What is the standard electrode (half-cell) potential? Give its uses.
(N/A) Standard electrode (half-cell) potential: Under standard conditions,which include a temperature of $298 \ K$,a gas pressure of $1 \ bar$,and a solution concentration of $1 \ M$,the reduction potential of an electrode (half-cell) is defined as the standard electrode potential,measured in volts $(V)$.
Uses:
$(i)$ Construction of the electrochemical series ($EMF$ series): When half-cell reactions are arranged in decreasing order of their standard reduction potential,the resulting series is known as the electrochemical series. This series helps in predicting the spontaneity of redox reactions and the relative strength of oxidizing and reducing agents.
Uses:
$(i)$ Construction of the electrochemical series ($EMF$ series): When half-cell reactions are arranged in decreasing order of their standard reduction potential,the resulting series is known as the electrochemical series. This series helps in predicting the spontaneity of redox reactions and the relative strength of oxidizing and reducing agents.
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Give the cell potential formula for the Daniell cell and the Copper-Silver cell.
Easy
View SolutionGiven:
$Fe^{3+}_{(aq)} + e^- \to Fe^{2+}_{(aq)}; E^o = +0.77 \ V$
$Al^{3+}_{(aq)} + 3e^- \to Al_{(s)}; E^o = -1.66 \ V$
$Br_{2(aq)} + 2e^- \to 2Br^-_{(aq)}; E^o = +1.09 \ V$
Considering the electrode potentials,which of the following represents the correct order of reducing power?
$Fe^{3+}_{(aq)} + e^- \to Fe^{2+}_{(aq)}; E^o = +0.77 \ V$
$Al^{3+}_{(aq)} + 3e^- \to Al_{(s)}; E^o = -1.66 \ V$
$Br_{2(aq)} + 2e^- \to 2Br^-_{(aq)}; E^o = +1.09 \ V$
Considering the electrode potentials,which of the following represents the correct order of reducing power?
DifficultJEE MAIN 2014
View SolutionIf the standard reduction potentials of four electrodes $A$, $B$, $C$, and $D$ are $+2.5 \text{ V}$, $+3.0 \text{ V}$, $-2.0 \text{ V}$, and $-1.5 \text{ V}$ respectively, in which of the following cases is the standard $emf$ of the cell maximum?
DifficultMHT CET 2026
View SolutionGiven:
$E^o_{Fe^{3+} /Fe} = -0.036 \ V, E^o_{Fe^{2+} /Fe} = -0.439 \ V$
The value of standard electrode potential for the change,
$Fe^{3+}_{(aq)} + e^- \rightarrow Fe^{2+}_{(aq)}$ will be ........ $V$.
$E^o_{Fe^{3+} /Fe} = -0.036 \ V, E^o_{Fe^{2+} /Fe} = -0.439 \ V$
The value of standard electrode potential for the change,
$Fe^{3+}_{(aq)} + e^- \rightarrow Fe^{2+}_{(aq)}$ will be ........ $V$.
What is the observation we get when a gold ring is placed in the solution of $AgNO_3$? $[E_{Ag^{+}|Ag}^o = 0.80 \ V$ and $E_{Au^{3+}|Au}^o = 1.40 \ V]$
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