6 RBTS PAPER(CHEMISTRY)
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6 RBTS PAPER

163243 Find the product of electrolysis at anode and at cathode evolve due to electrolysis of aquous \(\mathrm{NaCl}\) respectively: [RBQ]

1 \(\mathrm{H}_2\) gas at cathode, \(\mathrm{O}_2\) gas at anode
2 \(\mathrm{H}_2\) gas at cathode, \(\mathrm{Cl}_2\) gas at anode
3 \(\mathrm{H}_2\) gas at anode, \(\mathrm{Cl}_2\) gas at cathode
4 \(\mathrm{H}_2\) gas at anode, \(\mathrm{O}_2\) gas at cathode
CBSE 2008
6 RBTS PAPER

163260 Which of the following aqueous solution produces metal after electrolysis : [RBQ]

1 \(\mathrm{CuCl}_2\)
2 \(\mathrm{KMnO}_4\)
3 \(\mathrm{ZnCl}_2\)
4 \(\mathrm{CH}_3 \mathrm{COONa}\)
NCERT-XII-34
6 RBTS PAPER

163244 Using the data given below find out in which option the order of reducing power is correct :
\( \begin{gathered}
\mathrm{E}^{\circ} \mathrm{Cr}_2 \mathrm{O}_7^{-2} / \mathrm{Cr}^{3+}=1.33 \mathrm{~V}, \mathrm{E}^{\circ} \mathrm{Cl}_2 / \mathrm{Cl}^{-}=1.36 \mathrm{~V}, \\
\mathrm{E}^{\circ} \mathrm{MnO}_4^{-} / \mathrm{Mn}^{2+}=1.51 \mathrm{~V}, \mathrm{E}^{\circ} \mathrm{Cr}^{3+} / \mathrm{Cr}=-0.74 \mathrm{~V}
\end{gathered} \) [RBQ]

1 \(\mathrm{Cr}^{3+}<\mathrm{Cl}^{-}<\mathrm{Mn}^{2+}<\mathrm{Cr}\)
2 \(\mathrm{Mn}^{2+}<\mathrm{Cl}^{-}<\mathrm{Cr}^{3+}<\mathrm{Cr}\)
3 \(\mathrm{Cr}^{3+}<\mathrm{Cl}^{-}<\mathrm{Cr}_2 \mathrm{O}_7^{2-}<\mathrm{MnO}_4^{-}\)
4 \(\mathrm{Mn}^{2+}<\mathrm{Cr}^{3+}<\mathrm{Cl}^{-}<\mathrm{Cr}\)
CBSE 2005
6 RBTS PAPER

163245 For the given cell \(\mathbf{M g}\left|\mathbf{M g}^{2+}\right|\left|\mathrm{Cu}^{2+}\right| \mathrm{Cu}\) [RBQ]

1 \(\mathrm{Cu}\) is the oxidising agent
2 Cu is cathode
3 The cell reaction is \(\mathrm{Mg}+\mathrm{Cu}^{2+} \rightarrow \mathrm{Mg}^{2+}+\mathrm{Cu}\)
4 Both 2 and 3 option are correct
CBSE 2011
6 RBTS PAPER

163246 A 5A current is passed through a solution of zinc sulphate for \(\mathbf{4 0} \mathrm{min}\). The amount of zinc deposited at the cathode is : [RBQ]

1 \(40.65 \mathrm{~g}\)
2 \(0.4065 \mathrm{~g}\)
3 \(4.065 \mathrm{~g}\)
4 \(65.04 \mathrm{~g}\)
NCERT-XII-52
NEET DIGITAL LIBRARY
6 RBTS PAPER

163243 Find the product of electrolysis at anode and at cathode evolve due to electrolysis of aquous \(\mathrm{NaCl}\) respectively: [RBQ]

1 \(\mathrm{H}_2\) gas at cathode, \(\mathrm{O}_2\) gas at anode
2 \(\mathrm{H}_2\) gas at cathode, \(\mathrm{Cl}_2\) gas at anode
3 \(\mathrm{H}_2\) gas at anode, \(\mathrm{Cl}_2\) gas at cathode
4 \(\mathrm{H}_2\) gas at anode, \(\mathrm{O}_2\) gas at cathode
CBSE 2008
6 RBTS PAPER

