01. Faraday's Law
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ELECTROCHEMISTRY

275999 What is the time (in sec) required for depositing all the silver present in $125 \mathrm{~mL}$ of 1 $\mathrm{M} \mathrm{AgNO}_{3}$ solution by passing a current of 241.25 A?
$(1 \mathrm{~F}=96500 \mathrm{C})$

1 10
2 50
3 1000
4 100
AP-EAMCET-2006
ELECTROCHEMISTRY

276000 Assertion (A) : A current of $96.5 \mathrm{~A}$ is passed into aqueous $\mathrm{AgNO}_{3}$ solution for $100 \mathrm{~s}$. The weight of silver deposited is $10.89 \mathrm{~g}$ (at.wt. of $\mathrm{Ag}=108$ ).
Reason (R) : The mass of a substance deposited during the electrolysis of an electrolyte is inversely proportional to the quantity of electricity passing through the electrolyte.

1 Both (A) and (R) are true and (R) is the correct explanation of $(\mathrm{A})$.
2 Both (A) and (R) are true, but (R) is not the correct explanation of (A).
3 (A) is true, but (R) is false.
4 (A) is false, but (R) is true.
AP-EAMCET-2006
ELECTROCHEMISTRY

276001 When same quantity of electricity is passed through aqueous $\mathrm{AgNO}_{3}$ and $\mathrm{H}_{2} \mathrm{SO}_{4}$ solutions connected in series, $5.04 \times 10^{-2} \mathrm{~g}$ of $\mathrm{H}_{2}$ is liberated. What is the mass of silver (in gram) deposited? (Eq. wts. of hydrogen $=1.008$, silver $=108$ )

1 54
2 0.54
3 5.4
4 10.8
AP-EAMCET-2008
ELECTROCHEMISTRY

276022 How many Faradays are needed for reduction of 2.5 mole of $\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}$ into $\mathrm{Cr}^{3+}$ ?

1 15
2 12
3 6
4 3
GUJCET-2007
NEET DIGITAL LIBRARY
ELECTROCHEMISTRY

275999 What is the time (in sec) required for depositing all the silver present in $125 \mathrm{~mL}$ of 1 $\mathrm{M} \mathrm{AgNO}_{3}$ solution by passing a current of 241.25 A?
$(1 \mathrm{~F}=96500 \mathrm{C})$

1 10
2 50
3 1000
4 100
AP-EAMCET-2006
ELECTROCHEMISTRY

276000 Assertion (A) : A current of $96.5 \mathrm{~A}$ is passed into aqueous $\mathrm{AgNO}_{3}$ solution for $100 \mathrm{~s}$. The weight of silver deposited is $10.89 \mathrm{~g}$ (at.wt. of $\mathrm{Ag}=108$ ).
Reason (R) : The mass of a substance deposited during the electrolysis of an electrolyte is inversely proportional to the quantity of electricity passing through the electrolyte.

1 Both (A) and (R) are true and (R) is the correct explanation of $(\mathrm{A})$.
2 Both (A) and (R) are true, but (R) is not the correct explanation of (A).
3 (A) is true, but (R) is false.
4 (A) is false, but (R) is true.
AP-EAMCET-2006
ELECTROCHEMISTRY

276001 When same quantity of electricity is passed through aqueous $\mathrm{AgNO}_{3}$ and $\mathrm{H}_{2} \mathrm{SO}_{4}$ solutions connected in series, $5.04 \times 10^{-2} \mathrm{~g}$ of $\mathrm{H}_{2}$ is liberated. What is the mass of silver (in gram) deposited? (Eq. wts. of hydrogen $=1.008$, silver $=108$ )

1 54
2 0.54
3 5.4
4 10.8
AP-EAMCET-2008
ELECTROCHEMISTRY

276022 How many Faradays are needed for reduction of 2.5 mole of $\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}$ into $\mathrm{Cr}^{3+}$ ?

