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
For a first-order reaction, the time required for 99.9% of the reaction to take place is nearly :
(1) 10 times that required for half of the reaction
(2) 100 times that required for two-third of the reaction
(3) 10 times that required for one-fourth of the reaction
(4) 20 times that required for half of the reaction