The reaction occurs in which of the given galvanic cell? 1 2 H 2 ( g ) + AgCl ( s ) ⇌ H + ( aq ) + Cl - ( aq ) + Ag ( s )

Pt | H 2 ( g ) | HCl ( sol n ) | AgCl ( s ) | Ag

Ag | AgCl ( s ) | KCl ( sol n ) | AgNO 3 | Ag

Pt | H 2 ( g ) | HCl ( sol n ) | AgNO 3 ( sol n ) | Ag

Pt | H 2 ( g ) | KCl ( sol n ) | AgCl ( s ) | Ag

EASY

Earn 100

Two half cells have reduction potentials $- 0.76 V$ and $- 0.13 V$ respectively. A galvanic cell is made from these two half cells. Which of the following statement is correct?

50% studentsanswered this correctly

Important Questions on Electrochemistry

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Electrochemical Cells

In a galvanic cell, the salt bridge

HARD

Chemistry>Physical Chemistry>Electrochemistry>Electrochemical Cells

The products of hydrogen fuel cell are

EASY

Chemistry>Physical Chemistry>Electrochemistry>Electrochemical Cells

What is salt bridge? Give its two functions.

HARD

Chemistry>Physical Chemistry>Electrochemistry>Electrochemical Cells

For the cell $Zn (s) |{ZnSO}_{4} (aq)| |{CuSO}_{4} (aq)| Cu (s)$ , when the concentration of ${Zn}^{2 +}$ is $10$ times the concentration of ${Cu}^{2 +}$ , the expression for $ΔG (in J {mol}^{- 1})$ is

$[F =$ Faraday's constant, $R =$ universal gas constant, $T =$ temperature, $E^{o} cell = 1.1 V]$

EASY

Chemistry>Physical Chemistry>Electrochemistry>Electrochemical Cells

A galvanic cell transforms the energy released by a spontaneous redox reaction into electrical energy that can be used to perform work. In a galvanic cell, electrons flow from

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Electrochemical Cells

What is salt bridge? Mention its functions.

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Electrochemical Cells

What is a salt bridge? Give two functions of salt bridge?

EASY

Chemistry>Physical Chemistry>Electrochemistry>Electrochemical Cells

Which is symbolic representation for following cell reaction,

{Mg}_{(s)} + {Cl}_{2} (g) \to {Mg}_{(aq)}^{2 +} + 2 {Cl}_{(aq)}^{-}

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Electrochemical Cells

The following reaction takes place at $298 K$ in an electrochemical cell involving two metals $A$ and $B$ ,

$A^{2 +} (aq) + B (s) \to B^{2 +} (aq) + A (s)$

with $[A^{2 +}] = 4 \times 10^{- 3} M$ and $[B^{2 +}] = 2 \times 10^{- 3} M$ in the respective half-cells, the cell EMF is $1.091 V$ . The equilibrium constant of the reaction is closest to;

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Electrochemical Cells

An electrochemical cell can behave like an electrolytic cell when ______.

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Electrochemical Cells

Write the cell reaction for the following cells.
(a)

Fe | {Fe}^{2 +} | | H_{2} {SO}_{4} | H_{2} (Pt)

(b)

(Pt) H_{2} | HCl | {Cl}_{2} (Pt)

EASY

Chemistry>Physical Chemistry>Electrochemistry>Electrochemical Cells

E_{{Cu}^{2 +} | Cu}^{0} = + 0 .34 V

E_{{Zn}^{2 +} | Zn}^{0} = - 0 .76 V

Identify the incorrect statement from the options below for the above cell:

HARD

Chemistry>Physical Chemistry>Electrochemistry>Electrochemical Cells

What are Galvanic cells? Explain the working of Galvanic cells with one example.

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Electrochemical Cells

Represent a cell consisting of ${Mg}^{2 +}$ | $Mg$ half cell and ${Ag}^{+}$ | $Ag$ half cell and write the cell reaction.

$(E °_{Ag} = 0.799 V, E °_{Mg} = - 2.37 V)$

EASY

Chemistry>Physical Chemistry>Electrochemistry>Electrochemical Cells

The device which convert the energy of combustion of fuels directly into electrical energy is called

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Electrochemical Cells

E_{cell}

of the following cell is

Pt (s) ∣ H_{2} (g),

bar

|H^{+} (1 M) ‖ H^{+} (0.1 M)| H_{2} (g), 1 bar ∣ Pt (s)

HARD

Chemistry>Physical Chemistry>Electrochemistry>Electrochemical Cells

The reaction occurs in which of the given galvanic cell?

$\frac{1}{2} H_{2} (g) + AgCl (s) ⇌ H^{+} (aq) + {Cl}^{-} (aq) + Ag (s)$

HARD

Chemistry>Physical Chemistry>Electrochemistry>Electrochemical Cells

An important fuel cell involves the reaction of hydrogen with oxygen to form water. The option describing reactions occurring at anode and cathode in this fuel cell is

EASY

Chemistry>Physical Chemistry>Electrochemistry>Electrochemical Cells

At $298 K$ , the $e . m . f .$ of the galvanic cell mentioned below is $(E^{0} = 1.1 V)$

$Zn (s) |{Zn}^{2 +} (10^{- 3} M) ‖ {Cu}^{2 +} (0.1 M)| Cu (s)$

EASY

Chemistry>Physical Chemistry>Electrochemistry>Electrochemical Cells

The standard Gibbs energy for the given cell reaction in

k J m o l^{- 1}

298 K

is:

Z n (s) + C u^{2 +} (a q) ⟶ Z n^{2 +} (a q) + C u (s)

E^{0} = 2 V a t 298 K

(F a r a d a y' s c o n s t a n t, F = 96000 C m o l^{- 1})

Two half cells have reduction potentials –0.76 V and – 0.13 V respectively. A galvanic cell is made from these two half cells. Which of the following statement is correct?

Important Questions on Electrochemistry

Learn and Prepare for any exam you want !

Two half cells have reduction potentials $- 0.76 V$ and $- 0.13 V$ respectively. A galvanic cell is made from these two half cells. Which of the following statement is correct?