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Q1. In a 1st order reaction, reactant concentration C varies with time t as
•  1/C increases linearly with t
•  C decreases with 1/t
•  Log C decreases with 1/t
•  Log C decreases linearly with t
Solution
B

Q2.Rate equation for a second order reaction is:
•  K=1/t^2 ∙a/((a-x))
•  K=1/t∙x/(a(a-x))
•  K=1/t log⁡〖a/(a(a-x))〗
•  K=2.303/t log⁡〖a/((a-x))〗
Solution
dx/dt=K(a-x)^2 is differential form of II order. Integrate it to get (c).

Q3.  The rate constant (k^' ) of one of the reaction is found to be double that of the rate constant (k^'') of another reaction. Then the relationship between the corresponding activation energies of the two reaction (E_a^' and E_a^'' ) can be represented as
•   E_a^'>E_a^''
•  E_a^'=4E^''
•  E_1^'=E_a^''
•  E_a^'
Solution
∵ Rate constant (k^' )> rate constant (k^(' ')) Greater the rate constant lesser will be the activation energy ∴E_a^'

Q4. Which increases on increase of temperature?
•  Energy of activation (E_a)
•  Collision frequency (Z)
•  Rate constant (k)
•  Both (a) and (c)
Solution
The collision frequency (Z)and rate contant(k) increase on increase of temperature. With the increase in temperature, the average kinetic energy of the molecules increases and this leads to an increase in number of collisions per unit time (Z). The rate constant (k) of a reaction is also increases with increase of temperature.

Q5.Find the two third life (t_(1/2))of a first order reaction in which k=5.48×〖10〗^(-14)per second
•  2.01×〖10〗^13 s
•  201×〖10〗^20 s
•  0.201×〖10〗^10 s
•  201×〖10〗^13 s
Solution
Let ,initial concentration=a Final concentration=a- 2/3 a= a/3 t_(2/3)=2.303/k log a/(a/3) =2.303/(5.48×〖10〗^(-14) ) log⁡3 =2.01×〖10〗^13 s

Q6. Which one is not correct?
•  Rate of zero order reaction does not depend upon initial concentration of reactant
•  Rate of zero order reaction depends upon initial concentration of reactant
• t_(1/2) of first order reaction is independent of initial concentration of reaction
•  t_(1/2) of zero order reaction is dependent of initial concentration of reaction
Solution
The rate of zero order reaction is independent of the concentration of the reactants or the concentration of the reactant do not change with time. Thus, the rate of reaction remains constant. dx/dt=k(a-x)^0⇒dx/dt=k Or Rate=k

•  0.693/k
•  k/2.303
•  -k/2.303
•  log⁡[A]_0
Solution
Q8.2N_2 O_5 (g)→4NO_2 (g)+O_2 (g) What is the ratio of the rate of decomposition of N_2 O_5 to rate of formation of O_2 ?
•  1:2
•  2:1
•  1:4
•  4:1
Solution
Q9.Unit of frequency factor (A) is
•  mol/L
•  mol/L×s
•  It does not have any unit
•  Depends upon order of reaction
Solution
Unit of A depends on unit of k.

Q10. If the volume of the vessel in which the reaction 2NO+O_2→2NO_2 is occurring is diminished to 1/3rd of its initial volume. The rate of the reaction will be increased by
•  9 times
•  27 times
•  36 times
• 3 times
Solution
As we know that, rate of reaction is directly proportional to concentration of reactant and inversely proportional to the volume of vessel. i.e.,concentrationα∝n/v For a given reaction, 2NO(g)+O_2 (g)⇌2NO_2 (g) Rate of reaction=k[NO]^2 [O_2] If volume of vessel is reduced by 1/3 rd of its initial value, then concentration of compound is increase by 3 times. Hence, the rate of reaction will be increased by 27 times. #### Written by: AUTHORNAME

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