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

For the reaction, N₂ + 3H₂ → 2NH₃, If  the value of  would be

• 3 x 10^-4 mol L^-1 s^-1

• 4 x 10^-4 mol L^-1s^-1

•  6 x 10^-4 mol L^-1s^-1

•  6 x 10^-4 mol L^-1s^-1

In the reaction,


The rate of appearance of bromine (Br)₂ is related to rate of disappearnace of bromide ions as following

The rate constant k₁ and k₂ for two different reactions are 10¹⁶. e^-2000/T and 10¹⁵.e^-1000/T respectively. The temperature at which k₁ = k₂

• 1000 K 

• 2000/2.303 K 

• 2000 K 

• 2000 K 

The bromination of acetone cytosine and guanine solution is represented by this equation.
 CH₃COCH₃ (aq) + Br₂ (aq) →CH₃COCH₂Br (aq) + H⁺ (aq) + Br^- (aq)
These kinetic data were obtained for given reaction concentrations.

• Rate = k[CH₃COCH₃][H⁺]

• Rate = k[CH=COCH₃][Br₂]

• Rate = k [CH₃COCH₃][Br₂][H⁺]

• Rate = k [CH₃COCH₃][Br₂][H⁺]

598.

The reaction of hydrogen and iodine monochloride is given as:
H₂ (g) + 2ICl (g) → 2 HCl (g)  + I₂ (g)
This reaction is of first order with respect to H₂ (g) and ICI (g), following mechanisms were proposed:

Mechanism A:
H₂ (g) + 2 ICl (g)  → 2 HCl (g) + I₂ (g) 

Mechanism B:
H₂ (g) + ICl (g) →HCl (g) + HI (g) ;slow
HI (g) + ICl (g)  → HCl (g) + I₂ (g); fast

Which of the above mechanism (s) can be consistent with the given information about the reaction? 

• B only

• A and B both

• Neither A nor B

• Neither A nor B

In a first order reaction A →B, if k israte constant and initial concentration of the reactant A is 0.5 A M then the half -life is : 

• 0.693/0.5 k

• log2/k

• 
• 

If 60% of a first order reaction was completed in 60 min, 50% of the same reaction would be completed in approximately:

• 50 min

• 45 min

• 60 min

• 60 min