276035 A $100.0 \mathrm{~mL}$ dilute solution of $\mathrm{Ag}^{+}$is electrolysed for $\mathbf{1 5 . 0}$ minutes with a current of $1.25 \mathrm{~mA}$ and the silver is removed completely. What was the initial $\left[\mathrm{Ag}^{+}\right]$?

276036 One coulomb of charge passes through a solution of $\mathrm{AgNO}_{3}$ and $\mathrm{CuSO}_{4}$ connected in series and the concentration of two solutions being in the ratio $1: 2$. The ratio of amount of $\mathrm{Ag}$ and $\mathrm{Cu}$ deposited on Pt electrode is

276037 How much Coulomb needed to convert 1 mole of $\mathrm{MnO}_{4}$ into $\mathrm{Mn}^{2+}$ ?

276038 $4.5 \mathrm{~g}$ of aluminum (atomic mass $27 \mathrm{amu}$ ) is deposited at cathode from $\mathrm{Al}^{3+}$ solution by a certain quantity of electric charge. The volume of hydrogen produced at STP from $\mathrm{H}^{+}$ions in solution by the same quantity of electric charge will be

276039 The weight of $\mathrm{Cu}$ deposited, when 2 Faraday of electricity is passed will be

276035 A $100.0 \mathrm{~mL}$ dilute solution of $\mathrm{Ag}^{+}$is electrolysed for $\mathbf{1 5 . 0}$ minutes with a current of $1.25 \mathrm{~mA}$ and the silver is removed completely. What was the initial $\left[\mathrm{Ag}^{+}\right]$?

276036 One coulomb of charge passes through a solution of $\mathrm{AgNO}_{3}$ and $\mathrm{CuSO}_{4}$ connected in series and the concentration of two solutions being in the ratio $1: 2$. The ratio of amount of $\mathrm{Ag}$ and $\mathrm{Cu}$ deposited on Pt electrode is

276037 How much Coulomb needed to convert 1 mole of $\mathrm{MnO}_{4}$ into $\mathrm{Mn}^{2+}$ ?

276038 $4.5 \mathrm{~g}$ of aluminum (atomic mass $27 \mathrm{amu}$ ) is deposited at cathode from $\mathrm{Al}^{3+}$ solution by a certain quantity of electric charge. The volume of hydrogen produced at STP from $\mathrm{H}^{+}$ions in solution by the same quantity of electric charge will be

276039 The weight of $\mathrm{Cu}$ deposited, when 2 Faraday of electricity is passed will be

276035 A $100.0 \mathrm{~mL}$ dilute solution of $\mathrm{Ag}^{+}$is electrolysed for $\mathbf{1 5 . 0}$ minutes with a current of $1.25 \mathrm{~mA}$ and the silver is removed completely. What was the initial $\left[\mathrm{Ag}^{+}\right]$?

276036 One coulomb of charge passes through a solution of $\mathrm{AgNO}_{3}$ and $\mathrm{CuSO}_{4}$ connected in series and the concentration of two solutions being in the ratio $1: 2$. The ratio of amount of $\mathrm{Ag}$ and $\mathrm{Cu}$ deposited on Pt electrode is

276037 How much Coulomb needed to convert 1 mole of $\mathrm{MnO}_{4}$ into $\mathrm{Mn}^{2+}$ ?

276038 $4.5 \mathrm{~g}$ of aluminum (atomic mass $27 \mathrm{amu}$ ) is deposited at cathode from $\mathrm{Al}^{3+}$ solution by a certain quantity of electric charge. The volume of hydrogen produced at STP from $\mathrm{H}^{+}$ions in solution by the same quantity of electric charge will be

276039 The weight of $\mathrm{Cu}$ deposited, when 2 Faraday of electricity is passed will be

276035 A $100.0 \mathrm{~mL}$ dilute solution of $\mathrm{Ag}^{+}$is electrolysed for $\mathbf{1 5 . 0}$ minutes with a current of $1.25 \mathrm{~mA}$ and the silver is removed completely. What was the initial $\left[\mathrm{Ag}^{+}\right]$?

276036 One coulomb of charge passes through a solution of $\mathrm{AgNO}_{3}$ and $\mathrm{CuSO}_{4}$ connected in series and the concentration of two solutions being in the ratio $1: 2$. The ratio of amount of $\mathrm{Ag}$ and $\mathrm{Cu}$ deposited on Pt electrode is

276037 How much Coulomb needed to convert 1 mole of $\mathrm{MnO}_{4}$ into $\mathrm{Mn}^{2+}$ ?

276038 $4.5 \mathrm{~g}$ of aluminum (atomic mass $27 \mathrm{amu}$ ) is deposited at cathode from $\mathrm{Al}^{3+}$ solution by a certain quantity of electric charge. The volume of hydrogen produced at STP from $\mathrm{H}^{+}$ions in solution by the same quantity of electric charge will be

276039 The weight of $\mathrm{Cu}$ deposited, when 2 Faraday of electricity is passed will be

276035 A $100.0 \mathrm{~mL}$ dilute solution of $\mathrm{Ag}^{+}$is electrolysed for $\mathbf{1 5 . 0}$ minutes with a current of $1.25 \mathrm{~mA}$ and the silver is removed completely. What was the initial $\left[\mathrm{Ag}^{+}\right]$?

276036 One coulomb of charge passes through a solution of $\mathrm{AgNO}_{3}$ and $\mathrm{CuSO}_{4}$ connected in series and the concentration of two solutions being in the ratio $1: 2$. The ratio of amount of $\mathrm{Ag}$ and $\mathrm{Cu}$ deposited on Pt electrode is

276037 How much Coulomb needed to convert 1 mole of $\mathrm{MnO}_{4}$ into $\mathrm{Mn}^{2+}$ ?

276038 $4.5 \mathrm{~g}$ of aluminum (atomic mass $27 \mathrm{amu}$ ) is deposited at cathode from $\mathrm{Al}^{3+}$ solution by a certain quantity of electric charge. The volume of hydrogen produced at STP from $\mathrm{H}^{+}$ions in solution by the same quantity of electric charge will be

276039 The weight of $\mathrm{Cu}$ deposited, when 2 Faraday of electricity is passed will be