Q. No.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.
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
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
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
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.
The correct expression for the 3/4th life of a first-order reaction is:
\(1 . \frac{k}{2 . 303} log \frac{4}{3}\)
\(2 . \frac{2 . 303}{k} log \frac{3}{4}\)
\(3 . \frac{2 . 303}{k} log\) \(4\)
\(4 . \frac{2 . 303}{k}\) \(log\) \(3\)
The activation energies of the forward and backward reactions in the case of a chemical reaction are 30.5 and 45.4 KJ/mol respectively. The reaction is
1. Exothermic
2. Endothermic
3. Neither exothermic nor endothermic
4. Independent of temperature
Mechanism of a hypothetical reaction
is given below
(i)
(ii)
(iii)
The overall order of the reaction will be
1. 1
2. 2
3. 0
4. 1.5
The activation energy of a reaction can be determined from the slope of the graph between :
1. ln K vs T
2. ln vs T
3. ln K vs
4.
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