1 15
2 12
3 6
4 3
GUJCET-2007
Join With Us for More Updates
ELECTROCHEMISTRY

275999 What is the time (in sec) required for depositing all the silver present in $125 \mathrm{~mL}$ of 1 $\mathrm{M} \mathrm{AgNO}_{3}$ solution by passing a current of 241.25 A?
$(1 \mathrm{~F}=96500 \mathrm{C})$

1 10
2 50
3 1000
4 100
AP-EAMCET-2006
ELECTROCHEMISTRY

276000 Assertion (A) : A current of $96.5 \mathrm{~A}$ is passed into aqueous $\mathrm{AgNO}_{3}$ solution for $100 \mathrm{~s}$. The weight of silver deposited is $10.89 \mathrm{~g}$ (at.wt. of $\mathrm{Ag}=108$ ).
Reason (R) : The mass of a substance deposited during the electrolysis of an electrolyte is inversely proportional to the quantity of electricity passing through the electrolyte.

1 Both (A) and (R) are true and (R) is the correct explanation of $(\mathrm{A})$.
2 Both (A) and (R) are true, but (R) is not the correct explanation of (A).
3 (A) is true, but (R) is false.
4 (A) is false, but (R) is true.
AP-EAMCET-2006
ELECTROCHEMISTRY

276001 When same quantity of electricity is passed through aqueous $\mathrm{AgNO}_{3}$ and $\mathrm{H}_{2} \mathrm{SO}_{4}$ solutions connected in series, $5.04 \times 10^{-2} \mathrm{~g}$ of $\mathrm{H}_{2}$ is liberated. What is the mass of silver (in gram) deposited? (Eq. wts. of hydrogen $=1.008$, silver $=108$ )

1 54
2 0.54
3 5.4
4 10.8
AP-EAMCET-2008
ELECTROCHEMISTRY

276022 How many Faradays are needed for reduction of 2.5 mole of $\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}$ into $\mathrm{Cr}^{3+}$ ?

1 15
2 12
3 6
4 3
GUJCET-2007
For More Updates join with Us
ELECTROCHEMISTRY

275999 What is the time (in sec) required for depositing all the silver present in $125 \mathrm{~mL}$ of 1 $\mathrm{M} \mathrm{AgNO}_{3}$ solution by passing a current of 241.25 A?
$(1 \mathrm{~F}=96500 \mathrm{C})$

1 10
2 50
3 1000
4 100
AP-EAMCET-2006
ELECTROCHEMISTRY

276000 Assertion (A) : A current of $96.5 \mathrm{~A}$ is passed into aqueous $\mathrm{AgNO}_{3}$ solution for $100 \mathrm{~s}$. The weight of silver deposited is $10.89 \mathrm{~g}$ (at.wt. of $\mathrm{Ag}=108$ ).
Reason (R) : The mass of a substance deposited during the electrolysis of an electrolyte is inversely proportional to the quantity of electricity passing through the electrolyte.

1 Both (A) and (R) are true and (R) is the correct explanation of $(\mathrm{A})$.
2 Both (A) and (R) are true, but (R) is not the correct explanation of (A).
3 (A) is true, but (R) is false.
4 (A) is false, but (R) is true.
AP-EAMCET-2006
ELECTROCHEMISTRY

276001 When same quantity of electricity is passed through aqueous $\mathrm{AgNO}_{3}$ and $\mathrm{H}_{2} \mathrm{SO}_{4}$ solutions connected in series, $5.04 \times 10^{-2} \mathrm{~g}$ of $\mathrm{H}_{2}$ is liberated. What is the mass of silver (in gram) deposited? (Eq. wts. of hydrogen $=1.008$, silver $=108$ )

1 54
2 0.54
3 5.4
4 10.8
AP-EAMCET-2008
ELECTROCHEMISTRY

276022 How many Faradays are needed for reduction of 2.5 mole of $\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}$ into $\mathrm{Cr}^{3+}$ ?

1 15
2 12
3 6
4 3
GUJCET-2007