The amount of electricity required to deposit one mole of Copper from Copper sulphate solution is –
(A) 1 Faraday
(B) 2.33 Faraday
(C) 2 Faraday
(D) 1.33 Faraday
1 Answers
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The amount of electricity required to produce one mole of copper from copper sulphate solution will be:
Correct Answer - C `Cu^(2+) + 2e^(-) rarr Cu (s)` 1 mole copper requires 2 mole electron i.e., 2 faraday charge
2 Answers 1 views
When 96500 coulombs of electricity are passed through nickel sulphate solution, the amount of nickel deposited will be
Correct Answer - B 1 faraday deposits 1 equivalent of nickel 1 equivalent of `Ni = 1//2` mole of nickel
2 Answers 1 views
A steady current of `10.0` A is maintained in a copper voltameter . Calculate the time required to deposit `2.5` g of copper . Relative atomic mass of
`because m`=Zit and `Z=(E)/(F)=(M)/(pF) therefore m=(Mit)/(pF)` where m=2.5g. `F=96500C//"mol",M=63.5,i=10A` and p=2 `therefore t=(mpF)/(Mi)=(2.5xx2xx96500)/( 63.5xx10)= 760s`
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A copper refining cell consists of two parallel copper plate electrodes 5 cm apart and 1 metre squre, immersed in a copper sulphate solution of resist
`m=Zit=Z((V)/(R))t` `rARr V=(mR)/(Zt)=(mrhol)/(Zat)` `=(0.66xx1.2xx10^(-2)xx5xx10^(-2))/(3.33xx10^(-7)xx1xx60xx60)` =0.33 volt
2 Answers 1 views
When a quantity of electricity is passed through `CuSO_(4)` solution, 0.16 g of copper gets deposited. If the same quantity of electricity is passed t
Correct Answer - B Number of equivalents of copper deposited `=0.16/32=0.005` Volume of `H_(2)` gas at STP `=11.2xx0.005` `=0.056` litre `=56 cm^(3)`
2 Answers 1 views
The "mole"s of electrons required to deposit 1 gm equivalent aluminium (at wt. =27) from a solution of aluminium chloride will be:
Correct Answer - A `Al^(3+)+3e^(-)toAl` So mole of `e^(-)=3`
2 Answers 1 views
One mole of an organic amide (A) on alkaline hydrolysis gives one mole of `NH_(3)` and one mole of a monobasic acid of equivalent mass 74. What is the
`R-overset(O)overset(||)C-NH_(2)+OH^(-)toR-overset(O)overset(||)C-O^(-)+NH_(3)` R+45=74orR=29i.e., `CH_(3)CH_(2)-` Monobsic acid=`CH_(3)CH_(2)COOH,` Mol. Mass=`CH_(3)CH_(2)CONH_(2)=73`
2 Answers 2 views
How long will it take to deposit eleectrolyically voltsmeter127 g of copper on the copper on the cathode of a copper voltameter by a currect of 50 A?
Correct Answer - 7711 s
2 Answers 1 views
Calculate the currect required to deposit 1 g copper in 30 minutes in a voltmeter contaning cupric sulphate . Atommic mass od slver =107.9 , atomic ma
Correct Answer - 1.713 A
2 Answers 1 views
i. Saving Deposit, Recurring Deposit, Cash Credit. Fixed Deposit ii. Overdraft, Fixed Deposit, Discounting of Bills, Cash Credit
i. Cash Credit ii. Fixed Deposit
2 Answers 1 views