Electrochemistry Test

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Electrochemistry Test - 66

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Weekly Quiz Competition

Question 1
1 / -0

A Voltaic cell consists of an electrode of solid silver immersed in 0.10M $${ AgNO }_{ 3 }$$ Solution and an electrode of unknown metal X immersed in a 0.10M solution $${ X(NO }_{ 3 })_{ 2 }$$. A porous barrier separates the two half of the cell. Also given:

$$E\left( { Ag^{ + } }/{ Ag } \right)$$ = 0.80V and $${ E }_{ cell }$$ = 1.05V and at 25 degree Celsius

$${ X_{ (s) } }/{ { X }^{ 2+ } }(1.0M)\parallel { Ag }^{ + }(0.1M)/{ Ag }_{ (s) }$$

Which of the following statements regarding the cell and X is correct?

A
Standard Emf (E) of $${ { X }^{ 2+ } }/{ X }$$ is -0.25V at 25 degree Celsius

B
X is a stronger reducing agent than $${ H }_{ 2{ (g) } }$$

C
As cell operate, concentrations of both $${ X }^{ 2+ }and{ Ag }^{ + }$$ increases in their respective half cells

D
As cell operate, concentration of $${ X }^{ 2+ }$$ increases in anode chamber while concentration of $${ Ag }^{ + }$$ decreases in cathode chamber

Solution
Question 2
1 / -0

For a cell reaction represented by the equation $$Cu(s)+2Ag^{+}(aq)\rightarrow Cu^{2+}(aq)+2Ag(s)$$ the value of $$\Delta G^{\circ}$$ could be obtained by

A
setting up $$Cu(s)/Cu^{2+}(aq)$$ and $$Ag(s)/Ag^{+}(aq)$$ half - cells (using molar solution and measuring the emf of the resulting cell)

B
adding powered copper to a solution of $$Ag^{+}$$ ions and determining the enthalpy cgange, repeating this experiment at different temperatures

C
Setting up $$Cu(s)/Cu^{2+}(aq)$$ and $$Ag(s)/Ag^{+}(aq)$$ half-cells and determining the molarities of the ions which gives an emf of zero for the cell

D
Setting up $$Cu(s)/Cu^{2+}(aq)$$ and $$Ag(s)/Ag^{+}(aq)$$ half-cells, using the resultant emf to drive a motor and measuring the work which it can do
Question 3
1 / -0

Which one of the following metals could not be obtained on electrolysis of aqueous solution of its salts ?

A
Ag

B
Mg

C
Cu

D
Cr

Solution

The reduction potential of $$Mg$$ is less than that of water $$(E^o=-0.83\ V)$$. Hence their ions in the aqueous solution cannot be reduced instead water will be reduced
$$2H_2O +2e^- \to H_2+2OH^-$$.
Question 4
1 / -0

A
$$2\times$$$$10^{-2}$$ $$M$$

B
$$2\times$$$$10^{-3}$$ $$M$$

C
$$1.5\times$$$$10^{-3}$$ $$M$$

D
$$1.5\times$$$$10^{-2}$$ $$M$$

Solution
Question 5
1 / -0

Number of electrons lost during electrolysis of 0.355 g of $$Cl^-$$ is:

A
$$0.01$$

B
$$0.01 N_{0}$$

C
$$0.02 N_{0}$$

D
$$\cfrac {0.01}{2 N_0}$$
Question 6
1 / -0

Without losing its concentration $$ZnCl_2$$ solution cannot be kept in contact with :

A
$$Au$$

B
$$Al$$

C
$$Pb$$

D
$$Ag$$
Question 7
1 / -0

$${{\text{E}}^{\text{o}}}_{{\text{C}}{{\text{u}}^{{\text{2 + }}}}{\text{|Cu = }}}\,{\text{ + 0}}{\text{.337}}\,{\text{V}}\,$$, $${{\text{E}}^{\text{o}}}_{{\text{Z}}{{\text{n}}^{{\text{2 + }}}}{\text{|Zn = }}}\,{\text{-0.762}}\, {\text{V}}\,$$ The EMF of the cell, $${\text{Zn|Z}}{{\text{n}}^{{\text{2 + }}}}\left( {{\text{0}}{\text{.1M}}} \right)||\,{\text{C}}{{\text{u}}^{{\text{2 + }}}}\left( {{\text{0}}{\text{.01M}}} \right){\text{|Cu}}$$ is :

A
$$+1.099 V$$

B
$$-1.099 V$$

C
$$+1.069 V$$

D
$$-1.069 V$$

Solution
Question 8
1 / -0

On the basis of the following $$E^0$$ the strongest oxidising agent is:
$$\begin{array}{l}{\left[ {Fe{{\left( {CN} \right)}_6}} \right]^{4 - }} \to {\left[ {Fe{{\left( {CN} \right)}_6}} \right]^{3 - }} + {e^ - };{E^0} = - 0.35V\\F{e^{2 + }} \to F{e^{3 + }} + {e^ - };{E^0} = - 0.77V\end{array}$$

A
$$F{e^{3 + }}$$

B
$${\left[ {Fe{{\left( {CN} \right)}_6}} \right]^{3 - }}$$

C
$${\left[ {Fe{{\left( {CN} \right)}_6}} \right]^{4 - }}$$

D
$$F{e^{2 + }}$$
Question 9
1 / -0

An amino acid migrates towards the cathode when the electric field is applied. This implies that

A
pH> pl

B
Pl >pH

C
Pl=pH

D
None of these

Solution
Question 10
1 / -0

$$\frac{1}{2}F_{2}+e^{-}\rightarrow F^{-};\ E^{\circ}=+3.02V$$
The electrode potential for given reaction: $$F_{2}+2e^{-}\rightarrow 2F^{-}$$

A
3.02 V

B
6.04 V

C
1.5 V

D
-3.02 V

Solution