163260 Which of the following aqueous solution produces metal after electrolysis : [RBQ]

1 \(\mathrm{CuCl}_2\)
2 \(\mathrm{KMnO}_4\)
3 \(\mathrm{ZnCl}_2\)
4 \(\mathrm{CH}_3 \mathrm{COONa}\)
NCERT-XII-34
6 RBTS PAPER

163244 Using the data given below find out in which option the order of reducing power is correct :
\( \begin{gathered}
\mathrm{E}^{\circ} \mathrm{Cr}_2 \mathrm{O}_7^{-2} / \mathrm{Cr}^{3+}=1.33 \mathrm{~V}, \mathrm{E}^{\circ} \mathrm{Cl}_2 / \mathrm{Cl}^{-}=1.36 \mathrm{~V}, \\
\mathrm{E}^{\circ} \mathrm{MnO}_4^{-} / \mathrm{Mn}^{2+}=1.51 \mathrm{~V}, \mathrm{E}^{\circ} \mathrm{Cr}^{3+} / \mathrm{Cr}=-0.74 \mathrm{~V}
\end{gathered} \) [RBQ]

1 \(\mathrm{Cr}^{3+}<\mathrm{Cl}^{-}<\mathrm{Mn}^{2+}<\mathrm{Cr}\)
2 \(\mathrm{Mn}^{2+}<\mathrm{Cl}^{-}<\mathrm{Cr}^{3+}<\mathrm{Cr}\)
3 \(\mathrm{Cr}^{3+}<\mathrm{Cl}^{-}<\mathrm{Cr}_2 \mathrm{O}_7^{2-}<\mathrm{MnO}_4^{-}\)
4 \(\mathrm{Mn}^{2+}<\mathrm{Cr}^{3+}<\mathrm{Cl}^{-}<\mathrm{Cr}\)
CBSE 2005
6 RBTS PAPER

163245 For the given cell \(\mathbf{M g}\left|\mathbf{M g}^{2+}\right|\left|\mathrm{Cu}^{2+}\right| \mathrm{Cu}\) [RBQ]

1 \(\mathrm{Cu}\) is the oxidising agent
2 Cu is cathode
3 The cell reaction is \(\mathrm{Mg}+\mathrm{Cu}^{2+} \rightarrow \mathrm{Mg}^{2+}+\mathrm{Cu}\)
4 Both 2 and 3 option are correct
CBSE 2011
6 RBTS PAPER

163246 A 5A current is passed through a solution of zinc sulphate for \(\mathbf{4 0} \mathrm{min}\). The amount of zinc deposited at the cathode is : [RBQ]

1 \(40.65 \mathrm{~g}\)
2 \(0.4065 \mathrm{~g}\)
3 \(4.065 \mathrm{~g}\)
4 \(65.04 \mathrm{~g}\)
NCERT-XII-52
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6 RBTS PAPER

163243 Find the product of electrolysis at anode and at cathode evolve due to electrolysis of aquous \(\mathrm{NaCl}\) respectively: [RBQ]

1 \(\mathrm{H}_2\) gas at cathode, \(\mathrm{O}_2\) gas at anode
2 \(\mathrm{H}_2\) gas at cathode, \(\mathrm{Cl}_2\) gas at anode
3 \(\mathrm{H}_2\) gas at anode, \(\mathrm{Cl}_2\) gas at cathode
4 \(\mathrm{H}_2\) gas at anode, \(\mathrm{O}_2\) gas at cathode
CBSE 2008
6 RBTS PAPER

163260 Which of the following aqueous solution produces metal after electrolysis : [RBQ]

1 \(\mathrm{CuCl}_2\)
2 \(\mathrm{KMnO}_4\)
3 \(\mathrm{ZnCl}_2\)
4 \(\mathrm{CH}_3 \mathrm{COONa}\)
NCERT-XII-34
6 RBTS PAPER

163244 Using the data given below find out in which option the order of reducing power is correct :
\( \begin{gathered}
\mathrm{E}^{\circ} \mathrm{Cr}_2 \mathrm{O}_7^{-2} / \mathrm{Cr}^{3+}=1.33 \mathrm{~V}, \mathrm{E}^{\circ} \mathrm{Cl}_2 / \mathrm{Cl}^{-}=1.36 \mathrm{~V}, \\
\mathrm{E}^{\circ} \mathrm{MnO}_4^{-} / \mathrm{Mn}^{2+}=1.51 \mathrm{~V}, \mathrm{E}^{\circ} \mathrm{Cr}^{3+} / \mathrm{Cr}=-0.74 \mathrm{~V}
\end{gathered} \) [RBQ]

