Chemical Kinetics Free Question Bank
In a reaction, A + B → Product, rate is doubled when the concentration of B is doubled, and rate increases by a factor of 8 when the concentrations of both the reactants (A and B) are doubled, rate law for the reaction can be written as [CBSE AIPMT 2012]
A Rate = k[A] [B]B Rate = k[A]2[B]
C Rate = k[A][B]2
D Rate = k[A]2[B]2
E NA
In a zero-order reaction for every 10° rise of temperature, the rate is doubled. If the temperature is increased from 10°C to 100°C, the rate of the reaction will become [CBSE AIPMT 2012]
A 64 timesB 128 times
C 256 times
D 512 times
E NA
For a first order reaction (A) → products the concentration of A changes from 0.1M to 0.025 M in 40minutes. The rate of reaction when the concentration of A is 0.01 M is: [AIEEE 2012]
A 1.73 × 10–5 M/minB 3.47 × 10–4 M/min
C 3.47 × 10–5 M/min
D 1.73 × 10–4 M/min
E NA
The activation energy of a reaction at a given temperature is found to be 2.303 RT J mol–1. The ratio of rate constant to the Arrhenius factor is [Karnataka CET 2011]
A 0.1B 0.01
C 0.001
D 0.02
E NA
The following data were obtained during the first order decomposition of 2A(g) → B(g) + C(s) at a constant volume and at a particular temperature. Sr. No. Time Total pressure in Pascal 1. At the end of 10 min 300 2. After completion 200 The rate constant in min–1 is [Karnataka CET 2011]
A 69.3B 0.0693
C 6.93 × 10–4
D 6.93
E NA
Consider the reaction, Cl2 (aq) + H2S (aq) → S(s) + 2H+(aq) + 2Cl–(aq) The rate equation for this reaction is, rate = k [Cl2] [H2S] Which of these mechanisms is/are consistent with this rate equation? [AIEEE 2010] (a). Cl2 + H2S → H+ + Cl– + Cl+ + HS– (slow)     Cl+ + HS– → H+ + Cl– + S (fast) (b). H2S  H+ + HS– (fast equilibrium)     Cl2 + HS– → 2Cl– + H+ + S (slow)
A (a) onlyB (b) only
C Both (a) and (b)
D Neither (a) nor (b)
E NA
The time taken for 10% completion of a first order reaction is 20 min. Then, for 19% completion, the reaction will take [WB JEE 2009]
A 40 minsB 60 mins
C 30 mins
D 50 mins
E NA
For a chemical reaction A → B, the rate of the reaction is 2 × 10–3 mol dm–3 s–1 when the initial concentration is 0.05 mol dm–3. The rate of the same reaction is 1.6 × 10–2 mol dm–3 s–1 when the initial concentration is 0.1 mol dm–3. The order of the reaction is [Karnataka CET 2009]
A 0B 3
C 1
D 2
E NA
For the decomposition of a compound AB at 600 K, the following data were obtained [Karnataka CET 2009] [AB] mol dm–3 Rate of decomposition of AB in mol dm–3 s–1 0.20 2.75 × 10–8 0.40 11.0 × 10–8 0.60 24.75 × 10–8 The order for the decomposition of AB is
A 0B 1
C 2
D 1.5
E NA
Which one of the following is a second order reaction? [Karnataka CET 2007]
A CH3COOCH3 + NaOH → CH3COONa + H2OB H2 + Cl2 Â 2HCl
C NH4NO3 → N2 + 3H2O
D H2 + Br2 → 2BHr
E NA
Consider a reaction, aG + bH → Products. When concentration of both the reactants G and H is doubled, the rate increases by eight times. However, when the concentration of G is doubled keeping the concentration of H fixed, the rate is doubled. The overall order of the reaction is: [IIT JEE 2007]
A 0B 1
C 2
D 3
E NA
If 60% of a first order reaction was completed in 60 minutes, 50% of the same reaction would be completed in approximately [CBSE PMT 2007]
A 45 minutesB 60 minutes
C 40 minutes
D 50 minutes
E NA
In a first order reaction A → B, if k is rate constant and initial concentration of the reactant A is 0.5 M, then the half-life is [CBSE PMT 2007]
AB
C
D
E NA
Which of the following statements for order of reaction is not correct? [IIT JEE 2005]
A Order can be determined experimentallyB Order of a reaction is equal to the sum of the power of concentration terms in differential rate law
C It is not affected with the stoichiometric coefficients of the reactants
D Order cannot be fractional
E NA
The rate of reaction between two reactants A and B decreases by a factor of 4 if the concentration of reactant B is doubled. The order of reaction with respect to reactant B is [CBSE AIPMT 2005]
A 2B –2
C 1
D –1
E NA
A reaction involving two different reactants can never be [AIEEE 2005]
A Unimolecular reactionB First order reaction
C Second order reaction
D Bimolecular reaction
E NA
Consider an endothermic reaction, X → Y with activation energies Eb and Ef respectively for the backward and forward reactions, respectively. In general, [AIEEE 2005]
A Eb < EfB Eb > Ef
C Eb = Ef
D there is no definite relation between Eb and Ef
E NA
t1/4 can be taken as the time taken for the concentration of a reactant to drop to 3/4 of its initial value. If rate constant for a first order reaction is k, then t1/4 can be written as [AIEEE 2005]A0.01/kB0.29/kC0.69/kD0.75/k
A 0.01/kB 0.29/k
C 0.69/k
D 0.75/k
E NA
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