Depict the galvanic cell in which the reaction is:
\( Zn_{\left ( s \right )} \;+ \;2 \;Ag_{\left ( aq \right )}^{+} \;\rightarrow \;Zn^{2+}_{\left ( aq \right )} \;+ \;2 \;Ag_{\left ( s \right )} \)
Further show:
(i) which of the electrode is negatively charged?
(ii) the carriers of the current in the cell.
(iii) individual reaction at each electrode.
The galvanic cell corresponding to the given redox reaction can be shown as:
\( Zn|Zn^{2+}_{\left ( aq \right )}+||Ag^{+}_{\left ( aq \right )}|Ag \)
(i) Zn electrode is negatively charged because at this electrode, Zn oxidizes to \( Zn^{2+}\)and the leaving electrons accumulate on this electrode.
(ii) The carriers of current are ions in the cell.
(iii) Reaction at Zn electrode is shown as:
\( Zn_{\left ( s \right )} \;\rightarrow \;Zn^{2+}_{\left ( aq \right )} \;+ \;2 \;e^{-}\)
Reaction at Ag electrode is shown as:
\( Ag^{+}_{\left ( aq \right )} \;+ \;e^{-}\;\rightarrow \;Ag_{\left ( s \right )}\)
Answered by Pragya Singh | 1 year agoFluorine reacts with ice and results in the change:
\( H_{ 2 }O_{ (s) } \; + \; F_{ 2 \; (g) } \; \rightarrow \; HF_{ (g) } \; + \; HOF_{ (g) } \)
Justify that this reaction is a redox reaction
Given the standard electrode potentials,
\( \dfrac{ K^{+}}{K}\)= –2.93V
\( \dfrac{ Ag^{+}}{Ag}\) = 0.80V
\( \dfrac{Hg^{2+}}{Hg}\) = 0.79V
\(\dfrac{ Mg^{2+}}{Mg}\) = –2.37V
\(\dfrac{Cr^{3+}}{Cr}\) = –0.74V
Arrange these metals in their increasing order of reducing power.
Arrange the given metals in the order in which they displace each other from the solution of their salts.
Al, Fe, Cu, Zn, Mg
Predict the products of electrolysis in each of the following:
(i) An aqueous solution of \( AgNO_{3}\) with silver electrodes
(ii) An aqueous solution \( AgNO_{3}\) with platinum electrodes
(iii) A dilute solution of \( H_{2}SO_{4}\) with platinum electrodes
(iv) An aqueous solution of \( CuCl_{2}\)with platinum electrodes.
Using the standard electrode potentials given, predict if the reaction between the following is feasible:
(a) \( Fe^{ 3+ }_{ (aq) }+ and\; I^{ – }_{ (aq) }\)
(b) \( Ag^{ + }_{ (aq) }+ and\; Cu^{ }_{ (s) }\)
(c) \( Fe^{ 3+ }_{ (aq) }+and\; Cu^{ }_{ (s) }\)
(d) \( Ag^{ }_{ (s) } and \;Fe^{ 3+ }_{ (aq) }\)
(e) \( Br_{ 2 \; (aq) }and\; Fe^{ 2+ }_{ (aq) }\)