Consider the following standard electrode potentials ( E o in volts) in aqueous solution: E l e m e n t M 3 + / M M + / M A l - 1.66 + 0.55 T l + 1.26 - 0.34 Based on these data, which of the following statements is correct?

T l + is more stable than A l +

T l + is more stable than A l 3 +

A l + is more stable than A l 3 +

T l 3 + is more stable than A l 3 +

MEDIUM

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Consider the following standard electrode potentials ( $E °$ in volts) in aqueous solution:

Element $M^{3 +} / M$ $M^{+} / M$

$Αl$ $- 1.66$ $+ 0.55$

$Tl$ $+ 1.26$ $- 0.34$

Based on these data, which of the following statements is CORRECT?

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Important Questions on Electrochemistry

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Electrode Potential and Standard Electrode Potential

Consider the following standard electrode potentials (

E^{o}

in volts) in aqueous solution:

\begin{matrix} \underset{}{E l e m e n t} & \underset{}{M^{3 +} / M} & \underset{}{M^{+} / M} \\ A l & - 1.66 & + 0.55 \\ T l & + 1.26 & - 0.34 \end{matrix}

Based on these data, which of the following statements is correct?

HARD

Chemistry>Physical Chemistry>Electrochemistry>Electrode Potential and Standard Electrode Potential

The standard electrode potential $E^{o}$ and its temperature coefficient $(\frac{dE}{dT})$ for a cell are $2 V$ and $- 5 {\times10}^{- 4} V K^{- 1}$ at $300 K$ , respectively. The reaction is $Zn (s) + {Cu}^{2 +} (aq) \to {Zn}^{2 +} (aq) + Cu (s)$ . The standard reaction enthalpy $(Δ_{r} H^{-})$ at $300 K$ in $m o l^{- 1}$ is

$[$ Use $R = 8 J K^{- 1} {mol}^{- 1}$ and $F =96,500 C {mol}^{- 1}]$

HARD

Chemistry>Physical Chemistry>Electrochemistry>Electrode Potential and Standard Electrode Potential

In the cell,

Pt (s) |H_{2} (g, 1 bar)| HCl (aq) |AgCl (s)| Ag (s) |Pt (s),

the cell potential is

0 .92 V

when a

10^{- 6}

molar

HCl

solution is used. The standard electrode potential of

Ag | AgCl | {Cl}^{-}

electrode is:

(Given,

\frac{2 .303 RT}{F} = 0 .06 V

298 K

)

EASY

Chemistry>Physical Chemistry>Electrochemistry>Electrode Potential and Standard Electrode Potential

If the

E_{c e l l}^{o}

for a given reaction has a negative value, which of the following gives the correct relationship for the values of

∆ G^{o}

and

K_{e q}

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Electrode Potential and Standard Electrode Potential

Define standard emf of a cell.

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Chemistry>Physical Chemistry>Electrochemistry>Electrode Potential and Standard Electrode Potential

A variable, the opposite external potential

(E_{ext})

is applied to the cell

Z n | Z n^{2 +} (1 M) ∥ C u^{2 +} (1 M) | C u

, of potential

1.1 V

. When

E_{e x t} < 1.1 V

and

E_{e x t} > 1.1 V

, respectively electrons flow from

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Electrode Potential and Standard Electrode Potential

If the standard electrode potential for a cell is

2 V

300 K,

the equilibrium constant

(K)

for the reaction.

Zn (s) + {Cu}^{2 +} (aq) ⇌ {Zn}^{2 +} (aq) + Cu (s)

300 K

is approximately:

(R = 8 {JK}^{- 1} {mol}^{- 1}, F = 96000 C {mol}^{- 1})

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Electrode Potential and Standard Electrode Potential

The voltage of the cell consisting of

Li (s)

and

F_{2} (g)

electrodes is

5.92 V

at standard condition at

298 K

. What is the voltage if the electrolyte consists of

2 M LiF

.
Given that,

\ln 2 = 0 .693, R = 8 .314 {JK}^{- 1} {mol}^{- 1} F = 96500 C {mol}^{- 1}

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Electrode Potential and Standard Electrode Potential

The metals near the bottom of the electrochemical series are :

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Electrode Potential and Standard Electrode Potential

For the following electrochemical cell at

289 K,

Pt (s) | H_{2} (g, 1 bar) | H^{+} (aq, 1 M) | | M^{4 +} (aq .) {, M}^{2+} (aq .) | Pt (s)

E_{c e l l} = 0.092 V

when

\frac{[M^{2 +} (a q .)]}{[M^{4 +} (a q .)]} = 10^{x}

Given:

E_{M^{4 +} / M^{2 +}}^{0} = 0.151 V; 2.303 \frac{R T}{F} = 0.059

The value of

x

is -

EASY

Chemistry>Physical Chemistry>Electrochemistry>Electrode Potential and Standard Electrode Potential

