Which of the following expressions correctly represents the equivalent conductance at infinite dilution of ${Al2(SO4)3}$ ? Given that ${\wedge^{\circ}_{Al^{3+}}}$ and ${- \wedge^{\circ}_{SO^{2-}_4}}$ are the equivalent conductances at infinite dilution of the respective ions
- ${ \wedge^{\circ}_{Al^{3+}} + \wedge^{\circ}_{SO_4^{2-}}}$
- $ \left({\wedge^{\circ}_{Al^{3+}} + \wedge^{\circ}_{SO_4^{2-}}} \right) \times 6$
- $ \frac{1}{3}{\wedge^{\circ}_{Al^{3+}} + \frac{1}{2} \wedge^{\circ}_{SO_4^{2-}}} $
- ${2 \wedge^{\circ}_{Al^{3+}} + 3 \wedge^{\circ}_{SO_4^{2-}}}$
The Correct Option is A
Approach Solution - 1
Since equivalent conductance's are given only for ions, the equivalent conductance at infinite dilution,
$\Lambda _{eq}^{\infty }=\Lambda _{Al\,3+}^{o}+\Lambda _{so_{4}^{2-}}^{o}$
Approach Solution -2
Ans: The equivalent conduction at the infinite dilution (Λ°), for an electrolyte is calculated by the use of Kohlrausch’s law. It states that,
At infinite dilution, each of the ion makes a constant contribution towards the equivalent conductivity of an electrolyte, this is irrespective of the nature of the other ion that is present in the solution.
the expression for the equivalent conductance at infinite dilution of Al2(SO4)3 is:
Λ°(Al2(SO4)3) = 2Λ°(Al^3+) + 3Λ°(SO4^2-)
Since equivalent conductance's are given only for ions, the equivalent conductance at infinite dilution,
Λ°(Al^3+) + Λ°(SO4^2-)
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Concepts Used:
Electrochemical Cells
An electrochemical cell is a device that is used to create electrical energy through the chemical reactions which are involved in it. The electrical energy supplied to electrochemical cells is used to smooth the chemical reactions. In the electrochemical cell, the involved devices have the ability to convert the chemical energy to electrical energy or vice-versa.
Classification of Electrochemical Cell:
Cathode
- Denoted by a positive sign since electrons are consumed here
- A reduction reaction occurs in the cathode of an electrochemical cell
- Electrons move into the cathode
Anode
- Denoted by a negative sign since electrons are liberated here
- An oxidation reaction occurs here
- Electrons move out of the anode
Types of Electrochemical Cells:
Galvanic cells (also known as Voltaic cells)
- Chemical energy is transformed into electrical energy.
- The redox reactions are spontaneous in nature.
- The anode is negatively charged and the cathode is positively charged.
- The electrons originate from the species that undergo oxidation.
Electrolytic cells
- Electrical energy is transformed into chemical energy.
- The redox reactions are non-spontaneous.
- These cells are positively charged anode and negatively charged cathode.
- Electrons originate from an external source.