Q1. For the reaction, 2N_2 O_5 (g)→4NO_2 (g)+O_2 (g) If the concentration of NO_2 increase by 5.2×〖10〗^(-3) M in 100 s then the rate of the reactions
  •  2×〖10〗^(-3) Ms^(-1)
  •  7.6×〖10〗^(-4) Ms^(-1)
  •  0.5×〖10〗^(-4) Ms^(-1)
  •  1.3×〖10〗^(-5) Ms^(-1)
Rate of reaction =1/4 d(NO_2 )/dt=(5.2×〖10〗^(-3))/(4×100) =1.3×〖10〗^(-5 ) Ms^(-1)

Q2.For a fist order reaction, the concentration changes from 0.8 to 0.4 in 15 min. The time taken for the concentration to change from 0.1 M to 0.025 M is
  •  60 min
  •  30 Min
  •  15 Min
  •  7.5 min
T_50=15 min k=2.303log2/T_50 =2.303log2/15 a=0.1M (a-x)=0.025 M For first order reaction, k=2.303log2/T_50 log⁡(a/(a-x)) 2.303log2/15=(2×2.303log2)/t log 0.1/0.025 =2.303/t log4 ∴2.303log2/15=(2×2.303log2)/t ∴ t=30 min

Q3.  If the concentration units are reduced by n times, then the value of rate constant of first order will:
  •   Increase by n times
  •  Decrease by factor of n
  •  None of these
  •  Not change
Rate constant is characteristic constant of a reaction and depends only on temperature and catalyst.

Q4. Inversion of cane-sugar in dilute acid is a
  •  Bimolecular reaction
  •  Trimolecular reaction
  •  Unimolecular reaction
  •  Pseudo-unimolecular reaction
c_12 H_22 O_11+H_2 O□(→┴(Dil.acid) ) C_6 H_12 O_6+C_6+H_12 O_6 Excess glucose fructose when one of the reactant is present in large excess, the second order reaction confirms to the first order and is knows as Pseudo-unimolecular reaction

Q5.The unit of rate constant for a zero order reaction
  •  mol L^(-1) s^(-1)
  •  mol s^(-1)
  •  L s^(-1)
  •  L mol^(-1) s^(-1)

Q6. For the reaction; 2N_2 O_5⟶4NO_2+O_2, rate and rate constant are 1.02×〖10〗^(-4) M sec^(-1)⁡and 3.4×〖10〗^(-5) sec^(-1)⁡M respectively, then concentration of N_2 O_5, at that time will be:
  •  1.732 M
  •  3 M
  • 1.02×〖10〗^(-4) M
  •  3.5×〖10〗^5 M
r=K[N_2 O_5] ∴[N_2 O_5 ]=r/K=(1.02×〖10〗^(-4))/(3.4×〖10〗^(-5) )=3M .

Q7.If “a” and “t_(1/2)” are initial concentration of reactant and half-life of a zero order reaction respectively, which of the following is correct ?
  •  t_(1/2)∝a^2
  •  t_(1/2)∝1/a^2
  •  t_(1/2)∝a
  •  t_(1/2)∝1/a
For zero order reaction integrated rate equation is kt=[A]_0-[A] If 〖[A]〗_0=a,[A]=a/2,t=t_(1/2) kt_(1/2)=a-a/2 kt_(1/2)=a/2 t_(1/2)=a/2k ∴ t_(1/2)∝a

Q8.In the reaction 2A+B→A_2 B, if the concentration of A is doubled and of B is halved, then the rate of the reaction will
  •  Decrease by two times
  •  Increase by two times
  •  Increase by four times
  •  Remain the same
2A+B→A_2 B r_1=k[A]^2 [B] r_2=k[2A]^2 [B/2] Or r_2=2k[A]^2 [B] ∴r_2=2r_1

Q9.The Arrhenius equation expressing the effect of temperature on the rate constant of reaction is:
  •  K=E_a/RT
  •  K=e^(-Ea/RT)
  •  K=log_e⁡〖E_a/RT〗
  •  K=Ae^(-E_a/RT)
This is Arrhenius equation.

Q10. The rate constant is given by the equation K=Ae^(-E_a/RT) which factor should register a decrease for the reaction to proceed more rapidly?
  •  A
  •  E_a
  •  Z
  • T
A decrease in E_a will increase rate constant K and thus rate of reaction increases.

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