List of top Chemistry Questions on Electrochemistry asked in CUET (UG)

In an electrochemical cell, the standard electrode potential of Zn\(^{2+}\)/Zn is \(-0.76\, \text{V}\) and that of Cu\(^{2+}\)/Cu is \(+0.34\, \text{V}\). What is the standard EMF of the cell?
What is the numerical value of one Faraday in Coulombs?
Read the following passage and answer the next five questions based on it.

Battery or cell converts chemical energy of the redox reaction to electrical energy. In fuel cells (a galvanic cell), the chemical energy of combustion of fuels like H2, ethanol, etc., is directly converted to electrical energy. In a fuel cell, H2 and O2 react to produce electricity, where H2 gas is oxidized at the anode and oxygen is reduced at the cathode, and the reactions involved are:

Anode reaction: H2 + 2OH- → 2H2O + 2e-

Cathode reaction: O2 + 2H2O + 4e- → 4OH-

67.2 L of H2 at STP reacts in 15 minutes.

During electrolysis of acidified water. 2.8 Litre of oxygen gas is released (at STP). The charge passed through the anode is -
The cell reaction occurring at anode in the electrolysis of aqueous NaCl solution is:
The standard reduction potential for Sn$^{4+}$/Sn$^{2+}$ is +0.15 V and for Cr$^{3+}$/Cr is -0.74 V. These two half-cells, coupled in their standard states, are connected to make a cell. The galvanic cell can be correctly represented by:
The quantity of charge required to obtain 2 mol of Mn$^{2+}$ from MnO$_4^{-}$ is:
Find the value of \(E^\circ\) in the missing link in following diagram
Find the value of E in the missing link in following diagram

Match List - I with List - II

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