What mass of silver (Atomic mass = 108 text{ | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(D) Step $1$: Calculate moles of $O_2$ gas at $STP$. Moles = $5600 	ext{ mL} / 22400 	ext{ mL/mol} = 0.25 	ext{ mol}$.Step $2$: Calculate equivalen

Vedclass · Accepted Answer

$108.0$

Vedclass · Answer

(D) Step $1$: Calculate moles of $O_2$ gas at $STP$. Moles = $5600 	ext{ mL} / 22400 	ext{ mL/mol} = 0.25 	ext{ mol}$.Step $2$: Calculate equivalents of $O_2$. The reaction is $2H_2O ightarrow O_2 + 4H^+ + 4e^-$. The $n$-factor for $O_2$ is $4$. Equivalents = $0.25 	imes 4 = 1$.Step $3$: According to Faraday's law, equivalents of $Ag$ deposited = equivalents of $O_2$ displaced = $1$.Step $4$: Mass of $Ag$ = Equivalents $	imes$ Equivalent mass = $1 	imes 108 	ext{ g/mol} = 108 	ext{ g}$.

What mass of silver (Atomic mass = $108 \text{ g/mol}$) is deposited by a quantity of electricity that displaces $5600 \text{ mL}$ of $O_2$ gas at $STP$ (in $\text{ g}$)?

Similar Questions

Mass in grams of copper deposited by passing $9.6487 \ A$ current through a voltmeter containing copper sulphate solution for $100 \ s$ is (Given : Molar mass of $Cu: 63 \ g \ mol^{-1}, 1 \ F=96487 \ C$ ) (in $g$)

In the electrolysis of water,one Faraday of electrical energy would evolve

$7.5 \ A$ current is passed for $200 \ s$ through $AgNO_3$ solution. If experimentally $1.08 \ g$ of $Ag$ is obtained,then calculate the current efficiency (cell capacity). $[Ag = 108 \ u]$

How many coulombs are required for the oxidation of $1 \, mol$ of $H_2O_2$ to $O_2$?

State Faraday's laws of electrolysis and mention their uses.

Vedclass Test Series

Exam Paper Generator

Online Exam Module