Questions in electrochemistry

SelectQuestion
An electrochemical cell is set up as follows $Pt({{H}_{2}},\,1\,atm)/0.1\,M\,HCl||0.1M\,\text{acetic acid/(}{{H}_{2}},\,1\,atm)Pt$ emf of this cell will not be zero because
At ${{25}^{o}}C$, the standard emf of a cell having reaction involving two electron change is found to be 0.295 V. The equilibrium constant of the reaction is
What is the potential of a half-cell consisting of zinc electrode in 0.01m $ZnS{{O}_{4}}$ solution at ${{258}^{o}}C({{E}^{0}}=0.763\,V)$
The cell reaction of a cell is, $M{{g}_{(s)}}+C{{u}^{2+}}(aq)\to C{{u}_{(s)}}+M{{g}^{2+}}(aq)$ If the standard reduction potentials of Mg and Cu are – 2.37 and + 0.34 V respectively. The emf of the cell is
The standard reduction potential for $F{{e}^{2+}}/Fe$ and $S{{n}^{2+}}/Sn$ electrodes are – 0.44 and – 0.14 volt respectively. For the given cell reaction $F{{e}^{2+}}+Sn\to Fe+S{{n}^{2+}}$, the standard emf is
For a cell reaction involving a two-electron change, the standard emf of the cell is found to be 0.295 V at ${{25}^{o}}C$. The equilibrium constant of the reaction at ${{25}^{o}}C$ will be
Calculate standard free energy change for the reaction $\frac{1}{2}Cu\,(s)+\frac{1}{2}C{{l}_{2}}(g)$ ? $\frac{1}{2}C{{u}^{2+}}+C{{l}^{-}}$ taking place at ${{25}^{o}}C$ in a cell whose standard emf is 1.02 volts
The emf of the cell in which the following reaction $Zn(s)+N{{i}^{2+}}(a=1.0)$? $Z{{n}^{2+}}(a=10)+Ni\,(s)$ occurs, is found to be 0.5105 V at 298K. The standard emf of the cell is
Aluminium displaces hydrogen from acids but copper does not. A galvanic cell prepared by combining $Cu/C{{u}^{2+}}$ and $Al/A{{l}^{3+}}$ has an emf of 2.0 V at 298 K. If the potential of copper electrode is + 0.34 V, that of aluminium is
What is the potential of a cell containing two hydrogen electrodes the negative one in contact with ${{10}^{-8}}M\,{{H}^{+}}$ and positive one in contact with $0.025 M\, {{H}^{+}}$

View Selected Questions (0)

Back to Categories

Back to Home