State and explain kohlrausch's law of independent migration of ions.

Weak electrolytes like acetic acid have lower degree of dissociation at higher concentrations and hence for such electrolytes, the change in Λ m with dilution due to the increase in the degree of dissociation and consequently the number of ions in total volume of solution that contains 1 mole of electrolyte. In such cases, Λ m increases steeply on dilution, especially near lower concentrations. Therefore, Λ m o cannot be obtained by the extrapolation of Λ m to zero concentration. At infinite dilution, electrolyte dissociates completely but at such low concentration, the conductivity of the solution is so low, that it cannot be measured experimentally. In such cases, Λ m o for weak electrolytes can be obtained by using kohlrausch's law. Kohlrausch's law of independent migration of ions states that the limiting molar conductivity of an electrolyte can be represented as the sum of the individual contributions of the anion and the cation of the electrolyte. Thus, Λ m o = ν + λ + o + ν - λ - o Here, λ + o , λ - o are the limiting molar conductivities of the cation and anion respectively.

What are galvanic cells? Explain the working of a galvanic cell with a neat sketch taking Daniel cell as example.

Galvanic cell: A device which converts chemical energy into electrical energy by the use of spontaneous redox reactions is called Galvanic cell or voltaic cell. E.g: Daniel cell. Daniel cell: It is a special type of galvanic cell. It contains two half cells in the same vessel. The vessel is divided into two chambers. Left chambers is filled with ZnSO 4 ( aq ) solution and Zn-rod is dipped into it. Right chamber is filled with CuSO 4 ( aq ) solution and copper rod is dipped into it. Process diaphragm acts as a salt bridge. The two half cells are connected to external battery. Cell reactions: Ion Zn / ZnSO 4 half cell, oxidation reaction occurs Zn → Zn 2 + + 2 e - Ion Cu / CuSO 4 half cell, reduction reaction occurs. Cu 2 + + 2 e - → Cu The net cell reaction is Zn + Cu 2 + ⇔ Zn 2 + + Cu Cell is represented as Zn / Zn 2 + ∥ Cu 2 + / Cu

Write the Arrhenius equation for the rate constant (k) of a reaction.

The temperature dependence of the rate of a chemical reaction can be accurately explained by Arrhenius equation. k = A e - Ea RT where A is the Arrhenius factor or the frequency factor. It is also called pre-exponential factor. It is a constant specific to a particular reaction. R is gas constant and E a is activation energy measured in joules/mole ( J mol - 1 ) .

What are pseudo first order reactions? Give one example.

The reactions which are not truly of first order but become reactions of first order under certain conditions are called pseudo first order reactions. For example, hydrolysis of ester. Rate = k ' [ CH 3 COOC 2 H 5 ] [ H 2 O ] Since water is in excess and [ H 2 O ] is constant . So , Rate = k [ CH 3 COOC 2 H 5 ] , where k = k ' [ H 2 O ]

The rate constant for a first order reaction is 60 s - 1 . How much time will it take to reduce the initial concentration of the reactant to its 1 / 16 th value?

Given, rate constant k for a first order reaction = 60 s - 1 Let us assume: Initial concentration R 0 = x Final concentration R = x 16 Formula for first order reaction, t = 2.303 k l o g R 0 R = 2.303 k l o g x x 16 = 2.303 k l o g 1 1 16 = 2.303 60 l o g 16 = 4.6 × 10 - 2 s Hence, the required time is 4.6 × 10 - 2 s .

A first order reaction takes 40 minutes for 30 % decomposition. Calculate t 1 / 2 ?

Given data: Order of reaction = 1 R 0 = 100 ; R = 100 - 30 = 70 First order rate equation is: k = 2 .303 t log R 0 R k = 2.303 40 l o g 100 70 = 2.303 40 l o g 10 7 = 8.91 × 10 - 3 m i n - 1 Therefore, t 1 / 2 of the decomposition reaction can be determined as follows: t 1 / 2 = 0 .693 k = 0.693 8.91 × 10 - 3 = 77.71 m i n .

Derive an integrated rate equation for a first order reaction.

Let us, consider a unimolecular first order reaction represented by the general equation, A → Product At t = 0 a 0 At t = t a - x x The initial concentration of A is a mole L - 1 and its concentration after time t is ( a – x ) mole L - 1 . This means during the time interval t , x mole L – 1 of A has reacted. The rate of reaction at any time t is given by the following first order kinetics. dx dt = k a - x where k is the rate constant of the reaction. dx a - x = kdt This is differential rate equation and can be solved by integration. ∫ dx a - x = k ∫ dt - ln a - x = k . t + C . . . . . ( 1 ) where C is integration constant. The constant C can be evaluated by applying the initial condition of the reaction i.e. when t = 0 , x = 0 . Putting these in equation (1), we get C = – ln a Putting the value of C in equation (1), we get – ln ( a – x ) = k . t – lna k = 1 t ln a a - x = 2 . 303 t log a a - x . . . . . ( 2 ) Equation (2) integrated rate equation for a first order reaction.

E M B I B E

Intermediate Second Year Chemistry>Chapter 3 - Electrochemistry and Chemical Kinetics>Questions>Q 3

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12th Andhra Pradesh Board

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What are the units of rate of reaction?

Important Questions on Electrochemistry and Chemical Kinetics

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12th Andhra Pradesh Board

IMPORTANT

Intermediate Second Year Chemistry>Chapter 3 - Electrochemistry and Chemical Kinetics>Questions>Q 4

Draw the graphs that relate the concentrations (C) of the reactants and the reaction times(t) and the concentrations of the products (C) and the reaction times(t) in chemical reactions.