When temperature is increased from 27C to 127C, rate of reaction becomes doubled, then Ea will be?
1. 1.66 kcal.
2. 3.32 kcal.
3. 5.33 kcal.
4. 6.64 kcal.
If 2M, 1L solution of acetic acid is added to 3M, 1L ethyl alcohol then the following elementary reaction takes place.
CH3COOH + C2H5OH CH3COOC2H5 + H20
If each solution is diluted by 1 litre then the initial rate becomes how many times:-
(1) 4
(2) 2
(3) 0.5
(4) 0.25
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
For a first order reaction A product :
(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
The activation energy of a reaction is zero. The rate constant of the reaction is :
1. increases with an increase in temperature
2. decreases with a decrease in temperature
3. decreases with an increase in temperature
4. is 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 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
Time required to decompose half of the substance for (n)th order reaction is propotional to:-
1. 1/an-1
2. a1-n
3. an-1
4. Both 1 and 2
What is the activation energy for reverse reaction on the basis of given data ?
N2O4(g) 2NO2(g) ΔH = +54kJ
Ea(forward) = +57.2 kJ
1. -54 kJ
2. +3.2 kJ
3. 60.2 kJ
4. 111.2 kJ