For the reaction, , the rate law for the disappearence of will be
1.
2.
3.
4.
In a catalytic reaction involving the formation of ammonia by Haber’s process , the rate of appearence of was measured as .The rate of disappearance of H2 will be
1. 2.5×10–4 mol L–1s–1
2. 1.25×10–4 mol L–1s–1
3. 3.75×10–4 mol L–1s–1
4. 5.00×10–4 mol L–1s–1
For a chemical reaction, A products, the rate of reaction doubles when the concentration of
A is increased by 4 times. The order of reaction is
1. 4
2. 0
3. 1/2
4. 1
The units of rate constant and rate of reaction are same for :
1. First order reaction
2. Second order reaction
3. Third order reaction
4. Zero order reaction
A reaction occurs by the
following mechanism
Its order would be
1. 3/2
2. 1
3. Zero
4. 2
Which of the following represents the
expression for 3/4th life of a first order reaction?
1.
2.
3.
4.
For a reaction X(g) Y(g) + Z(g), the half life
period is 10 min. In what period of time would
the conenctration of X be reduced to 10% of
original concentration
1. 20 min
2. 33 min
3. 15 min
4. 25 min
The hydrolysis of ester is alkaline medium is a
1. 1st order reaction with molecularity 1
2. 1st order reaction with molecularity 2
3. 2nd order reaction with molecularity 1
4. 2nd order reaction with molecularity 2
Select the law that corresponds to data shown
for the following reaction A + B Products
Exp. [A] [B] Intial rate
1 0.012 0.035 0.1
2 0.024 0.070 0.8
3 0.024 0.035 0.1
4 0.012 0.070 0.8
1.
2.
3.
4.
The activation energy for the forward reaction
XY is 60kJ mol–1 and H is –20kJ mol–1, the
activation energy for the reverse recation is
1. 40kJ mol–1
2. 60kJ mol–1
3. 80kJ mol–1
4. 20kJ mol–1
The plot of log k vs helps to calculate :
1. Energy of activation.
2. Rate constant of reaction.
3. Order of the reaction.
4. Energy of activation as well as the frequency factor.
Rate constant K = 1.2×103 mol–1 L s–1 and Ea = 2.0×102 kJ mol–1. When T , A is equal
to
1. 2.0 × 102 kJ mol–1
2. 1.2 × 103 mol–1L s–1
3. 1.2 × 103 mol L–1 s–1
4. 2.4 × 103 kJ mol–1L s–1
The rate constant for a reaction 2×10–2 s–1 at 300 K and 8×10–2 s–1 at 340 K. The energy of activation of the reaction is:
1. 14.69 kJ mol–1
2. 29.39 kJ mol–1
3. 44.34 kJ mol–1
4. 22.05 kJ mol–1
The effect of a catalyst in a chemical reaction is
to change the
1. Acivation energy
2. Equilibrium concentration
3. Heat of reaction
4. Final products
For an endothermic reaction, where H represents the enthalpy of the reaction in kJ/mol, the minimum value for the energy of activation will be
1. Less than H
2. Zero
3. More than H
4. Equal to H