275994 In two separate experiments, the same quantity of electricity was passed through silver and gold solutions [Assume ' $t$ ' constant] The amounts of $\mathrm{Ag}$ and $\mathrm{Au}$ deposited are 2.15 and $1.31 \mathrm{~g}$, respectively. The valency of gold is [Atomic mass of $\mathrm{Ag}=107.9 ; \mathrm{Au}=197$ ]

275995 If 5 ampere of current is passed for 193 seconds through a solution containing Copper salt, 0.32 g of copper is deposited. What is the oxidation state of the $\mathrm{Cu}$ in the salt?

275996 A certain quantity of electricity is passed through aqueous $\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}$ and $\mathrm{CuSO}_{4}$ solutions connected in series. $0.09 \mathrm{~g}$ of $\mathrm{Al}$ is deposited on cathode during electrolysis. The amount of copper deposited on cathode in grams is
(At. wt. of

275997 When 9.65 $\mathrm{C}$ of electricity is passed through a solution of $\mathrm{AgNO}_{3}$ (atomic weight of silver 108), the amount of silver deposited is :

275998 What is the approximate quantity of electricity (in coulomb) required to deposit all the silver from $250 \mathrm{~mL}$ of $1 \mathrm{M} \mathrm{AgNO}_{3}$ aqueous solution?

275994 In two separate experiments, the same quantity of electricity was passed through silver and gold solutions [Assume ' $t$ ' constant] The amounts of $\mathrm{Ag}$ and $\mathrm{Au}$ deposited are 2.15 and $1.31 \mathrm{~g}$, respectively. The valency of gold is [Atomic mass of $\mathrm{Ag}=107.9 ; \mathrm{Au}=197$ ]

275995 If 5 ampere of current is passed for 193 seconds through a solution containing Copper salt, 0.32 g of copper is deposited. What is the oxidation state of the $\mathrm{Cu}$ in the salt?

275996 A certain quantity of electricity is passed through aqueous $\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}$ and $\mathrm{CuSO}_{4}$ solutions connected in series. $0.09 \mathrm{~g}$ of $\mathrm{Al}$ is deposited on cathode during electrolysis. The amount of copper deposited on cathode in grams is
(At. wt. of

275997 When 9.65 $\mathrm{C}$ of electricity is passed through a solution of $\mathrm{AgNO}_{3}$ (atomic weight of silver 108), the amount of silver deposited is :

275998 What is the approximate quantity of electricity (in coulomb) required to deposit all the silver from $250 \mathrm{~mL}$ of $1 \mathrm{M} \mathrm{AgNO}_{3}$ aqueous solution?

275994 In two separate experiments, the same quantity of electricity was passed through silver and gold solutions [Assume ' $t$ ' constant] The amounts of $\mathrm{Ag}$ and $\mathrm{Au}$ deposited are 2.15 and $1.31 \mathrm{~g}$, respectively. The valency of gold is [Atomic mass of $\mathrm{Ag}=107.9 ; \mathrm{Au}=197$ ]

275995 If 5 ampere of current is passed for 193 seconds through a solution containing Copper salt, 0.32 g of copper is deposited. What is the oxidation state of the $\mathrm{Cu}$ in the salt?

275996 A certain quantity of electricity is passed through aqueous $\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}$ and $\mathrm{CuSO}_{4}$ solutions connected in series. $0.09 \mathrm{~g}$ of $\mathrm{Al}$ is deposited on cathode during electrolysis. The amount of copper deposited on cathode in grams is
(At. wt. of

275997 When 9.65 $\mathrm{C}$ of electricity is passed through a solution of $\mathrm{AgNO}_{3}$ (atomic weight of silver 108), the amount of silver deposited is :

275998 What is the approximate quantity of electricity (in coulomb) required to deposit all the silver from $250 \mathrm{~mL}$ of $1 \mathrm{M} \mathrm{AgNO}_{3}$ aqueous solution?

275994 In two separate experiments, the same quantity of electricity was passed through silver and gold solutions [Assume ' $t$ ' constant] The amounts of $\mathrm{Ag}$ and $\mathrm{Au}$ deposited are 2.15 and $1.31 \mathrm{~g}$, respectively. The valency of gold is [Atomic mass of $\mathrm{Ag}=107.9 ; \mathrm{Au}=197$ ]

275995 If 5 ampere of current is passed for 193 seconds through a solution containing Copper salt, 0.32 g of copper is deposited. What is the oxidation state of the $\mathrm{Cu}$ in the salt?

275996 A certain quantity of electricity is passed through aqueous $\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}$ and $\mathrm{CuSO}_{4}$ solutions connected in series. $0.09 \mathrm{~g}$ of $\mathrm{Al}$ is deposited on cathode during electrolysis. The amount of copper deposited on cathode in grams is
(At. wt. of

275997 When 9.65 $\mathrm{C}$ of electricity is passed through a solution of $\mathrm{AgNO}_{3}$ (atomic weight of silver 108), the amount of silver deposited is :

275998 What is the approximate quantity of electricity (in coulomb) required to deposit all the silver from $250 \mathrm{~mL}$ of $1 \mathrm{M} \mathrm{AgNO}_{3}$ aqueous solution?

275994 In two separate experiments, the same quantity of electricity was passed through silver and gold solutions [Assume ' $t$ ' constant] The amounts of $\mathrm{Ag}$ and $\mathrm{Au}$ deposited are 2.15 and $1.31 \mathrm{~g}$, respectively. The valency of gold is [Atomic mass of $\mathrm{Ag}=107.9 ; \mathrm{Au}=197$ ]

275995 If 5 ampere of current is passed for 193 seconds through a solution containing Copper salt, 0.32 g of copper is deposited. What is the oxidation state of the $\mathrm{Cu}$ in the salt?

275996 A certain quantity of electricity is passed through aqueous $\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}$ and $\mathrm{CuSO}_{4}$ solutions connected in series. $0.09 \mathrm{~g}$ of $\mathrm{Al}$ is deposited on cathode during electrolysis. The amount of copper deposited on cathode in grams is
(At. wt. of

275997 When 9.65 $\mathrm{C}$ of electricity is passed through a solution of $\mathrm{AgNO}_{3}$ (atomic weight of silver 108), the amount of silver deposited is :

275998 What is the approximate quantity of electricity (in coulomb) required to deposit all the silver from $250 \mathrm{~mL}$ of $1 \mathrm{M} \mathrm{AgNO}_{3}$ aqueous solution?