Chemical Kineti...

Direction (Q. Nos. 1-13) This section contains multiple choice questions. Each question has four choices (a), (b), (c) and (d), out of which ONLY ONE is correct

Q. In the following reaction, which has maximum rate w.r.t. rate of disappearance of NH₃?
4NH₃ + 50₂ →  4NO + 6H₂O

The rate of formation of NO(g) in the reaction, 2NOBr(g) → 2NO(g) + Br₂(g) was reported as 1.6 x 10^-4 Ms^-1. Thus, rate of the reaction is 

Rate of formation of SO₃ in the reaction below is 100 kg min^-1.
2SO₂ + O₂ → 2SO₃
Hence, rate of disappearance of SO₂ will be:

The following reaction can take place in both directions:

For the forward reaction, the rate varies with the concentration of A as and for the backward reaction,

Hence, net reaction rate is:

For a reaction, xA → yB, rate of disappearance of ‘A’ is related to the rate of appearance of 'B' by the equation 

Thus, x and y respectively are

For the reaction,

H₂(g) + A₂(g)  2H(g) + A₂(g)

k_f = 2.2 x 10⁴ L mol^-1s^-1 and K_c = 1.00 x 10^-4 at 3000 K. Thus, k_b is 

For a reaction,

hen x, y and z are 

For the reaction,

2N₂O₅(g) → 4NO₂ (g) + O₂(G)

Thus,

The decomposition of acetaldehyde is given by the following reaction:

CH₃CHO(g) → CH₄(g) + CO(g)

Rate of the reaction with respect to the pressure of the reactant is 

For the reaction, 

 then rate law is

For gaseous reaction, the rate can be expressed as

The initial rates of reaction for the equation, 2A + B → Products.

Products were determined under various initial concentrations of reactants.

Thus, rate law is equal to

For the reaction, A + 2B → Product, the reaction rate was halved on doubling the concentration of A. Thus, order w.r.t. A is

Direction (Q. Nos. 14 and 15) This section contains a passage describing theory, experiments, data, etc. Two questions related to the paragraph have been given. Each question has only one correct answer out of the given 4 options (a), (b), (c) and (d)

Passage 

The decomposition of NO₂ at 400 K proceeds at a of rate of 5.4 x 10 ^-5 mol L^-1 s^-1 when [NO₂] = 0.01 mol^-1

2 NO₂(g) → 2NO(g ) + O₂(g).

Q. What is the rate law when observed rate is 1.35 x 10^-5 mol L^-1 s^-1 at [NO₂] = 0.005 mol L^-1?

The decomposition of NO₂ at 400 K proceeds at a of rate of 5.4 x 10 ^-5 mol L^-1 s^-1 when [NO₂] = 0.01 mol^-1

2 NO₂(g) → 2NO(g ) + O₂(g).

Q. Rate constant of the reaction will be 

Direction (Q. Nos. 16-18) This section contains 3 questions. When worked out will result in one integer from 0 to 9 (both inclusive)

In the following reaction

Q. Where negative sign indicates rate of disappearance of the reactant. What is the value of x/y ?

The reaction rate is defined as the rate at which the concentration of the reactants __________ with time or the concentration of products ___________ with time.

In a certain polluted atmosphere containing O₃ at a steady concentration of 2.0 x 10^-6 M, the hourly production of O₃ by all sources was estimated as 7.2 x 10^-15 M. If the only mechanism for destruction of O₃ in the second-order reaction is

2O₃ → 3O₂

then rate constant for destruction reaction, defined by the rate law for - Δ[O₃]/Δf is x * 10^-7 M^-1 s^-1 . What is the value of x?

Only One Option Correct Type

This section contains 2 multiple choice questions. Each question has four choices (a), (b), (c) and (d), out of which ONLY ONE is correct

For a reversible reaction, net rate is 

hence given reaction is 

Reaction kinetics deals with the study of