1 \(\mathrm{Cr}^{3+}<\mathrm{Cl}^{-}<\mathrm{Mn}^{2+}<\mathrm{Cr}\)
2 \(\mathrm{Mn}^{2+}<\mathrm{Cl}^{-}<\mathrm{Cr}^{3+}<\mathrm{Cr}\)
3 \(\mathrm{Cr}^{3+}<\mathrm{Cl}^{-}<\mathrm{Cr}_2 \mathrm{O}_7^{2-}<\mathrm{MnO}_4^{-}\)
4 \(\mathrm{Mn}^{2+}<\mathrm{Cr}^{3+}<\mathrm{Cl}^{-}<\mathrm{Cr}\)
CBSE 2005
6 RBTS PAPER

163245 For the given cell \(\mathbf{M g}\left|\mathbf{M g}^{2+}\right|\left|\mathrm{Cu}^{2+}\right| \mathrm{Cu}\) [RBQ]

1 \(\mathrm{Cu}\) is the oxidising agent
2 Cu is cathode
3 The cell reaction is \(\mathrm{Mg}+\mathrm{Cu}^{2+} \rightarrow \mathrm{Mg}^{2+}+\mathrm{Cu}\)
4 Both 2 and 3 option are correct
CBSE 2011
6 RBTS PAPER

163246 A 5A current is passed through a solution of zinc sulphate for \(\mathbf{4 0} \mathrm{min}\). The amount of zinc deposited at the cathode is : [RBQ]

1 \(40.65 \mathrm{~g}\)
2 \(0.4065 \mathrm{~g}\)
3 \(4.065 \mathrm{~g}\)
4 \(65.04 \mathrm{~g}\)
NCERT-XII-52
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6 RBTS PAPER

163243 Find the product of electrolysis at anode and at cathode evolve due to electrolysis of aquous \(\mathrm{NaCl}\) respectively: [RBQ]

1 \(\mathrm{H}_2\) gas at cathode, \(\mathrm{O}_2\) gas at anode
2 \(\mathrm{H}_2\) gas at cathode, \(\mathrm{Cl}_2\) gas at anode
3 \(\mathrm{H}_2\) gas at anode, \(\mathrm{Cl}_2\) gas at cathode
4 \(\mathrm{H}_2\) gas at anode, \(\mathrm{O}_2\) gas at cathode
CBSE 2008
6 RBTS PAPER

163260 Which of the following aqueous solution produces metal after electrolysis : [RBQ]

1 \(\mathrm{CuCl}_2\)
2 \(\mathrm{KMnO}_4\)
3 \(\mathrm{ZnCl}_2\)
4 \(\mathrm{CH}_3 \mathrm{COONa}\)
NCERT-XII-34
6 RBTS PAPER

163244 Using the data given below find out in which option the order of reducing power is correct :
\( \begin{gathered}
\mathrm{E}^{\circ} \mathrm{Cr}_2 \mathrm{O}_7^{-2} / \mathrm{Cr}^{3+}=1.33 \mathrm{~V}, \mathrm{E}^{\circ} \mathrm{Cl}_2 / \mathrm{Cl}^{-}=1.36 \mathrm{~V}, \\
\mathrm{E}^{\circ} \mathrm{MnO}_4^{-} / \mathrm{Mn}^{2+}=1.51 \mathrm{~V}, \mathrm{E}^{\circ} \mathrm{Cr}^{3+} / \mathrm{Cr}=-0.74 \mathrm{~V}
\end{gathered} \) [RBQ]

1 \(\mathrm{Cr}^{3+}<\mathrm{Cl}^{-}<\mathrm{Mn}^{2+}<\mathrm{Cr}\)
2 \(\mathrm{Mn}^{2+}<\mathrm{Cl}^{-}<\mathrm{Cr}^{3+}<\mathrm{Cr}\)
3 \(\mathrm{Cr}^{3+}<\mathrm{Cl}^{-}<\mathrm{Cr}_2 \mathrm{O}_7^{2-}<\mathrm{MnO}_4^{-}\)
4 \(\mathrm{Mn}^{2+}<\mathrm{Cr}^{3+}<\mathrm{Cl}^{-}<\mathrm{Cr}\)
CBSE 2005
6 RBTS PAPER

