Calculate $E^o_{cell}$ for the following cell in $V$:
$Zn_{(s)} | Zn^{2+}_{(aq.)} || Ag^{+}_{(aq.)} | Ag_{(s)}$
Given: $E^o_{Zn^{2+}/Zn} = -0.76 \ V$ ; $E^o_{Ag^{+}/Ag} = 0.80 \ V$

Which of the following metals does not liberate hydrogen from dilute hydrochloric acid?

Given $E^{0}_{Fe^{2+}|Fe} = -0.441 \, V$ and $E^{0}_{Fe^{3+}|Fe^{2+}} = 0.771 \, V$,calculate the standard $EMF$ for the reaction $Fe + 2Fe^{3+} \rightarrow 3Fe^{2+}$ in $V$.

Given:
$E^o_{Cr^{3+}/Cr} = -0.74 \ V$,$E^o_{MnO_4^-/Mn^{2+}} = 1.51 \ V$
$E^o_{Cr_2O_7^{2-}/Cr^{3+}} = 1.33 \ V$,$E^o_{Cl_2/Cl^{-}} = 1.36 \ V$
Based on the data given above,the strongest oxidising agent will be:

In a cell reaction
$Cu_{(s)} + 2Ag^{+}_{(aq)} \to Cu^{2+}_{(aq)} + 2Ag_{(s)}$
$E_{cell}^o = + 0.46 \ V$.
If the concentration of $Cu^{2+}$ ions is doubled,then $E_{cell}^o$ will be

What is standard electrode potential?