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 ]

What are elementary reactions?

Elementary reactions: A balanced chemical equation never gives us a true picture of how a reaction takes place since rarely a reaction gets completed in one step. The reactions taking place in one step are called elementary reactions or an elementary reaction is a chemical reaction in which one or more chemical species react directly to form products in a single reaction step and with a single transition state.

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 34

HARD

12th Andhra Pradesh Board

IMPORTANT

Earn 100

Give the construction and working of a standard hydrogen electrode with a neat diagram.

Important Questions on Electrochemistry and Chemical Kinetics

HARD

12th Andhra Pradesh Board

IMPORTANT

Intermediate Second Year Chemistry>Chapter 3 - Electrochemistry and Chemical Kinetics>Questions>Q 35

State and explain the Nernst equation with the help of a metallic electrode and anon-metallic electrode.

HARD

12th Andhra Pradesh Board

IMPORTANT

Intermediate Second Year Chemistry>Chapter 3 - Electrochemistry and Chemical Kinetics>Questions>Q 36

Explain with a suitable example the relation between the Gibbs energy of chemical reaction (G) and the functioning of the electrochemical cell.

EASY

12th Andhra Pradesh Board

IMPORTANT

Intermediate Second Year Chemistry>Chapter 3 - Electrochemistry and Chemical Kinetics>Questions>Q 37

On what factors the electrical conductance of an aqueous electrolyte solution depends?

HARD

12th Andhra Pradesh Board

IMPORTANT

Intermediate Second Year Chemistry>Chapter 3 - Electrochemistry and Chemical Kinetics>Questions>Q 38

How is molar conductivity of an aqueous solution of an electrolyte measured experimentally?

MEDIUM

12th Andhra Pradesh Board

IMPORTANT

Intermediate Second Year Chemistry>Chapter 3 - Electrochemistry and Chemical Kinetics>Questions>Q 39

Explain the variation of molar conductivity with the change in concentration of the electrolyte. Give reasons.

HARD

12th Andhra Pradesh Board

IMPORTANT

Intermediate Second Year Chemistry>Chapter 3 - Electrochemistry and Chemical Kinetics>Questions>Q 40

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

MEDIUM

12th Andhra Pradesh Board

IMPORTANT

Intermediate Second Year Chemistry>Chapter 3 - Electrochemistry and Chemical Kinetics>Questions>Q 41

What is electrolysis? Give Faraday's first law of electrolysis?

EASY

12th Andhra Pradesh Board

IMPORTANT

Intermediate Second Year Chemistry>Chapter 3 - Electrochemistry and Chemical Kinetics>Questions>Q 42

What are the products obtained at cathode and the anode during the electrolysis of the following when platinum electrodes are used in the electrolysis.

Molten $KCl$

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