Chemical Kinetics and Nuclear Chemistry
Choose the correct option:
Which one of the following statements is correct?
2A + B → Products
(in mol L–1)
(in mol L–1)
|Initial Rate of reaction
(in mol L–1 min–1)
|I||0.10||0.20||6.93 × 10–3|
|II||0.10||0.25||6.93 × 10–3|
|III||0.20||0.30||1.386 × 10–2|
The time (in minutes) required to consume half of A is:
X2 + Y2 → 2XY is given below :
(i) X2 → X + X(fast)
(ii) X + Y2 ⇌ XY + Y (slow)
(iii) X + Y → XY (fast)
The overall order of the reaction will be:
|Initial rate of
formation of C
(mol L−1S−1 )
|1.2 × 10−3
1.2 × 10−3
2.4 × 10−3
The rate law for the formation of C is
The rate of a reaction doubles when its temperature changes from 300 K to 310 K. Activation energy of such a reaction will be :
(R = 8.314 JK−1 mol−1 and log 2 = 0.301)
In the reaction,
P + Q → R + S
the time taken for 75% reaction of P is twice the time taken for 50% reaction of P. The concentration of Q varies with reaction time as shown in the figure. The overall order of the reaction is
is plotted for a straight line with a slope −6670 k is obtained. The activation energy for this reaction will be (R = 8.314 JK−1mol−1).
What is the activation energy for a reaction if its rate doubles when the temperature is raised from 20°C to 35°C? (R = 8.314 J mol−1 K−1)
An organic compound undergoes first-order decomposition. The time taken for its decomposition to 1/8 and 1/10 of its concentration are and respectively.
What is the value of
The half-life period of the reaction is
Assertion : A catalyst increases the rate of a reaction.
Reason : in presence of a catalyst, the activation energy of the reaction decreases.
Bombardment of aluminium by particle leads to its disintegration in two ways, (i) and (ii) as shown. Products X,Y and Z respectively are,
Plots showing the variation of the rate constant (k) with temperature (T) are given below. The plot that follows Arrhenius equation is
The concentration of R in the reaction R→P was measured as a function of time and the following data is obtained
The order of the reaction is
For a first order reaction the temperature (T) dependent rate constant (k) was found to follow the equation The pre-exponential factor and the activation energy respectively, are
Under the same reaction conditions, initial concentration of 1.386 mol dm-3 of a substance becomes half in 40 seconds and 20 seconds through first order and zero order kinetics, respectively, Ratio of the rate constants for first order and of the reactions is
The plot of atomic number (y-axis) versus number of neutrons (x-axis) for stable nuclei shows a curvature towards x-axis from the line of 45o slope as the atomic number is increased.
Proton − proton electrostatic repulsion begin to overcome attractive forces involving protons and neutrons and neutrons in heavier nuclides.
Concentration of A changes from 0.1 M to 0.025 M in 40 minutes. Find the rate of reaction of A when concentration of A is 0.01 M
(A) Rate = −d[N2]/dt = −1/3d[H2]/dt = 1/2d[NH3]/dt
(B) Rate = −d[N2]/dt = −3d[H2]/dt = 2d[NH3]/dt
(C) Rate = d[N2]/dt = 1/3d[H2]/dt = 1/2d[NH3]/dt
(D) Rate = −d[N2]/dt = −d[H2]/dt = d[NH3]/dt