NEET AIPMT Chemistry Chapter Wise Solutions – Chemical Kinetics
Contents
NEET AIPMT Chemistry Chapter Wise SolutionsPhysicsBiology
1. Mechanism of a hypothetical reaction
The overall order of the reaction will be (NEET 2017)
(a) 2
(b) 0
(c) 1.5
(d) 1
2. A first order reaction has a specific reaction rate of 10-2 sec-1 . How much time will it take for 20 g of the reactant to reduce to 5 g? (NEET 2017)
(a) 138.6 sec
(b) 346.5 sec
(c) 693.0 sec
(d) 238.6 sec
3. The decomposition of phosphine (PH3) on tungsten at Tow pressure is a first-order reaction. It is because the (NEET-II 2016)
(a) rate is proportional to the surface coverage
(b) rate is inversely proportional to the surface coverage
(c) rate is independent of the surface coverage
(d) rate of decomposition is very slow.
4. The rate of first-order reaction is 0.04 mol L-1s-1 at 10 seconds and 0.03 mol L-1 s-1 at 20 seconds after initiation of the reaction. The half-life period of the reaction is (NEET-I 2016)
(a) 44.1 s
(b) 54.1 s
(c) 24.1s
(d) 34.1s
5. The addition of a catalyst during a chemical reaction alters which of the following quantities? (NEET-I 2016)
(a) Enthalpy
(b) Activation energy
(c) Entropy
(d) Internal energy
6. The rate constant of the reaction A —> B is 0.6 x 10-3 mol L-1 s -1. If the concentration of A is 5 M, then concentration of B after 20 minutes is (2015)
(a) 3.60 M
(b) 0.36 M
(c) 0.72 M
(d) 1.08 M
7. The activation energy of a reaction can be determined from the slope of which of the following graphs? (2015, Cancelled)
8. When initial concentration of a reactant is doubled in a reaction, its half-life period is not affected. The order of the reaction is (2015, Cancelled)
(a) second
(b) more than zero but less than first
(c) zero
(d) first.
9. What is the activation energy for a reaction if its rate doubles when the temperature is raised from 20°C to 35°C? (NEET 2013) (R = 8.314 J mol-1 K-1)
(a) 34.7 kJ mol-1
(b) 15.1 kJ mol-1
(c) 342 kJ mol-1
(d) 269 kJ mol-1
10. For a reaction between A and B the order with respect to A is 2 and the other with respect to B is 3. The concentrations of both A and B are doubled, the rate will increase by a factor of (Karnataka NEET 2013)
(a) 12
(b) 16
(c) 32
(d) 10
11. A reaction is 50% complete in 2 hours and 75% complete in 4 hours. The order of reaction is (Karnataka NEET 2013)
(a) 1
(b) 2
(c) 3
(d) 0
12. 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 concentration of both the reactants (A and B) are doubled, rate law for the reaction can be written as (2012)
(a) rate = k[A][B]²
(b) rate = k[A]²[B]²
(c) rate = k[A][B]
(d) rate = k[A]²[B]
13. In a zero-order reaction, for every 10°C 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 (2012)
(a) 256 times
(b) 512 times
(c) 64 times
(d) 128 times
14. Activation energy (Ea) and rate constants (k1, and k2) of a chemical reaction at two different temperatures (T1 and T2) are related by (2012)
15. Which one of the following statements for the order of a reaction is incorrect? (2011)
(a) Order can be determined only experimentally.
(b) Order is not influenced by stoichiometric coefficient of the reactants.
(c) Order of a reaction is sum of power to the concentration terms of reactants to express the rate of reaction.
(d) Order of reaction is always whole number.
