Q. No.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
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
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
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.
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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