JEE Exam > JEE Notes > Chapter-wise Tests for JEE Main & Advanced > JEE Advanced (Fill in the Blanks): Electrochemistry
JEE Advanced (Fill in the Blanks): Electrochemistry | Chapter-wise Tests for JEE Main & Advanced PDF Download
Fill in the Blanks
1. Of the halide ions, _____ is the most powerful reducing agent. (1978)
Ans: I–
Solution: ( ∵ I2 is weakest oxidising agent)
2. The more ............... the standard reduction potential, the ............... is its ability to displace hydrogen from acids. (1986 - 1 Mark)
Ans: negative, greater
Solution: negative, greater; Among the various metals, since sodium has the minimum reduction potential, it must be strongest reducing agent. In general, more the reduction potential
lesser is its reducing action.
3. The electrical conductivity of a solution of acetic acid will be .............. if a solution of sodium hydroxide is added. (1987 - 1 Mark)
Ans: increased
True/False
The dependence of electrode potential for the electrode Mn+ /M with concentration under STP conditions is given by the expression :
(1993 - 1 Mark)
Ans: False
Solution : False : When the temperature is 273, the value of the factor will come out as 0.0541 instead of 0.0591. The value 0.0591 comes out at 298 K and not at 273 K.
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FAQs on JEE Advanced (Fill in the Blanks): Electrochemistry - Chapter-wise Tests for JEE Main & Advanced
| 1. What is electrochemistry? |  |
Ans. Electrochemistry is the branch of chemistry that deals with the study of chemical reactions that involve the transfer of electrons between species. It involves the study of redox reactions, where one species loses electrons (oxidation) and another species gains electrons (reduction).
| 2. What is the importance of electrochemistry? | |
Ans. Electrochemistry is of great importance in various fields. It is crucial in understanding and optimizing electrochemical processes such as battery operation, corrosion, and electroplating. It also plays a significant role in the field of energy storage and conversion, as in fuel cells and electrolysis. Moreover, electrochemical techniques are widely used in analytical chemistry for determining the concentration of certain substances.
| 3. What is the Nernst equation? | |
Ans. The Nernst equation is an equation that relates the electrode potential of an electrochemical cell to the concentration of reactants and products involved in the cell reaction. It is given by E = E° - (0.0592/n)log(Q), where E is the electrode potential, E° is the standard electrode potential, n is the number of electrons transferred in the cell reaction, and Q is the reaction quotient.
| 4. How does a galvanic cell work? | |
Ans. A galvanic cell, also known as a voltaic cell, is an electrochemical cell that converts chemical energy into electrical energy. It consists of two half-cells, each containing an electrode immersed in an electrolyte solution. The two half-cells are connected by a salt bridge or a porous barrier. In one half-cell, oxidation occurs, leading to the release of electrons. These electrons flow through an external circuit to the other half-cell, where reduction occurs. The flow of electrons generates an electric current.
| 5. What is Faraday's law of electrolysis? | |
Ans. Faraday's law of electrolysis states that the amount of a substance produced or consumed during an electrolysis reaction is directly proportional to the quantity of electrical charge passed through the electrolyte. It can be expressed as m = (Q × M) / (n × F), where m is the mass of the substance, Q is the electrical charge passed, M is the molar mass of the substance, n is the number of electrons transferred, and F is the Faraday constant.
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