO_2(g)
(a). Express the rate of the reaction in terms of changes in the concentration of NO,O₂ and NO₂.
(b). At a particular instant, when [O₂] is decreasing at 0.2 mol L⁻¹s⁻¹ at what rate is [NO₂] increasing at that instant?

The rate of the reaction X + 2y→ product is 4 x 10^-3 mol L^-1S^-1, if [X] = [Y] = 0.2M and rate constant at 400K is 2 x 10^-2s^-1, What is the overall order of the reaction.

For a reaction x + y + z\(\longrightarrow \) products the rate law is given by rate =k[x]^3/2[y]^1/2. What is the overall order of the reaction and what is the order of the reaction with respect to z.

Explain briefly the collision theory of bimolecular reactions.

The decomposition of Cl₂O₇ at 500K in the gas phase to Cl₂ and O₂ is a first order reaction. After 1 minute at 500K, the pressure of Cl₂O₇ falls from 0.08 to 0.04 atm. Calculate the rate constant in s^-1

Identify the order for the following reactions
(i) Rusting of Iron
(ii) Radioactive disintegration of ₉₂U²³⁸
(iii) 2A+3B⟶ products ;rate = k[A]^1/2[B]²

(i) Molecularity of any reaction is not equal to zero. Why?
(ii) For which type of reactions, order, and molecularity have the same value?

The rate constant, the activation energy and frequency factor of a chemical reaction at 25^oC are 3.0 x 10^-4 S^-1; 104.4 kJ mol^-1  and 6.0 x 10¹⁴ S^-1 respectively. What is the value of the rate constant when T ⟶ ∞?

A first order reaction is found to have a rate A constant k = 7.39 x 10^-5 S^-1. Find the half life of this reaction.

A reaction is second order with respect to a reactant. How is the rate of reaction affected if the concentration of the reactant is
(i) doubled (ii) reduced to half

A reaction is first order in A and second order in B.
(i) Write the differential rate equation.
(ii) How is rate affected on increasing the concentration of B three times?
(iii) How is the rate affected when the concentrations of both A and B are doubled?

Show that in case of first order reaction, the time required for 99.9% completion is nearly ten times the time required for half completion of the reaction.

The rate constant for a first order reaction is 1.54 x 10^-3 s^-1. Calculate its half life time.

A zero order reaction is 20% complete in 20 minutes. Calculate the value of the rate constant. In what time will the reaction be 80% complete?

In a pseudo first order hydrolysis of ester in water, the following results were obtained.

(i) Calculate the average rate of reaction between the time interval 30 to 60 seconds.
(i) Calculate the pseudo first order rate constant for the hydrolysis of ester.

Write an account of the Arrhenius equation for rates of chemical reactions. 

The conversion of molecules x to y follows second order kinetics. Its concentration of x is increased to three times how will it affect the rate of formation of y?
For the reaction x ➝ y as it follows second order kinetics wherefore the rate of formation of y?

The specific reaction rates of a chemical reaction are 2.45 x 10^-5 sec^-1 at 273 K and 16.2 x 10^-4 sec^-1 at 303 K. Calculate the activation energy.

Rate constant of a first order reaction is 0.45 sec^-1, calculate its half life.