16. The rate of the reaction : 2N205 —» 4N02 + 02 can be written in three ways.
The relationship between k and k’ and between k and k” are (Mains 2011)
(a) k’ = 2k ; k” = k
(b) k’ = 2k ; k” = k/2
(c) k’ = 2k ; k” = 2k
(d) k’ = k ; k” = k
17. The unit of rate constant for a zero order reaction is
(a) mol L-1 s-1
(b) L mol-1 s-1
(c)L² mol-1 s-1
(d)s-1
18. The half-life of a substance in a certain enzyme- catalysed reaction is 138 s. The time required for the concentration of the substance to fall from 1.28 mg L-1 to 0.04 mg L-1 is (Mains 2011)
(a) 414 s
(b) 552 s
(c) 690 s
(d) 276 s
19. For the reaction N205(g)—>2NO2(g) + 1/2O2(g) value of rate of disappearance of N205 is given as 6.25 x 10-3mol L-1s-1. The rate of formation of N02 and 02 is given respectively as (2010)
20. During the kinetic study of the reaction, 2A + B —» C + D, following results were obtained (2010)
(a) Rate = k[A]²[B]
(b) Rate = k[A][B]
(c) Rate = k[A]²[B]²
(d) Rate = k[A][B]²
21. The rate of the reaction, 2NO + Cl2 —> 2NOCl is given by the rate equation rate = k[NO]²[Cl2]. The value of the rate constant can be increased by (Mains 2010)
(a) increasing the temperature
(b) increasing the concentration of NO
(c) increasing the concentration of the Cl2
(d) doing all of these.
22. For the reaction, N2 + 3H2 —» 2NH3, if d[NH3] /dt= 2 x 10-4 mol L-1 s-1 the value of -d[H2]/dt would be
(a) 4 x 10-4 mol L-1 s-1
(b) 6 x 10-4 mol L-1 s-1
(c) 1 x 10-4 mol L-1 s-1
(d) 3 x 10-4 mol L-1 s-1
23.In the reaction, (2009)
24. Half-life period of a first order reaction is 1386 seconds. The specific rate constant of the reaction is (2009)
(a) 0.5 x 10-2 s-1
(b) 0.5 x 10-3 s-1
(c) 5.0 x 10-2 s-1
(d) 5.0 x 10-3 s-1
25.For the reaction A + B —>products, it is observed that (2009)
(i) on doubling the initial concentration of A only, the rate of reaction is also doubled and
(ii) on doubling the initial concentration of both A and B, there is a change by a factor of 8 in the rate of the reaction.
The rate of this reaction is given by
(a) rate = k[A] [B]²
(b) rate = k[A]² [B]²
(c) rate = k[A] [B]
(d) rate = k[A]² [B]
26. The bromination of acetone that occurs in acid solution is represented by this equation. (2008)
27.The rate constants K1, and K2, for two different reactions are 1016 . e-2000/T and 1015 . e-1000/T, respectively. The temperature at which K1 = K2 is (2008)
(a)2000 k
(b)1000/2.303 k
(c)1000 k
(d)2000/2.303 k
28. If 60% of a first order reaction was completed in 60 minutes, 50% of the same reaction would be completed in approximately (2007)
(log 4 = 0.60, log 5 = 0.69)
(a) 45 minutes
(b) 60 minutes
(c) 40 minutes
(d) 50 minutes.
29. 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 (2007)
(a)log2/k
(b)log2/k√0.5
(c)In 2/k
(d)0.693/0.5k
30. The reaction of hydrogen and iodine monochloride is given as: (2007)
(a) A and B both
(b) Neither A nor B
(c) A only
(d) B only.
