Three voltameters containing aqueous solution | vedclass

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

Question

(B) According to Faraday's law of electrolysis,the mass deposited is given by $w = \frac{E 	imes I_{eff} 	imes t}{96500}$.Here,$w = 10.8 \ g$,$E_{Ag

Vedclass · Accepted Answer

$0.536$

Vedclass · Answer

(B) According to Faraday's law of electrolysis,the mass deposited is given by $w = \frac{E 	imes I_{eff} 	imes t}{96500}$.Here,$w = 10.8 \ g$,$E_{Ag} = 108 \ g/mol$,$t = 10 \ hours = 36000 \ s$.The current efficiency is $50\%$,so the effective current $I_{eff} = I 	imes 0.5$.Substituting the values: $10.8 = \frac{108 	imes (I 	imes 0.5) 	imes 36000}{96500}$.$10.8 = \frac{108 	imes I 	imes 18000}{96500}$.$I = \frac{10.8 	imes 96500}{108 	imes 18000} = \frac{0.1 	imes 96500}{18000} = \frac{9650}{18000} \approx 0.536 \ A$.

Similar Questions

The ratio of weights of hydrogen gas liberated and magnesium deposited by passing the same amount of electricity from aqueous $H_2SO_4$ and fused $MgSO_4$ are :

What is the quantity of electricity required to produce $4.8 \ g$ of $Mg$ (molar mass $= 24 \ g \ mol^{-1}$) from its salt solution (in $F$)?

In electrolysis,if the duration of the passage of current is doubled,the mass liberated is

What is the nature of the Faraday constant?

How long should aqueous $NaCl$ be electrolysed by passing $100 \ A$ current,so that $0.5 \ mol$ chlorine is released at anode?

Vedclass Test Series

Exam Paper Generator

Online Exam Module