Saleha Pervez and Vandana Solutions for Chapter: Electrochemistry, Exercise 5: Chapter Practice

The incorrect statement about electrochemistry is:

$\mathrm{Zn}\left(\mathrm{s}\right)+{\mathrm{Cu}}^{2+}\left(\mathrm{aq}\right)\to {\mathrm{Zn}}^{2+}\left(\mathrm{aq}\right)+\mathrm{Cu}\left(\mathrm{s}\right)$. The above redox reaction is used in

For the generation of electrode potential of $1.1 \mathrm{V}$, the ideal concentration of zinc and copper ion (in $\mathrm{mol} {\mathrm{dm}}^{-3}$ ) in the galvanic cell is
 

Compound XA, XB, XC are added into separate test tubes containing A, B, C solutions. XB react with A and C. XA does not react with any of these. XC reacts with A. Which of the following is the correct decreasing order for the oxidation of the anions?

Select the strongest reducing agent from the given electrode potential.

Two electrolytic cells containing silver nitrate solution and dilute sulphuric acid were connected in a series. A steady current of $2.5 \mathrm{A}$ was passed through them till $1.078 \mathrm{g}$ of silver was deposited $(\mathrm{Ag} = 107.8 \mathrm{g}/\mathrm{mol})$. What is the weight of oxygen gas liberated during the reaction?
 

How many moles of $\mathrm{Hg}$ will be produced by electrolysing $1.0 \mathrm{M} \mathrm{Hg}({\mathrm{NO}}_3{)}_2$ solution with a current of $2.00 \mathrm{A}$ for $3$ hours?

$\left[\mathrm{Hg}\right({\mathrm{NO}}_3{)}_2= 200.6 \mathrm{g}/\mathrm{mol}]$

Iron may be protected from rusting by coating with zinc or tin. By referring to the data given below, explain why zinc protects iron more effectively than tin? ${\mathrm{Zn}}^{2+}+ 2{\mathrm{e}}^{-} \to \mathrm{Zn}, {\mathrm{E}}^{°} = -0.76 \mathrm{V}; {\mathrm{Fe}}^{2+}+2{\mathrm{e}}^{-}\to \mathrm{Fe}, \mathrm{E}°= - 0.44 \mathrm{V}; {\mathrm{Sn}}^{2+}+ 2{\mathrm{e}}^{-}\to \mathrm{Sn}, \mathrm{E}°=-0.14 \mathrm{V}$.