Given the standard potentials

E^{o} (\frac{C u^{2 +}}{C u})

and

E^{o} (\frac{C u^{+}}{C u})

0.340 V

and

0.522 V

respectively, the value of

E^{o} (\frac{C u^{2 +}}{C u^{+}})

EASY

Chemistry>Physical Chemistry>Electrochemistry>Electrode Potential and Standard Electrode Potential

Standard hydrogen electrode (SHE) is a

EASY

Chemistry>Physical Chemistry>Electrochemistry>Electrode Potential and Standard Electrode Potential

The equilibrium constant of a

2

electron redox reaction at

298 K

3.8 \times 10^{- 3} .

The cell potential

E^{o} (in V)

and the free energy change

{ΔG}^{o} (in kJ {mol}^{-})

for this equilibrium respectively, are

HARD

Chemistry>Physical Chemistry>Electrochemistry>Electrode Potential and Standard Electrode Potential

For the electrochemical cell,

Mg(s) |{Mg}^{2+} (aq,1 M)| |{Cu}^{2+} (aq,1 M)| Cu (s)

the standard emf of the cell is

2 .70 V

300 K .

When the concentration of

{Mg}^{2+}

is changed to

x M,

the cell potential changes to

2 .67 V

300 K .

The value of

x

is ________.

(given,

\frac{F}{R} {=11500 K V}^{- 1},

where

F

is the Faraday constant and

R

is the gas constants,

ln (10) = 2 .30

)

EASY

Chemistry>Physical Chemistry>Electrochemistry>Electrode Potential and Standard Electrode Potential

Given

E_{{Cl}_{2} / {Cl}^{-}}^{o} = 1 .36 V, E_{{Cr}^{3 +} / Cr}^{o} = - 0 .74 V

E_{{Cr}_{2} O_{7}^{2 -} / {Cr}^{3 +}}^{o} = 1 .33 V, E_{{MnO}_{4}^{-} / {Mn}^{2 +}}^{o} = 1 .51 V .

Among the following, the strongest reducing agent is:

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Electrode Potential and Standard Electrode Potential

To find the standard potential of

M^{3 +} / M

electrode, the following cell is constituted:

Pt / M / M^{3 +} (0 .001 mol L^{- 1}) / {Ag}^{+} (0 .01 mol L^{- 1}) / Ag

The emf of the cell is found to be

0.421 volt

298 K

. The standard potential of half-reaction

M^{3 +} + 3 e^{-} \to M

298 K

will be:

(Given:

E_{\frac{{Ag}^{+}}{Ag}}^{⊝}

298 K = 0.80 volt

)

EASY

Chemistry>Physical Chemistry>Electrochemistry>Electrode Potential and Standard Electrode Potential

What is the standard reduction potential

(E^{o})

for

{Fe}^{3 +} \to Fe ?

Given that:

{Fe}^{2 +} + 2 e^{-} \to Fe; E_{{Fe}^{2 +} / Fe}^{o} = - 0 .47 V

{Fe}^{3 +} + e^{-} \to {Fe}^{2 +}; E_{{Fe}^{3 +} / {Fe}^{2 +}}^{o} = + 0 .77 V

HARD

Chemistry>Physical Chemistry>Electrochemistry>Electrode Potential and Standard Electrode Potential

The pressure of

H_{2}

required to make the potential of hydrogen electrode zero in pure water at 298 K is:

EASY

Chemistry>Physical Chemistry>Electrochemistry>Electrode Potential and Standard Electrode Potential

The standard emf of the cell

Zn ∣ {Zn}^{2 +} ‖ {Ag}^{+} | Ag

1.56 V .

If the standard reduction potential of

Ag

0.8 V,

the standard oxidation potential of

Zn

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Electrode Potential and Standard Electrode Potential

Four successive members of the first row of transition elements are listed below with atomic numbers. Which one of them is expected to have the highest

E_{M^{3 +} / M^{2 +}}^{o}

value?

Element	$M^{3 +} / M$	$M^{+} / M$
$Αl$	$- 1.66$	$+ 0.55$
$Tl$	$+ 1.26$	$- 0.34$

Consider the following standard electrode potentials (E° in volts) in aqueous solution: Element M3+/M M+/M Αl -1.66 +0.55 Tl +1.26 -0.34 Based on these data, which of the following statements is CORRECT?

Important Questions on Electrochemistry

Learn and Prepare for any exam you want !

Consider the following standard electrode potentials ( $E °$ in volts) in aqueous solution:

Element $M^{3 +} / M$ $M^{+} / M$

$Αl$ $- 1.66$ $+ 0.55$

$Tl$ $+ 1.26$ $- 0.34$

Based on these data, which of the following statements is CORRECT?