Questions in electrochemistry

SelectQuestion
Assertion (A): Copper reacts with hydrochloric acid and liberates hydrogen from the solution of dilute hydrochloric acid Reason (R): Hydrogen is below copper in the electrochemical series
For the cell reaction $2Hg(l)+2A{{g}^{+}}(aq)\to 2Ag(s)+Hg_{2}^{2+}(aq)$ It is the given that $E_{A{{g}^{+}}/Ag}^{0}=0.800V,\,[A{{g}^{+}}]={{10}^{-3}}M$ $E_{Hg_{2}^{2+}/Hg}^{0}=0.785V$ and $[Hg_{2}^{2+}]={{10}^{-1}}M$
The standard electrode potentials of $Z{{n}^{2+}}/Zn$ and $A{{g}^{+}}/Ag$ are $– 0.763 V$ and $+ 0.799 V$ respectively. The standard potential of the cell is
What is the standard cell potential for the cell $Zn/Z{{n}^{2+}}(1M)||C{{u}^{2+}}(1M)/Cu$ ${{E}^{0}}$ for $Zn/Z{{n}^{2+}}(1M)=-0.76\,V$ and $C{{u}^{2+}}/Cu=+0.34\,V$
Normal aluminium electrode coupled with normal hydrogen electrode gives an emf of 1.66 volts. So the standard electrode potential of aluminium is
The standard reduction potential ${{E}^{0}}$ for the half reactions are as $Zn=Z{{n}^{2+}}+2{{e}^{-}};\,{{E}^{0}}=+0.76\,V$; $Fe=F{{e}^{2+}}+2{{e}^{-}};\,{{E}^{0}}=+0.41\,V$; The emf for cell reaction $F{{e}^{2+}}+Zn\to Z{{n}^{2+}}+Fe$ is
If a cell reaction is spontaneous, then
The standard electrode potential for the two electrode ${{A}^{+}}/A$ and ${{B}^{+}}/B$ are respectively 0.5 V and 0.75 V. The emf of the given cell $A|{{A}^{+}}(a=1)||{{B}^{+}}(a=1)|B$ will be
Standard reduction electrode potentials of three metals $A$, $B$ and $C$ are respectively $+ 0.5 V$, $– 3.0 V$ and $– 1.2 V$. the reducing powers of these metals are
Reduction potential of four elements P, Q, R, S is – 2.90, + 0.34, + 1.20 and – 0.76. Reactivity decreases in the order

View Selected Questions (0)

Back to Categories

Back to Home