Molar Conductivity and Cell Constant Quiz

Electrochemical cell converts chemical energy into electrical energy based on spontaneous redox reactions, while an electrolytic cell converts electrical energy into chemical energy for non-spontaneous reactions.

Electrochemical cells operate based on spontaneous redox reactions, where the Gibbs free energy change (ΔG) is negative.

In an electrochemical cell, two electrodes are usually placed in separate beakers, while in an electrolytic cell, both electrodes are suspended in the same electrolyte solution or melt.

<p>The main purpose of a fuel cell is to convert chemical energy directly into electrical energy through redox reactions.</p> Signup and view all the answers

<p>The Nernst Equation is crucial for determining the cell potential under non-standard conditions, providing insights into reaction spontaneity.</p> Signup and view all the answers

<p>Batteries store and release electrical energy through chemical reactions, while fuel cells directly convert chemical energy into electrical energy.</p> Signup and view all the answers

<p>The number of ions per unit volume increases on dilution, leading to a decrease in conductivity.</p> Signup and view all the answers

<p>Limiting molar conductivity is the molar conductivity of an electrolyte solution at infinite dilution.</p> Signup and view all the answers

<p>Kohlrausch’s law states that each ion in an electrolyte solution migrates independently. One application is in determining the molar conductivity of strong electrolytes.</p> Signup and view all the answers

<p>Molar conductivity (Lm) is the conductivity of a solution containing 1 mole of electrolyte.</p> Signup and view all the answers

<p>Kohlrausch’s law states that each ion in an electrolyte solution moves independently and contributes to the overall conductivity.</p> Signup and view all the answers

<p>Limiting molar conductivity is the molar conductivity of an electrolyte solution at infinite dilution.</p> Signup and view all the answers

<p>Ecell = E°cell − 0.0591 [Cr3+ ]^2 log n [Cr2O7^2- ][H+ ]^14</p> Signup and view all the answers

<p>1.33 V</p> Signup and view all the answers

<p>0.782 V</p> Signup and view all the answers

<p>The number of ions per unit volume that carry the current in a solution decreases on dilution.</p> Signup and view all the answers

<p>-517.24 kJ mol–1</p> Signup and view all the answers

<p>From Cu to Mg</p> Signup and view all the answers

<p>Pb(s) + PbO2(s) + 2H2SO4(aq) → 2PbSO4(s) + 2H2O(l)</p> Signup and view all the answers

<p>It can only be used once and cannot be recharged.</p> Signup and view all the answers

<p>The cell potential remains constant during its lifetime.</p> Signup and view all the answers

<p>It is a secondary cell.</p> Signup and view all the answers

<p>2PbSO4(s) + 2H2O(l) → Pb(s) + PbO2(s) + 2H2SO4(aq)</p> Signup and view all the answers

<p>Hydrogen oxygen fuel cell</p> Signup and view all the answers

<p>Molar conductivity increases with dilution for a weak electrolyte due to increased dissociation of ions.</p> Signup and view all the answers

<p>Molar conductivity decreases with dilution for a strong electrolyte due to fewer ions being present in solution.</p> Signup and view all the answers

<p>The cell constant is 0.097 cm^–1.</p> Signup and view all the answers

<p>4 Faradays.</p> Signup and view all the answers

<p>Chlorine gas is liberated at the anode due to kinetic factors, even though O2 has a higher standard reduction potential.</p> Signup and view all the answers

<p>2 Faradays.</p> Signup and view all the answers