163234 Exactly 0.4 faraday electric charge is passed through two electolytic cells in series, first containing \(\mathrm{AgNO}_3\) and second \(\mathrm{CuSO}_4\) solution. How many gram of each metal will be deposited assuming only cathodic reaction in each cell respectively : [RBQ]

163235 During the electrolysis of brine \((\mathrm{NaCl})\) solution, what volume of chlorine gas, at STP is produced in the same time, in which \(\mathbf{5 . 0}\) litre of hydrogen gas is liberated under the same condition : [RBQ]

163236 Given that \(\mathrm{E}_{\mathrm{Fe}^{3+}+\mathrm{Fe}}^{\circ}=-0.036 \mathrm{~V}, \mathrm{E}_{\mathrm{Fe}^{2+} \mid \mathrm{Fe}}^{\circ}=-0.439 \mathrm{~V}\), the value of standard electrode potental for the change \(\mathrm{Fe}_{(\mathrm{aq})}^{3+}+\overline{\mathrm{e}} \rightarrow \mathrm{Fe}_{(\mathrm{aq})}^{2+}\) will be : [RBQ]

163237 Electrolysis of dilute aqueous \(\mathrm{NaCl}\) solution was carried out by passing 10 milliampere current. The time required to liberate \(224 \mathrm{ml}\) (S.T.P) of \(\mathrm{H}_2\) gas at the cathode is : [RBQ]

163234 Exactly 0.4 faraday electric charge is passed through two electolytic cells in series, first containing \(\mathrm{AgNO}_3\) and second \(\mathrm{CuSO}_4\) solution. How many gram of each metal will be deposited assuming only cathodic reaction in each cell respectively : [RBQ]

163235 During the electrolysis of brine \((\mathrm{NaCl})\) solution, what volume of chlorine gas, at STP is produced in the same time, in which \(\mathbf{5 . 0}\) litre of hydrogen gas is liberated under the same condition : [RBQ]

163236 Given that \(\mathrm{E}_{\mathrm{Fe}^{3+}+\mathrm{Fe}}^{\circ}=-0.036 \mathrm{~V}, \mathrm{E}_{\mathrm{Fe}^{2+} \mid \mathrm{Fe}}^{\circ}=-0.439 \mathrm{~V}\), the value of standard electrode potental for the change \(\mathrm{Fe}_{(\mathrm{aq})}^{3+}+\overline{\mathrm{e}} \rightarrow \mathrm{Fe}_{(\mathrm{aq})}^{2+}\) will be : [RBQ]

163237 Electrolysis of dilute aqueous \(\mathrm{NaCl}\) solution was carried out by passing 10 milliampere current. The time required to liberate \(224 \mathrm{ml}\) (S.T.P) of \(\mathrm{H}_2\) gas at the cathode is : [RBQ]

163234 Exactly 0.4 faraday electric charge is passed through two electolytic cells in series, first containing \(\mathrm{AgNO}_3\) and second \(\mathrm{CuSO}_4\) solution. How many gram of each metal will be deposited assuming only cathodic reaction in each cell respectively : [RBQ]

163235 During the electrolysis of brine \((\mathrm{NaCl})\) solution, what volume of chlorine gas, at STP is produced in the same time, in which \(\mathbf{5 . 0}\) litre of hydrogen gas is liberated under the same condition : [RBQ]

163236 Given that \(\mathrm{E}_{\mathrm{Fe}^{3+}+\mathrm{Fe}}^{\circ}=-0.036 \mathrm{~V}, \mathrm{E}_{\mathrm{Fe}^{2+} \mid \mathrm{Fe}}^{\circ}=-0.439 \mathrm{~V}\), the value of standard electrode potental for the change \(\mathrm{Fe}_{(\mathrm{aq})}^{3+}+\overline{\mathrm{e}} \rightarrow \mathrm{Fe}_{(\mathrm{aq})}^{2+}\) will be : [RBQ]

163237 Electrolysis of dilute aqueous \(\mathrm{NaCl}\) solution was carried out by passing 10 milliampere current. The time required to liberate \(224 \mathrm{ml}\) (S.T.P) of \(\mathrm{H}_2\) gas at the cathode is : [RBQ]

163234 Exactly 0.4 faraday electric charge is passed through two electolytic cells in series, first containing \(\mathrm{AgNO}_3\) and second \(\mathrm{CuSO}_4\) solution. How many gram of each metal will be deposited assuming only cathodic reaction in each cell respectively : [RBQ]

163235 During the electrolysis of brine \((\mathrm{NaCl})\) solution, what volume of chlorine gas, at STP is produced in the same time, in which \(\mathbf{5 . 0}\) litre of hydrogen gas is liberated under the same condition : [RBQ]

163236 Given that \(\mathrm{E}_{\mathrm{Fe}^{3+}+\mathrm{Fe}}^{\circ}=-0.036 \mathrm{~V}, \mathrm{E}_{\mathrm{Fe}^{2+} \mid \mathrm{Fe}}^{\circ}=-0.439 \mathrm{~V}\), the value of standard electrode potental for the change \(\mathrm{Fe}_{(\mathrm{aq})}^{3+}+\overline{\mathrm{e}} \rightarrow \mathrm{Fe}_{(\mathrm{aq})}^{2+}\) will be : [RBQ]

163237 Electrolysis of dilute aqueous \(\mathrm{NaCl}\) solution was carried out by passing 10 milliampere current. The time required to liberate \(224 \mathrm{ml}\) (S.T.P) of \(\mathrm{H}_2\) gas at the cathode is : [RBQ]