JEE Questions for Chemistry Chemical Kinetics Quiz 8 - MCQExams.com

Units of rate constant for first and zero order reactions in terms of molarity M and time in seconds are respectively
  • sec–1, M sec–1
  • sec–1, M
  • M sec–1, sec–1
  • M, sec–1
Half-life of a reaction is found to be inversely proportional to the cube of initial concentration. The order of reaction is
  • 4
  • 3
  • 5
  • 2
Consider the chemical reaction, N2(g) + 3H2(g) → 2NH3 The rate of this reaction can be expressed in terms of time derivative of concentration of N2 (g), H2 (g) or NH2 (g). Identify the correct relationship amongst the rate expressions

  • Chemistry-Chemical Kinetics-1698.png
  • 2)
    Chemistry-Chemical Kinetics-1699.png

  • Chemistry-Chemical Kinetics-1700.png

  • Chemistry-Chemical Kinetics-1701.png
The reaction 2N2O5 → 2N2O4 + O2 is
  • Bimolecular and second order
  • Unimolecular and first order
  • Bimolecular and first order
  • Bimolecular and zero order
The activation energy for a simple chemical reaction A → B is Ea in forward direction. The activation energy for the reverse reaction
  • is negative of Ea
  • is always less than Ea
  • can be less than or more than Ea
  • is always double of Ea

Chemistry-Chemical Kinetics-1702.png
  • A is adsorption factor
  • Ea is energy of activation
  • R is Rydberg constant
  • K is equilibrium constant
Rate of first order reaction depends upon
  • time
  • concentration of reactant
  • temperature
  • all the three

Chemistry-Chemical Kinetics-1703.png

  • Chemistry-Chemical Kinetics-1704.png
  • 2)
    Chemistry-Chemical Kinetics-1705.png

  • Chemistry-Chemical Kinetics-1706.png

  • Chemistry-Chemical Kinetics-1707.png
For the reaction, 2A + B → Products, the following initial rates were obtained at various initial concentrations:
Chemistry-Chemical Kinetics-1708.png
  • Rate = k[A]2[B]o
  • Rate = k[A][B]
  • Rate = k[A]2[B]
  • Rate = 2 k[A][B]2
For the above reaction, the specific rate constant is
  • 23 sec−1
  • 0.46 l mol−1 sec−1

  • Chemistry-Chemical Kinetics-1709.png

  • Chemistry-Chemical Kinetics-1710.png
If initial concentration is reduced to 1/4th in a zero order reaction, the time taken for half the reaction to complete
  • remains same
  • becomes 4 times
  • becomes one-fourth
  • doubles
The rate constant for the reaction 2N2O5 → 4NO2 + O2 is 3.0 × 10–5 sec–1. If the rate is 2.40 × 10–5 mol litre–1 sec–1, then the concentration of N2O5 (in mol litre–1) is
  • 1.4
  • 1.2
  • 0.04
  • 0.8
For a first order reaction we have k = 100 sec-1. The time for completion of 50% reaction is:
  • 1m sec
  • 4 m sec
  • 7 m sec
  • 10 m sec
In the first order reaction, 75% of the reactant disappeared in 1.386 h. Calculate the rate constant of reaction.

  • Chemistry-Chemical Kinetics-1715.png
  • 2)
    Chemistry-Chemical Kinetics-1716.png

  • Chemistry-Chemical Kinetics-1717.png

  • Chemistry-Chemical Kinetics-1718.png
The decomposition of a substance follows first order kinetics. Its concentration is reduced to 1/8th of its initial value in 24 minutes. The rate constant of the decomposition process is

  • Chemistry-Chemical Kinetics-1720.png
  • 2)
    Chemistry-Chemical Kinetics-1721.png

  • Chemistry-Chemical Kinetics-1722.png

  • Chemistry-Chemical Kinetics-1723.png
The reaction A → B follows first order kinetics. The time taken for 0.8 mole of A to produce 0.6 mole of B is 1 hour. What is the time taken for conversion of 0.9 mole of A to produce 0.675 mole of B?
  • 1 hour
  • 0.5 hour
  • 0.25 hour
  • 2 hours
In a first order reaction the concentration of the reactant decreases from 800 mol/dm3 to 50 mol/dm3 in 2 × 107 sec. The rate constant of the reaction in sec-1 is

  • Chemistry-Chemical Kinetics-1726.png
  • 2)
    Chemistry-Chemical Kinetics-1727.png

  • Chemistry-Chemical Kinetics-1728.png

  • Chemistry-Chemical Kinetics-1729.png
An endothermic reaction A → B has an activation energy of 15 kcal/mole and the energy of reaction is 5 kcal/mole. The activation energy for the reaction B → A is
  • 20 kcal/mole
  • 15 kcal/mole
  • 10 kcal/mole
  • zero
The rate constant of a reaction at temperature 200 K is 10 times less than the rate constant at 400 K. What is the activation energy (Ea) of the reaction?
  • 1842.4 R
  • 921.2 R
  • 460.6 R
  • 230.3 R
In a second order reaction, first order in each reactant A and B, which one of the following reactant mixtures will provide the highest initial rate?
  • 0.1 mol of A and 0.1mol of B in 0.1 litre solvent
  • 0.2 mol of A and 0.2 mol of B in 0.1 litre solvent
  • 1.0 mol of A and 1.0 mol of B in 1 litre solvent
  • 0.1 mol of A and 0.1 mol of B in 0.2 litre solvent
The rate law for the reaction RCl + NaOH →ROH + NaCl is given by Rate = k [RCl]. The rate of this reaction
  • is doubled by doubling the concentration of NaOH
  • is halved by reducing the concentration of RCl by one half
  • is increased by increasing the temperature of the reaction
  • in unaffected by change in temperature
A reaction has a rate constant of 0.5 mol-1 dm3 min-1. If initial concentration of the reactant is 0.2 mol dm-3, half life of the reaction is
  • 1.4 min
  • 10 min
  • 15 min
  • 20 min
The rate constant of nth order has units

  • Chemistry-Chemical Kinetics-1734.png
  • 2)
    Chemistry-Chemical Kinetics-1735.png

  • Chemistry-Chemical Kinetics-1736.png

  • Chemistry-Chemical Kinetics-1737.png

Chemistry-Chemical Kinetics-1739.png
  • E1 > E2
  • E1 < E2
  • E1 = 2E2
  • E1 = E2
Consider the following statements: For a second order reaction: 2A → P
Chemistry-Chemical Kinetics-1740.png
  • 1 and 2
  • 1 and 3
  • 2 and 3
  • 1, 2 and 3
The rate of reaction of spontaneous reaction is generally very slow. This is due to the fact that..
  • the equilibrium constant of the reaction is < 1
  • the activation energy of the reaction is large
  • the reaction are exothermic
  • the reaction are endothermic

Chemistry-Chemical Kinetics-1742.png
  • 0.2 × 10-4
  • -0.2 × 10-4
  • 0.1 × 10-4
  • 0.3 × 10-4

Chemistry-Chemical Kinetics-1744.png
  • 0.012 atm min-1
  • 0.024 atm min-1
  • 0.006 atm min-1
  • 0.003 atm min-1
For the reaction A + B + C → Products, Rate = K [A]1/2 [B]1/3 [C]. The order of reaction is
  • 3
  • 1
  • 5/6
  • 11/6
For a reaction pA + qB → Products. Rate = K[A]m[B]n . Then
  • (p + q) = (m + n)
  • (p + q) ≠ (m + n)
  • (p + q) > (m + n)
  • (p + q) = (m + n) or (p + q) ≠ (m + n)
0:0:1


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