163245 For the given cell \(\mathbf{M g}\left|\mathbf{M g}^{2+}\right|\left|\mathrm{Cu}^{2+}\right| \mathrm{Cu}\) [RBQ]

1 \(\mathrm{Cu}\) is the oxidising agent
2 Cu is cathode
3 The cell reaction is \(\mathrm{Mg}+\mathrm{Cu}^{2+} \rightarrow \mathrm{Mg}^{2+}+\mathrm{Cu}\)
4 Both 2 and 3 option are correct
CBSE 2011
6 RBTS PAPER

163246 A 5A current is passed through a solution of zinc sulphate for \(\mathbf{4 0} \mathrm{min}\). The amount of zinc deposited at the cathode is : [RBQ]

1 \(40.65 \mathrm{~g}\)
2 \(0.4065 \mathrm{~g}\)
3 \(4.065 \mathrm{~g}\)
4 \(65.04 \mathrm{~g}\)
NCERT-XII-52
NEET DIGITAL LIBRARY
6 RBTS PAPER

163243 Find the product of electrolysis at anode and at cathode evolve due to electrolysis of aquous \(\mathrm{NaCl}\) respectively: [RBQ]

1 \(\mathrm{H}_2\) gas at cathode, \(\mathrm{O}_2\) gas at anode
2 \(\mathrm{H}_2\) gas at cathode, \(\mathrm{Cl}_2\) gas at anode
3 \(\mathrm{H}_2\) gas at anode, \(\mathrm{Cl}_2\) gas at cathode
4 \(\mathrm{H}_2\) gas at anode, \(\mathrm{O}_2\) gas at cathode
CBSE 2008
6 RBTS PAPER

163260 Which of the following aqueous solution produces metal after electrolysis : [RBQ]

1 \(\mathrm{CuCl}_2\)
2 \(\mathrm{KMnO}_4\)
3 \(\mathrm{ZnCl}_2\)
4 \(\mathrm{CH}_3 \mathrm{COONa}\)
NCERT-XII-34
6 RBTS PAPER

163244 Using the data given below find out in which option the order of reducing power is correct :
\( \begin{gathered}
\mathrm{E}^{\circ} \mathrm{Cr}_2 \mathrm{O}_7^{-2} / \mathrm{Cr}^{3+}=1.33 \mathrm{~V}, \mathrm{E}^{\circ} \mathrm{Cl}_2 / \mathrm{Cl}^{-}=1.36 \mathrm{~V}, \\
\mathrm{E}^{\circ} \mathrm{MnO}_4^{-} / \mathrm{Mn}^{2+}=1.51 \mathrm{~V}, \mathrm{E}^{\circ} \mathrm{Cr}^{3+} / \mathrm{Cr}=-0.74 \mathrm{~V}
\end{gathered} \) [RBQ]

1 \(\mathrm{Cr}^{3+}<\mathrm{Cl}^{-}<\mathrm{Mn}^{2+}<\mathrm{Cr}\)
2 \(\mathrm{Mn}^{2+}<\mathrm{Cl}^{-}<\mathrm{Cr}^{3+}<\mathrm{Cr}\)
3 \(\mathrm{Cr}^{3+}<\mathrm{Cl}^{-}<\mathrm{Cr}_2 \mathrm{O}_7^{2-}<\mathrm{MnO}_4^{-}\)
4 \(\mathrm{Mn}^{2+}<\mathrm{Cr}^{3+}<\mathrm{Cl}^{-}<\mathrm{Cr}\)
CBSE 2005
6 RBTS PAPER

163245 For the given cell \(\mathbf{M g}\left|\mathbf{M g}^{2+}\right|\left|\mathrm{Cu}^{2+}\right| \mathrm{Cu}\) [RBQ]

1 \(\mathrm{Cu}\) is the oxidising agent
2 Cu is cathode
3 The cell reaction is \(\mathrm{Mg}+\mathrm{Cu}^{2+} \rightarrow \mathrm{Mg}^{2+}+\mathrm{Cu}\)
4 Both 2 and 3 option are correct
CBSE 2011
6 RBTS PAPER

163246 A 5A current is passed through a solution of zinc sulphate for \(\mathbf{4 0} \mathrm{min}\). The amount of zinc deposited at the cathode is : [RBQ]

1 \(40.65 \mathrm{~g}\)
2 \(0.4065 \mathrm{~g}\)
3 \(4.065 \mathrm{~g}\)
4 \(65.04 \mathrm{~g}\)
NCERT-XII-52