The dissociation of H₂O₂ is a first order reaction. The half life for '16 V H₂O₂ is 30 min, calculate the time at which the solution is 1V H₂O₂ ?

1. 120 min.

2. 90 min.

3.  60 min.

4.  150 min.

If the activation energy is 65 kJ then the reaction at 25°C is .......times fast as compared to 0°C :-

1. 2 times

2. 5 times

3. 11 times

4. 16 times

When temperature is increased from 27$°$C to 127$°$C, rate of reaction becomes doubled, then E_a will be?

1. 1.66 kcal.

2. 3.32 kcal.

3. 5.33 kcal.

4. 6.64 kcal.

A 1 L solution of 2 M acetic acid is mixed with a 1 L solution of 3 M ethyl alcohol.
The following elementary reaction takes place:

CH₃COOH + C₂H₅OH → CH₃COOC₂H₅ + H₂O

If 1 L of water is added separately to each solution before mixing,
the initial rate of reaction becomes:
 

1. Four (4) times the original rate

2. Two (2) times the original rate

3. Half (0.5) of the original rate

4. One-fourth (0.25) of the original rate

For a certain reaction, 10% of the reactant dissociates in 1 hour, 20% of the reactant dissociates in 2 hours, 30% of the reactant dissociates in 3 hours. Then the units of the rate constant is:

1.  hour^-1

2.  mol L^-1 hr^-1

3.  mol L^-1 sec^-1

4.  mol L sec^-1

Which of the following plots correctly shows how the concentration of A changes with time for a first-order reaction A → products?
 

1.		2.
3.		4.

Two reactions of the same order have equal Pre-exponential factors but their activation energies differ by 24.9 kJ/mol. Calculate the ratio between the rate constants (K₁/K₂) these reactions at 27°C :

1. 2.2 × 10⁴

2. 1/2 × 10^-4

3. 1/2 × 10⁴

4. 2.2 × 10^-4

If the activation energy of a reaction is zero, how does the rate constant of the reaction change with temperature?

1.  Increases with the increase in temperature

2. Decreases with a decrease in temperature

3. Decreases with an increase in temperature

4. Nearly independent of temperature

The rate constant of a first order reaction is 10^-3 min^-1 at 27°C. The temperature coefficient of this  reaction is 2. The rate constant at 17°C will be :

(1) 10^-3 min^-1

(2) 5  x 10^-4 min^-1

(3) 2 x 10^-3 min^-1

(4) 10^-2 min^-1

 For the pseudo first order reaction A + B $\to$ P, when studied with 0.1 M of B is given by -d[A]/dt =k[A] where K = 1.85 x 10⁴ sec^-1. Calculate the value of rate constant for second order reaction :

(1) 1.85 x 10⁴

(2) 1.85 x 10^-4

(3) 1.85 x 10^-5

(4) 1.85 x 10⁵