330236 The mass of metal deposited by the electrolysis of an aqueous solution of metal ions increases in direct proportion to which property?
(P) Electrolysis current
(Q) Electrolysis time
(R) Metal ion charge

330240 The amount of electricity required to prepare 5.4 kg of aluminium from aluminium oxide by electrolysis is \({\mathrm{X \times 10^{7} \mathrm{C}}}\). The value of ' X ' is ____ .
\({\mathrm{\left[1 \mathrm{~F}=96500 \mathrm{~C} \mathrm{~mol}^{-1}\right]}}\)

330241 How many minutes will it take to plate out 5.2 g of Cr from a \({{\rm{O}}_{\rm{2}}}{\left( {{\rm{S}}{{\rm{O}}_{\rm{4}}}} \right)_{\rm{3}}}\) solution using a current of 9.65 A? (Atomic mass: Cr = 52.0)

330242 Match the column I with column II and mark the appropriate choice.
Column I
Column II
A
Electrochemical equivalent
P
Potential difference \( \times \) Quantity of charge
B
Faraday
Q
Mass of substance deposited by one coulomb of charge
C
Ampere
R
Charge carried by one mole of electrons
D
Electrical energy
S
One coulomb of electric charge passed through one second

330243 Assertion :
One coulomb of electric charge deposits weight equal to the electrochemical equivalent of the substance.
Reason :
One Faraday deposits one mole of the substance.

330236 The mass of metal deposited by the electrolysis of an aqueous solution of metal ions increases in direct proportion to which property?
(P) Electrolysis current
(Q) Electrolysis time
(R) Metal ion charge

330240 The amount of electricity required to prepare 5.4 kg of aluminium from aluminium oxide by electrolysis is \({\mathrm{X \times 10^{7} \mathrm{C}}}\). The value of ' X ' is ____ .
\({\mathrm{\left[1 \mathrm{~F}=96500 \mathrm{~C} \mathrm{~mol}^{-1}\right]}}\)

330241 How many minutes will it take to plate out 5.2 g of Cr from a \({{\rm{O}}_{\rm{2}}}{\left( {{\rm{S}}{{\rm{O}}_{\rm{4}}}} \right)_{\rm{3}}}\) solution using a current of 9.65 A? (Atomic mass: Cr = 52.0)

330242 Match the column I with column II and mark the appropriate choice.
Column I
Column II
A
Electrochemical equivalent
P
Potential difference \( \times \) Quantity of charge
B
Faraday
Q
Mass of substance deposited by one coulomb of charge
C
Ampere
R
Charge carried by one mole of electrons
D
Electrical energy
S
One coulomb of electric charge passed through one second

330243 Assertion :
One coulomb of electric charge deposits weight equal to the electrochemical equivalent of the substance.
Reason :
One Faraday deposits one mole of the substance.

330236 The mass of metal deposited by the electrolysis of an aqueous solution of metal ions increases in direct proportion to which property?
(P) Electrolysis current
(Q) Electrolysis time
(R) Metal ion charge

330240 The amount of electricity required to prepare 5.4 kg of aluminium from aluminium oxide by electrolysis is \({\mathrm{X \times 10^{7} \mathrm{C}}}\). The value of ' X ' is ____ .
\({\mathrm{\left[1 \mathrm{~F}=96500 \mathrm{~C} \mathrm{~mol}^{-1}\right]}}\)

330241 How many minutes will it take to plate out 5.2 g of Cr from a \({{\rm{O}}_{\rm{2}}}{\left( {{\rm{S}}{{\rm{O}}_{\rm{4}}}} \right)_{\rm{3}}}\) solution using a current of 9.65 A? (Atomic mass: Cr = 52.0)

330242 Match the column I with column II and mark the appropriate choice.
Column I
Column II
A
Electrochemical equivalent
P
Potential difference \( \times \) Quantity of charge
B
Faraday
Q
Mass of substance deposited by one coulomb of charge
C
Ampere
R
Charge carried by one mole of electrons
D
Electrical energy
S
One coulomb of electric charge passed through one second

330243 Assertion :
One coulomb of electric charge deposits weight equal to the electrochemical equivalent of the substance.
Reason :
One Faraday deposits one mole of the substance.

330236 The mass of metal deposited by the electrolysis of an aqueous solution of metal ions increases in direct proportion to which property?
(P) Electrolysis current
(Q) Electrolysis time
(R) Metal ion charge

330240 The amount of electricity required to prepare 5.4 kg of aluminium from aluminium oxide by electrolysis is \({\mathrm{X \times 10^{7} \mathrm{C}}}\). The value of ' X ' is ____ .
\({\mathrm{\left[1 \mathrm{~F}=96500 \mathrm{~C} \mathrm{~mol}^{-1}\right]}}\)

330241 How many minutes will it take to plate out 5.2 g of Cr from a \({{\rm{O}}_{\rm{2}}}{\left( {{\rm{S}}{{\rm{O}}_{\rm{4}}}} \right)_{\rm{3}}}\) solution using a current of 9.65 A? (Atomic mass: Cr = 52.0)

330242 Match the column I with column II and mark the appropriate choice.
Column I
Column II
A
Electrochemical equivalent
P
Potential difference \( \times \) Quantity of charge
B
Faraday
Q
Mass of substance deposited by one coulomb of charge
C
Ampere
R
Charge carried by one mole of electrons
D
Electrical energy
S
One coulomb of electric charge passed through one second

330243 Assertion :
One coulomb of electric charge deposits weight equal to the electrochemical equivalent of the substance.
Reason :
One Faraday deposits one mole of the substance.

330236 The mass of metal deposited by the electrolysis of an aqueous solution of metal ions increases in direct proportion to which property?
(P) Electrolysis current
(Q) Electrolysis time
(R) Metal ion charge

330240 The amount of electricity required to prepare 5.4 kg of aluminium from aluminium oxide by electrolysis is \({\mathrm{X \times 10^{7} \mathrm{C}}}\). The value of ' X ' is ____ .
\({\mathrm{\left[1 \mathrm{~F}=96500 \mathrm{~C} \mathrm{~mol}^{-1}\right]}}\)

330241 How many minutes will it take to plate out 5.2 g of Cr from a \({{\rm{O}}_{\rm{2}}}{\left( {{\rm{S}}{{\rm{O}}_{\rm{4}}}} \right)_{\rm{3}}}\) solution using a current of 9.65 A? (Atomic mass: Cr = 52.0)

330242 Match the column I with column II and mark the appropriate choice.
Column I
Column II
A
Electrochemical equivalent
P
Potential difference \( \times \) Quantity of charge
B
Faraday
Q
Mass of substance deposited by one coulomb of charge
C
Ampere
R
Charge carried by one mole of electrons
D
Electrical energy
S
One coulomb of electric charge passed through one second

330243 Assertion :
One coulomb of electric charge deposits weight equal to the electrochemical equivalent of the substance.
Reason :
One Faraday deposits one mole of the substance.