A current of 5A is passed fir 5hours through three voltameters arranged in series, containing solution of copper sulphate. Silver nitrate and sulphuric acid. Calculate the masses of silver, copper and hydrogen liberated (E.C.E of silver `=11.18xx10^(-7) kg C^(-1)`m=, atomic weight of silver =107.88, atomic weight of copper =63.57 and atomic weight weight of hyrdrogen=1.008.)
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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
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Exactly 0.4 faraday electric charge is passed through three electrolytic cells in series, first containing `AgNO_(3)`, second `CuSO_(4)` and third `Fe
The cathodic reaction in the cells are respectively. `underset(("1 mole"),(108 g))(Ag^(+))+underset(("1 mole"),("1 F"))(e^(-)) rarr Ag` `underset(("1 mole"),(63.5 g))(Cu^(2+))+underset(("2 mole"),("2 F"))(2e^(-)) rarr Cu` and `underset(("1 mole"),(56 g))(Fe^(3+))+underset(("3 mole"),("3 F"))(3e^(-)) rarr Fe`...
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How long has a current of 3 ampere to be applied through a solution of silver nitrate to coat a metal surface of `80 cm^(2)` with 0.005 mm thick layer
Mass of silver to be deposited = volume `xx` density = area `xx` thickness `xx` density Given : Area `=80 cm^(2)`, thickness =0.0005 cm and density `=10.5 g//cm^(3)` Mass of...
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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)`
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An electric current is passed through three cells connected in series containing `ZnSO_(4)`, acidulated water and `CuSO_(4)` respectively. What amount
`because` Eq. of `Cu=Eq`. Of `Zn=Eq`. Of `H_(2)` `(6.25)/(31.70)=(W_(Zn))/(32.6)=(W_(H_(2)))/(1)`
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How long a current of 3 ampere has to be passed through a soulution of silver nitrate to coat a metal. Surface of `80cm^(2)` with a 0.005 mm thick lay
`i=3amp, rho_(Ag)=10.5gm//cc`, `A=80cm^(2)`, thickness `=0.005cm` mm Asked: time`=?` Formula used: `(Q)/(96500)=(w)/(E)` Explanation: `Q=` charge in column, `E=` equivalent wt. `w=` weight Substitution and calculation volume `=` area `xx` thickness `=80cm^(2)xx0.005xx(1)/(10)cm=0.04cm^(3)`...
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A current of 1.0 A was passed for 2 hr through a solution of cuprocyanide and 0.3745 g of copper was deposited on the cathode. Calculate the current e
Correct Answer - A m(theoretical)`=(63.5xx0.1xx7200)/(96500)=0.4738g` `therefore%` efficiency `=(0.3745)/(0.4738)xx100=79%`
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A steady current is passed for 25minutes through a silver voltameter and ammeter in series and 0.059g of silver of deposited. The ammeter reads 0.3A.
Correct Answer - 0.33A
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Electrochemical equivalent for copper is `3.2xx10^(-7) kg C^(-1)` An electric current of 3.0 A is passed through a copper voltamater for one minture .
Correct Answer - `5.76xx10^(6) kg`
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A current o f1.5 A is passed through a silver voltameter for 35 minutes .The mass of silver deposited during electrolysis is 3.528 g Calculate the ele
Correct Answer - 0.00112g/c
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