The quantity of silver deposited when one coulomb charge is passed through\(AgNO_3\)solution:
- 0.1 g atom of silver
- 1 chemical equivalent of silver
- 1 g of silver
- 1 electrochemical equivalent of silver
The Correct Option is D
Approach Solution - 1
The amount of a substance deposited during electrolysis is determined using Faraday’s laws of electrolysis. The formula is:
\[W = ZIt,\]
where:
- \(W\) is the mass of the substance deposited,
- \(Z\) is the electrochemical equivalent of the substance,
- \(I\) is the current passed, and
- \(t\) is the time for which the current is passed.
Step 1: Relating charge to electrochemical equivalent
We know that:
\[Q = It,\]
where \(Q\) is the total charge passed through the solution. Substituting this into the equation for \(W\), we get:
\[W = ZQ\]
Step 2: Deposition of silver
For one coulomb of charge (\(Q = 1 \, \text{C}\)), the mass of silver deposited is directly proportional to the electrochemical equivalent (\(Z\)) of silver. Thus:
\[W = ZQ = (\text{electrochemical equivalent of silver}).\]
Step 3: Conclusion
The quantity of silver deposited when one coulomb of charge is passed is equal to the electrochemical equivalent of silver. This matches the given option.
Final Answer: (4).
Approach Solution -2
The mass of a substance deposited or liberated during electrolysis is directly proportional to the quantity of electricity (charge) passed through the solution.
According to Faraday’s first law of electrolysis:
\[ m = ZQ \] where:
m = mass of the substance deposited (in grams)
Z = electrochemical equivalent (in g/C)
Q = total charge passed (in coulombs)
Step 2: Given data.
Charge passed, Q = 1 coulomb
Step 3: Substitute in the formula.
\[ m = Z \times Q = Z \times 1 = Z \]
Therefore, the mass of silver deposited = 1 electrochemical equivalent of silver.
Step 4: Final Answer.
The quantity of silver deposited is:
\[ \boxed{1 \, \text{electrochemical equivalent of silver}} \]
Final Answer: 1 electrochemical equivalent of silver
Top JEE Main Chemistry Questions
What will be the equilibrium constant of the given reaction carried out in a \(5 \,L\) vessel and having equilibrium amounts of \(A_2\) and \(A\) as \(0.5\) mole and \(2 \times 10^{-6}\) mole respectively?
The reaction : \(A_2 \rightleftharpoons 2A\)- At equilibrium the concentrations of and in a sealed vessel at . What will be for the reaction
- Find out the major products from the following reactions
Cobalt chloride when dissolved in water forms pink colored complex $X$ which has octahedral geometry. This solution on treating with cone $HCl$ forms deep blue complex, $\underline{Y}$ which has a $\underline{Z}$ geometry $X, Y$ and $Z$, respectively, are
- The correct order of atomic radii is:
Top JEE Main Electrochemistry Questions
- $\text{The hydrogen electrode is dipped in a solution of pH = 3 at } 25^{\circ}\text{C. The potential of the electrode will be } -\_\_\_\_\_ \times 10^{-2} \text{ V.}$
$\left( \frac{2.303RT}{F} = 0.059 \, \text{V} \right)$ - The mass of zinc produced by the electrolysis of zinc sulfate solution with a steady current of 0.015 A for 15 minutes is _____ \( \times \, 10^{-4} \) g.
(Atomic mass of zinc = 65.4 amu) - The mass of silver (Molar mass of Ag : 108 gmol–1 ) displaced by a quantity of electricity which displaces 5600 mL of O2 at S.T.P. will be _____ g.
- The potential for the given half cell at 298 K is\[(-) \ldots \times 10^{-2} \, \text{V}.\]\[2\text{H}^+ (\text{aq}) + 2e^- \rightarrow \text{H}_2 (\text{g})\]\[[\text{H}^+] = 1M, \, P_{\text{H}_2} = 2 \, \text{atm}\](Given: \( 2.303 \frac{RT}{F} = 0.06 \, \text{V}, \log 2 = 0.3 \))
- The metals that are employed in the battery industries are
A. Fe
B. Mn
C. Ni
D. Cr
E. Cd
Choose the correct answer from the options given below:
Top JEE Main Questions
- In a hydrogen like atom, when an electron jumps from the $M$ - shell to the $L$ - shell, the wavelength of emitted radiation is $\lambda$. If an electron jumps from $N$-shell to the $L$-shell, the wavelength of emitted radiation will be :
- Two masses $m$ and $\frac{m}{2}$ are connected at the two ends of a massless rigid rod of length $l$. The rod is suspended by a thin wire of torsional constant $k$ at the centre of mass of the rod-mass system(see figure). Because of torsional constant $k$, the restoring torque is $\tau =k\theta$ for angular displacement $\theta$. If the rod is rota ted by $\theta_0$ and released, the tension in it when it passes through its mean position will be:
What will be the equilibrium constant of the given reaction carried out in a \(5 \,L\) vessel and having equilibrium amounts of \(A_2\) and \(A\) as \(0.5\) mole and \(2 \times 10^{-6}\) mole respectively?
The reaction : \(A_2 \rightleftharpoons 2A\)- The value of is
- The number of terms of an is even. The sum of the odd terms is and of the even terms is . The last term exceeds the first by . Then the number of terms in the series is ______.