163229 Which of the following cases shows zero oxidation state of carbon : \(\mathrm{CCl}_4, \mathrm{CH}_2 \mathrm{Cl}_2, \mathrm{C}_6 \mathrm{H}_{12} \mathrm{O}_6\) and HNC : [RBQ]

163230 Calculate the electrode potential at a copper electrode dipped in a \(0.1 \mathrm{M}\) solution of copper sulphate at \(25^{\circ} \mathrm{C}\). The standard electrode potential of \(\mathrm{Cu}^{2+} / \mathrm{Cu}\) system is 0.34 volt at \(298 \mathrm{~K}\). [RBQ]

163231 The standard oxidation potential of zinc is \(\mathbf{0 . 7 6}\) volt and of silver is \(\mathbf{- 0 . 8 0}\) volt. Calculate the emf of the cell :
\( \mathrm{Zn}\left|\mathrm{Zn}\left(\mathrm{NO}_3\right)_2 \| \mathrm{AgNO}_3\right| \mathrm{Ag} \)
\(0.25 \mathrm{M} \quad 0.1 \mathrm{M}\)
at \(25^{\circ} \mathrm{C}\) : [RBQ]

163232 Calculate the emf of the following cell at \(25^{\circ} \mathrm{C}\) :
\( \underset{2 \text { atm }}{\mathrm{Pt}} \mathrm{H}_2|\mathrm{HCl}| \underset{10}{\mathrm{H}_2, \mathrm{Ptm}} \) [RBQ]

163229 Which of the following cases shows zero oxidation state of carbon : \(\mathrm{CCl}_4, \mathrm{CH}_2 \mathrm{Cl}_2, \mathrm{C}_6 \mathrm{H}_{12} \mathrm{O}_6\) and HNC : [RBQ]

163230 Calculate the electrode potential at a copper electrode dipped in a \(0.1 \mathrm{M}\) solution of copper sulphate at \(25^{\circ} \mathrm{C}\). The standard electrode potential of \(\mathrm{Cu}^{2+} / \mathrm{Cu}\) system is 0.34 volt at \(298 \mathrm{~K}\). [RBQ]

163231 The standard oxidation potential of zinc is \(\mathbf{0 . 7 6}\) volt and of silver is \(\mathbf{- 0 . 8 0}\) volt. Calculate the emf of the cell :
\( \mathrm{Zn}\left|\mathrm{Zn}\left(\mathrm{NO}_3\right)_2 \| \mathrm{AgNO}_3\right| \mathrm{Ag} \)
\(0.25 \mathrm{M} \quad 0.1 \mathrm{M}\)
at \(25^{\circ} \mathrm{C}\) : [RBQ]

163232 Calculate the emf of the following cell at \(25^{\circ} \mathrm{C}\) :
\( \underset{2 \text { atm }}{\mathrm{Pt}} \mathrm{H}_2|\mathrm{HCl}| \underset{10}{\mathrm{H}_2, \mathrm{Ptm}} \) [RBQ]

163229 Which of the following cases shows zero oxidation state of carbon : \(\mathrm{CCl}_4, \mathrm{CH}_2 \mathrm{Cl}_2, \mathrm{C}_6 \mathrm{H}_{12} \mathrm{O}_6\) and HNC : [RBQ]

163230 Calculate the electrode potential at a copper electrode dipped in a \(0.1 \mathrm{M}\) solution of copper sulphate at \(25^{\circ} \mathrm{C}\). The standard electrode potential of \(\mathrm{Cu}^{2+} / \mathrm{Cu}\) system is 0.34 volt at \(298 \mathrm{~K}\). [RBQ]

163231 The standard oxidation potential of zinc is \(\mathbf{0 . 7 6}\) volt and of silver is \(\mathbf{- 0 . 8 0}\) volt. Calculate the emf of the cell :
\( \mathrm{Zn}\left|\mathrm{Zn}\left(\mathrm{NO}_3\right)_2 \| \mathrm{AgNO}_3\right| \mathrm{Ag} \)
\(0.25 \mathrm{M} \quad 0.1 \mathrm{M}\)
at \(25^{\circ} \mathrm{C}\) : [RBQ]

163232 Calculate the emf of the following cell at \(25^{\circ} \mathrm{C}\) :
\( \underset{2 \text { atm }}{\mathrm{Pt}} \mathrm{H}_2|\mathrm{HCl}| \underset{10}{\mathrm{H}_2, \mathrm{Ptm}} \) [RBQ]

163229 Which of the following cases shows zero oxidation state of carbon : \(\mathrm{CCl}_4, \mathrm{CH}_2 \mathrm{Cl}_2, \mathrm{C}_6 \mathrm{H}_{12} \mathrm{O}_6\) and HNC : [RBQ]

163230 Calculate the electrode potential at a copper electrode dipped in a \(0.1 \mathrm{M}\) solution of copper sulphate at \(25^{\circ} \mathrm{C}\). The standard electrode potential of \(\mathrm{Cu}^{2+} / \mathrm{Cu}\) system is 0.34 volt at \(298 \mathrm{~K}\). [RBQ]

163231 The standard oxidation potential of zinc is \(\mathbf{0 . 7 6}\) volt and of silver is \(\mathbf{- 0 . 8 0}\) volt. Calculate the emf of the cell :
\( \mathrm{Zn}\left|\mathrm{Zn}\left(\mathrm{NO}_3\right)_2 \| \mathrm{AgNO}_3\right| \mathrm{Ag} \)
\(0.25 \mathrm{M} \quad 0.1 \mathrm{M}\)
at \(25^{\circ} \mathrm{C}\) : [RBQ]

163232 Calculate the emf of the following cell at \(25^{\circ} \mathrm{C}\) :
\( \underset{2 \text { atm }}{\mathrm{Pt}} \mathrm{H}_2|\mathrm{HCl}| \underset{10}{\mathrm{H}_2, \mathrm{Ptm}} \) [RBQ]