The rate of constant of the reaction A → B is  0.6 x 10^-3 mole per second. If the concentration of A is 5 M then concentration of B after 20 min is 

• 1.08 M

• 3.60 M

• 0.36 M

• 0.36 M

The half -life of a substance in a certain enzyme catalysed reaction is 138 s. The time required for the concentration of the substance to fall from 1.28 mg L^-1 is 

• 414 s

• 552 s 

• 690 s

• 690 s

The rate of reaction 2N₂O₃ → 4 NO₂ + O₂ can be written in three ways



The relationship between k and k' and between k and k'' are 

• k' = 2k ; k' = k

• k' = 2k; k" = k/2

• k' = 2k; k' = 2k

• k' = 2k; k' = 2k

284.

The unit of rate constant for a zero order reaction is 

•  mol L^-1 s^-1

• L mol^-1 s^-1

• L² mol^-2 s^-1

• L² mol^-2 s^-1

For the reaction


the value of the rate of disappearance of N₂O₅ is given as 

• 6.25 x 10^-3 mol L^-1s^-1 and 6.25 x 10^-3 mol L^-1 s^-1

• 1.25 x 10^-2 mol L^-1s^-1 and 6.25 x 10^-3 mol L^-1 s^-1

• 6.25 x 10^-3 mol L^-1s^-1 and 3.125 x 10^-3 mol L^-1 s^-1

• 6.25 x 10^-3 mol L^-1s^-1 and 3.125 x 10^-3 mol L^-1 s^-1

For an endothermic reaction, energy of activation is E_a and enthalpy of reaction is ΔH (both of these in kJ/mol). Minimum value of E_a will be

• less than ΔH

• equal to ΔH

• more than ΔH

• more than ΔH

During the kinetic study of the reaction, 2A + B --> C+ D,  following results were obtained 

• rate = k[A]²[B]

• rate = k [A][B]

• rate = k[A]²[B]²

• rate = k[A]²[B]²

The rate of the reaction,

2NO + Cl₂ → 2NOCl is given by the rate equation, rate = k[NO]²[Cl₂]

The value of the rate constant can be increased by

• increasing the temperature

• increasing the concentration of NO

• increasing the concentration of the Cl₂

• increasing the concentration of the Cl₂

Half-life period of a first order reaction is 1386 s. The specific rate constant of the reaction is

• 5.0 x 10^-3s^-1

• 0.5 x 10^-2 s^-1

• 0.5 x 10^-3 s^-1

• 0.5 x 10^-3 s^-1

For the reaction, A+B → Products, it is observed that

1) On doubling the initial concentration of A only, the rate of reaction is also doubled and

2) On doubling the initial concentrations of both A and B , there is a change by a factor of 8 in the rate of the reaction.

The rate of this reaction is, given by

• rate = k [A]²[B]

• rate = k[A][B]²

• rate = k[A]²[B]²

• rate = k[A]²[B]²