The decomposition of phosphine (PH₃) on tungsten at low pressure is a first order reaction. It is because the _____.

For a reaction Rate = k[acetone]^3/2 then unit of rate constant and rate of reaction respectively is _______.

In a first order reaction x ⟶ y; if k is the rate constant and the initial concentration of the reactant x is 0.1M, then, the half life is_____.

Predict the rate law of the following reaction based on the data given below 
2A+B⟶C+3D

During the decomposition of H₂O₂ to give dioxygen, 48 g O₂ is formed per minute at certain point of time. The rate of formation of water at this point is

A+B \(\longrightarrow \) C; ∆H = 60 kJ mol^-1 Ea_f = 150 kJ. What is the activation energy of the backward reaction?

Which order reaction obeys the expression \({ t }_{ \frac { 1 }{ 2 } }\alpha \frac { 1 }{ \left[ A \right] } ?\)

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

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

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

Activation energy of a reactant is reduced by ________.

Two reactions A ⟶ B and C ⟶ D has the energy of activation 40 kJ and 60 kJ respectively. Which of the following statement is correct?
a) Comparison of rate cannot be determined
b) The reaction A ⟶ B proceeds at a faster rate compared to the reaction C ⟶ D
c) The reaction A ⟶ B proceeds at a slower rate compared to the reaction C ⟶ D.
d) Comparison of rate cannot be determined.

Assertion: A positive catalyst increases the rate of reaction.
Reason: A positive catalyst alters reaction mechanism and decreases activation energy.
Codes:
a) Both assertion and reason are true and the reason is the correct explanation of the assertion.
b) Both assertion and reason are true but the reason is not the correct explanation of the assertion.
c) Assertion is true but reason is false.
d) Both assertion and reason are false.

Assertion: Order and molecularity are same.
Reason: Order is determined experimentally and molecularity is the sum of the stoichiometric coefficient of rate determining elementary step.
Codes:
a) Both assertion and reason are true and the reason is the correct explanation of the assertion.
b) Both assertion and reason are true but the reason is not the correct explanation of the assertion.
c) Assertion is true but reason is false.
d) Both assertion and reason are false.

Assertion: A catalyst is a substance which alters the rate of a reaction.
Reason: In the presence of catalyst the energy of activation is increased.
Codes:
a) Both assertion and reason are true and the reason is the correct explanation of the assertion.
b) Both assertion and reason are true but the reason is not the correct explanation of the assertion.
c) Assertion is true but reason is false.
d) Both assertion and reason are false.

Consider the following statements and identify the incorrect statement(s).
(i) Decomposition of H₂O₂ is an II order reaction
(ii) t_1/u  is independent of initial concentration of a reaction.
(iii) Fractional order reactions are observed depending on their rates.
(iv) Rate = k [A]^p [B]^q; p + q = order.
a) only (ii)
b) both (ii) and (iii)
c) only (i)
d) None of these

Define half life of a reaction. Show that for a first order reaction half life is independent of initial concentration.

Describe the graphical representation of first order reaction.

For a chemical reaction, Variation in the concentration In[A] Vs time in seconds is given as

(i) What is the order of the reaction?
(ii) What is the unit of rate constant K?
(iii) Give the relationship between k and \({ t }_{ \frac { 1 }{ 2 } }\)

If the rate of a reaction gets doubled as the temperature is increased from 27^oC to 37^oC. Find the activation energy of reaction?

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

From the rate expression for the following reactions, determine their order of reaction and the dimensions of the rate constants.
(i) 3NO_(g) ⟶ N₂O_(g) Rate = K[NO]²
(ii) H₂O_2(aq) + 3I^-_(aq) +2H⁺ ⟶ 2H₂O_(l) +I₃^- Rate = K[H₂O₂][I^-]
(iii) CH₃CHO_(g) ⟶ CH_4(g) + CO_(g) Rate = K[CH₃ CHO]^3/2
(iv) C₂H₅Cl_(g) ⟶ C₂H_2(g) + HCl_(g) Rate = K[C₂H₅Cl]²

The time for half change in a first order decomposition of a substance A is 60 seconds. Calculate the rate constant. How much of A will be left after 180 seconds?

Benzene diazonium chloride in aqueous solution decomposes according to the equation \({ C }_{ 6 }{ H }_{ 5 }{ N }_{ 2 }Cl\longrightarrow { C }_{ 6 }{ H }_{ 5 }Cl+{ N }_{ 2 }\)Starting with an initial concentration of 10g L^-1, the volume of N₂ gas obtained at 50 °C at different intervals of time was found to be as under:

Show that the above reaction follows the first order kinetics. What is the value of the rate constant?

The initial rate of a first order reaction is 5.2 x 10^-6 mol lit^-1 S^-1 at 298 K. When the initial concentration of reactant is 2.6 x 10^-3 mol.lit^-1, calculate the first order rate constant of the reaction at the same temperature.