Question:
When the same quantity of current is passed through $ {CuSO_4}$ and $ {AgNO_3}$ solution 2.7 g of silver is deposited. The amount of copper deposited is
When the same quantity of current is passed through $ {CuSO_4}$ and $ {AgNO_3}$ solution 2.7 g of silver is deposited. The amount of copper deposited is
Updated On: Jun 21, 2022
- 0.4 g
- 3.2 g
- 1.6 g
- 0.8 g
Hide Solution
Verified By Collegedunia
The Correct Option is D
Solution and Explanation
According to Faraday's second law :
$ { \frac{ Wt. of \,Cu \, deposited}{ Wt. of\, Ag \,deposited} = \frac{E wt.of \,Cu}{E wt. \,of\, Ag} }$
Wt. of Cu deposited
$ = { \frac{E wt. of\, Cu \times Wt. of \,Ag \, deposited}{ E wt. of\, Ag} }$
$ = \frac{63.5 / 2 \times 2.7}{108} = 0.793 = 0.80 \, g$
$ { \frac{ Wt. of \,Cu \, deposited}{ Wt. of\, Ag \,deposited} = \frac{E wt.of \,Cu}{E wt. \,of\, Ag} }$
Wt. of Cu deposited
$ = { \frac{E wt. of\, Cu \times Wt. of \,Ag \, deposited}{ E wt. of\, Ag} }$
$ = \frac{63.5 / 2 \times 2.7}{108} = 0.793 = 0.80 \, g$
Was this answer helpful?
0
0
Top Questions on Electrochemistry
- Name and define the cell which was used for providing electric power in the Apollo space programme. Also write its one advantage.
- CBSE CLASS XII - 2025
- Chemistry
- Electrochemistry
- Calculate the molar conductance $\Lambda_m^\circ$ for CaCl$_2$, given that $\lambda^\circ(Ca^{+2}) = 119.5$ S cm$^2$ mol$^{-1}$ and $\lambda^\circ(Cl^-) = 76.3$ S cm$^2$ mol$^{-1}$.
- PSEB XII - 2025
- Chemistry
- Electrochemistry
- Write the Nearest equation and calculate the e.m.f of the following cell at 298K.
Fe(s) | Fe$^{2+$(0.001M) || H$^+$(1M) H$_2$(1atm) | Pt.
Given E$^\circ_{Fe^{+2}/Fe} = -0.44$ V.}
- PSEB XII - 2025
- Chemistry
- Electrochemistry
- How many Coulombs of electricity are required for complete oxidation of 90 gm of H$_2$O ?
- PSEB XII - 2025
- Chemistry
- Electrochemistry
- Give two differences between Galvanic Cell and Electrolytic cell.
- PSEB XII - 2025
- Chemistry
- Electrochemistry
View More Questions
Questions Asked in COMEDK UGET exam
- Given that the freezing point of benzene is $ 5.48^\circ C $ and its $ K_f $ value is $ 5.12^\circ C/m $, what would be the freezing point of a solution of 20 g of propane in 400 g of benzene?
- COMEDK UGET - 2024
- Colligative Properties
200 ml of an aqueous solution contains 3.6 g of Glucose and 1.2 g of Urea maintained at a temperature equal to 27$^{\circ}$C. What is the Osmotic pressure of the solution in atmosphere units?
Given Data R = 0.082 L atm K$^{-1}$ mol$^{-1}$
Molecular Formula: Glucose = C$_6$H$_{12}$O$_6$, Urea = NH$_2$CONH$_2$- COMEDK UGET - 2024
- Colligative Properties
- An inorganic compound W undergoes the following reactions: $ W + \text{Na}_2\text{CO}_3 \xrightarrow{\text{O}_2 / \text{heat}} X + H^+ \xrightarrow{} Y(s) $ $ Y(aq) + \text{KCl} (aq) \xrightarrow{} Z(s) $ Z appears in the form of orange crystals and is used as an oxidising agent in acid medium. Identify the compound W.
- COMEDK UGET - 2024
- coordination compounds
- A current of 3.0 A is passed through 750 ml of 0.45 M solution of CuSO₄ for 2 hours with a current efficiency of 90\%. If the volume of the solution is assumed to remain constant, what would be the final molarity of CuSO₄ solution?
- COMEDK UGET - 2024
- Solutions
- For a reaction $ 5X + Y \to 3Z $, the rate of formation of Z is $ 2.4 \times 10^{-5} \, \text{mol L}^{-1} \text{s}^{-1} $. Calculate the average rate of disappearance of X.
- COMEDK UGET - 2024
- Stoichiometry and Stoichiometric Calculations
View More Questions
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.