31. Consider the reaction: N2(g) + 3H2(g) —> 2NH3(g) The equality relationship between (2006)
32. For the reaction, 2A + B —» 3C + D, which of the following does not express the reaction rate (2006)
(a)-d[A]/2dt
(b)-d[C]/3dt
(c)-d[B]/dt
(d)d[D]/dt
33. 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 this reaction with respect to reactant B is (2005)
(a) 2
(b) -2
(c) 1
(d) -1
34. For a first order reaction A —> B the reaction rate at reactant concentration of 0.01 M is found to be 2.0 x 10-5 mol L-1 s-1. The half¬life period of the reaction is (2005)
(a) 30 s
(b) 220 s
(c) 300 s
(d) 347 s
35. The rate of a first order reaction is 1.5 x 10-2 mol L-1 min-1 at 0.5 M concentration of the reactant. The half-life of the reaction is (2004)
(a) 0.383 min
(b) 23.1 min
(c) 8.73 min
(d) 7.53 min
36. The temperature dependence of rate constant (k) of a chemical reaction is written in terms of Arrhenius equation, k = A.e-E*/RT. Activation energy (E* ) of the reaction can be calculated by plotting (2003)
(a) k vs T
(b) k vs 1/logT
(c) log k vs 1/T
(d) logk vs 1/logT
37. If the rate of the reaction is equal to the rate constant, the order of the reaction is (2003)
(a) 0
(b) 1
(c) 2
(d) 3
38. 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 ? (2003)
(a) 1 hour
(b) 0.5 hour
(c) 0.25 hour
(d) 2 hours
39. The activation energy for a simple chemical reaction A <—-> B is Ea in forward direction. The activation energy for reverse reaction (2003)
(a) is negative of Ea
(b) is always less than Ea
(c) can be less than or more than Ea
(d) is always double of Ea
40. 2A —> B + C It would be a zero order reaction when (2002)
(a) the rate of reaction is proportional to square of concentration of A
(b) the rate of reaction remains same at any concentration of A
(c) the rate remains unchanged at any concentration of B and C
(d) the rate of reaction doubles if concentration of B is increased to double.
41. 3A —> 2B, rate of reaction +d[B]/dt (2002)
42. When a bio-chemical reaction is carried out in laboratory, outside the human body in absence of enzyme, then rate of reaction obtained is 10-6 times, the activation energy of reaction in the presence of enzyme is (2001)
(a) 6/RT
(b) P is required
(c) different from Ea obtained in laboratory
(d) can’t say anything.
43. For the reaction; 2N2O5 —> 4N02 + 02 rate and rate constant are 1.02 x 10-4 and 3.4 x 10-5 sec-1 respectively, then concentration of N205 at that time will be (2001)
(a) 1.732
(b) 3
(c) 1.02 x 10-4
(d) 3.4 x 105
44. How enzymes increases the rate of reactions (2000)
(a) by lowering activation energy
(b) by increasing activation energy
(c) by changing equilibrium constant
(d) by forming enzyme substrate complex.
45. For the reaction H– + BiO3– + 3Br– —» 5Br2 + H20 which of the following relation correctly represents the consumption and formation of products.
46. For a first-order reaction, the half-life period is independent of (1999)
(a) first power of final concentration
(b) cube root of initial concentration
(c) initial concentration
(d) square root of final concentration
47. Activation energy of a chemical reaction can be determined by (1998)
(a) evaluating rate constants at two different temperatures
(b) evaluating velocities of reaction at two different temperatures
(c) evaluating rate constant at standard temperature
(d) changing concentration of reactants.
48. The experimental data for the reaction, (1997)
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The rate equation for the above data is
(a) Rate = k [A]²[B]²
(b) Rate = k [A]²[B]
(c) Rate = k [B2]
(d) Rate = k [B2]²
49.(1997)
50. The given reaction 2 FeCl3 + SnCl2 —>2 FeCl2 + SnCl4 is an example of (1996)
(a) third order reaction
(b) first order reaction
(c) second order reaction
(d) none of these.
51.The data for the reaction A + B—> C, is
The rate law corresponds to the above data is (1994)
(a) Rate = k[A][B]3
(b) Rate = k[A]2[B]2
(c) Rate = k[B]3
(d) Rate = k[B]4
52. By the action of enzymes, the rate of biochemical reaction (1994)
(a) does not change
(b) increases
(c) decreases
(d) either (a) or (c).
Answer Key
Explanations
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