Chemical Kineti...

Direction : Each question has four choices (a), (b), (c) and (d), out of which ONLY ONE is correct.

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?

2N₂ O₅ (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