Chemical Kineti...

For a given reaction,

A → Product,

rate = 1 x 10^-4 Ms^-1        at [A] = 0.01 M
rate = 1.41 x 10^-4   Ms^-1  at [A] = 0.02 M

Hence, rate law is 

The rate law for a reaction between the substances A and 8 is given by

rate = k[A]ⁿ [B]^m

If concentration of A is doubled and that of B is halved, the new rate as compared to the earlier rate would be 

The rate equation for the reaction,

2A + B → C

is found to be, rate = k[A] [B]

Q. The correct statement in relation to this reaction is that the

For the reaction,

2 A+B → Product

The half-life period was independent of concentration of B. On doubling the concentration A, rate increases two times. Thus, unit of rate constant for this reaction is

Which of the following statements appears to the first order reaction?

2N₂O₅(CCl₄) → 4NO₂(CCl₄) + O₂(g)

For a reaction, time of 75% reaction is thrice of time of 50% reaction. Thus, order of the reaction is

For nth order reaction,

Graphs between log (rate) and log[A₀] are of the type ([A₀] is the initial concentration)

Lines P, Q, R and S are for the order 

nA → Product

For the reaction, rate constant and rate of the reaction are equal, then on doubling the concentration of A, rate becomes,

For the simple reaction,

A → B

When [A] was changed from 0.502 mol dm^-3 to 1.004 mol dm^-3 half-life dropped from 52 s to 26 s at 300 K. Thus, order of the reaction is 

For the following reaction,

Variation of T50 with [A] is shown

Q.

After 10 min volume of N₂ (g) is 10 L and after complete reaction, volume of N₂ (g) is 50 L. Thus, T₅₀ is

Kinetics of the following reaction,

can be studied by

Graph between [B] and time t of the reaction of the type I for the reaction, A → B

Hence, graph between   and time t will be of the type

If in the fermentation of sugar in an enzymatic solution that is 0.12 M, the concentration of sugar is reduced to 0.06 M in 10 h and to 0.03 M in 20 h. Thus, order of the reaction is 

Direction (Q. No. 14) Choices for the correct combination of elements from Column I and Column II are given as options (a), (b), (c) and (d), out of which one is correct.

Direction (Q. Nos. 15-20) This section contains 3 paragraphs, each describing theory, experiments, data, etc. Six questions related to the paragraphs have been given. Each question has only one correct answer among the four given options (a), (b), (c) and (d).

Passage I 

Peroxy acetyl nitrite  is an air pollutant, as it decomposes into radicals :

A sample of polluted air is analysed for its PAN content which is reported as molecules per litre of air at 298 K.

Q.

Determine the order of the PAN decomposition

Passage I 

Peroxy acetyl nitrite  is an air pollutant, as it decomposes into radicals :

A sample of polluted air is analysed for its PAN content which is reported as molecules per litre of air at 298 K.

Q.

Rate constant of the reaction is

Passage II

H The reaction between nitric oxide (NO) and hydrogen (H₂)has been investigated by measuring the initial rate of decrease of pressure in known mixture of gases. The following results were obtained at 1000 K.

Q.

 Overall order of the reaction is

Passage II

H The reaction between nitric oxide (NO) and hydrogen (H₂)has been investigated by measuring the initial rate of decrease of pressure in known mixture of gases. The following results were obtained at 1000 K.

Q.

Rate constant of the overall reaction is

Passage III

A reaction between substances A and B is represented as:

A+B → C

Observations on the rate of this reaction are obtained as :

Q. 
Order of the reaction w.r.t. A and B respectively are

Passage III

A reaction between substances A and B is represented as:

A+B → C

Observations on the rate of this reaction are obtained as :

Q.

Rate constant of the overall reaction is

Graph between logT₅₀ (T₅₀ is half-life period) and  (a = initial concentration) for n th order reaction is of the type.

What is the value of n?

The acid catalysed hydrolysis of an organic compound A at 30°C has a time for half change of 100 min when carried out in a buffer solution at pH 5 and 10 min when carried out at pH 4. Half-life in both cases are independent of initial concentration of A If rate law is , then what is the value of (a + b)?

For a reaction, A → B, half-life time for a reaction at [A] = 0.1M is 200 s and at [A] = 0.4M it is 50 s. Thus, order of the reaction i s ......

For the reaction,

A + B → Product 

Following four experiments were carried out:

Derive the value of y.