Applications of electrolysis - class-XI
| Description: applications of electrolysis | |
| Number of Questions: 75 | |
| Created by: Akash Patil | |
| Tags: redox processes physics chemistry applied chemistry chemical changes chemical effects of electric current element, compound and chemical reaction electrolysis industrial inorganic chemistry |
If $Zn/Zn^{+2}$ electrode is diluted 100 times then the change in electromotive force will be :-
The process of depositing thin layer of a metal over an another metal with a help of electric current is called :
Which pair of electrolytes could not be distinguished by the products of electrolysis using inert electrodes.
Calculate the half cell potential at $298$K for the reactoin ,Zn$^{+2}$ + $2$e$^{-}$ $\rightarrow$ Zn if [Zn$^{+2}$] =$2$M,
E$^{o}$$ _{Zn^{+2}/Zn}$ =-$0.76$V
E$^{o}$
The volume of gases evolved at STP by passing 0.1 ampere of current 49 65 seconds to 1 aqua solution of potassium?
On passing one friday of electric charge through a dilute solution of an acid, the volume of hydrogen obtained at S.T.P. is :
Electrolysis rules of Faraday's states that mass depends on electrodes is proportional to:-
The process of electrolysis is used in:
Electromeric effect involves the completer transfer of
Refining an impure metal to give a pure metal is known as:
The most durable metal plating on iron to protect against corrosion is:
Extracting metals in the pure form from its compound is known as:
Electroplating is:
In the electrolysis of molten $Al _2O _3$ with inert electrodes:
Cost of electricity for the production of $X$ litres of $H _2$ at $NTP$ at the cathode is Rs $X$, then cost of electricity for the production $X$ litres of $O _2$ gas at $NTP$ at the anode will be:
A solution of $CuSO _4$ is electrolysed for $7$ minutes with a current of $0.6A$. The amount of electricity passed is equal to:
In the electroplating of iron by nickel, nickel sulphate solution is taken as electrolyte. What is the acid that is added to the electrolyte during the process?
During electrolysis of an aqueous solution of a salt, pH in the space near one of the electrodes is increased, which of the following salt solution was electrolysed?
A 5-ampere current is passed through a solution of zinc sulphate for $40 $ minutes. The amount of zinc deposited at the cathode is:
The same amount of electricity was passed through two separate electrolytic cells containing solutions of nickel nitrate $\left[ Ni{ \left( { NO } _{ 3 } \right) } _{ 2 } \right]$ land chromium nitrate $\left[Cr{ \left( { NO } _{ 3 } \right) } _{ 3 } \right]$ respectively. If $0.3g$ of nickel was deposited in the first cell, the common of chromium deposited is :
$(at. Wt. Of Ni=59, at. Wt. Of Cr=52)$
A certain quantity of electricity when passed through solution of ${ AgNO } _{ 3 }$, ${ ZnSO } _{ 4 }$, ${ CrI } _{ 3 }$. If X moles of Cr are deposited at its cathode, how many moles of Ag and Zn are deposited at their respective cathodes.
How long (approximate) should water be electrolysed by passing through $100$ amperes current so that the oxygen realised can completely burn $27.66\ g$ of diborane?
(Atomic weight of $B=10.8\ u$ )
The mass of carbon anode consumed (giving only carbondioxide) in the production of 270 kg of Aluminium metal from bauxite by the Hall process is :
The same amount of electricity was passed through two separate electrolytic cells containing solutions of nickel nitrate $[Ni(NO _{3}) _{2}$] and chromium nitrate $[Cr(NO _{3}) _{3}$] respectively.If 0.3 g of nickel was deposited in the first cell, the amount of chromium deposited is:
(at.wt of Ni=59, at. wt. of Cr=52)
On electrolysing a solution of dilute ${ H } _{ 2 }{ SO } _{ 4 }$ between platinum electrodes, the gas evolved at the anode is
In the manufacture of $NaOH$ by the electrolysis of $NaCl$ solution, the cathode and anode are separated using a diaphragm because :
Charge required for liberating $710 g$ of $Cl _{2}(g)$ by electrolyzing a concentrated solution of $NaCl$ will be:
The correct relation is
Which process occurs in the electrolysis of an aqueous solution of nickel chloride at nickel anode?
On the basic of information available from the reaction
$ 4AI + 3O _{2} \rightarrow 2AI _{2}O _{3}; \triangle G = -965$ kJ/mol of $O _{2}$
The minimum EMF required to carry out electrolysis of $ AI _{2}O _{3}$ is
By selecting electrolyte as sodium argentocyanide for electroplating of the metal article with silver. Which of the following condition ensures that deposit is smooth, firm and long-lasting?
A current of 3.7 A is passed for 6 h between nickel electrodes in 0.50 1 of 2 M solution of $Ni(NO _{3}) _{2}$. The molarity of $Ni^{2+}$ at the end of electrolysis is
Which electrolyte is selected for the electroplating of metal article with silver?
During silver plating of an article using potassium argentocyanide as an electrolyte, the anode material should be :
During electroplating of an article with nickel, the reduction reaction of the electrolysis occurs at:
In the electroplating of silver, $AgNO _3$ solution is usually used as:
The metal which is deposited at the cathode during the electrolysis of the solution of silver chloride
Galvanization of iron denotes coating with:
Which of the following is not an electrochemical process?
Galvanized iron sheets are coated with :
Electro refining which is based on phenomenon of Electrolysis where:
State True or False:
Rusting of iron is a physical change.
Which of the following is the preferred electrolyte for silver plating?
Why is electroplating done?
Electroplating is a process of deposition of ________ metal on the surface of _________ metal.
Anode is the _________ block and cathode is the _________ block in electrorefining of metal.
Electroplating is ________________ of metals and electro-refining is ___________ of metals.
The main applications of electrolysis are:
Which one of the following is not a main application of electrolysis?
When an external current is used to induce a non-spontaneous redox reaction, the process is called ________.
In the electrolysis of $CuCl _{2}$ solution, the mass of cathode increased by $6.4\ g$. What occurred at copper anode?
Which is correct about silver plating?
What is the number of moles of oxygen gas evolved by electrolysis of $180\ g$ of water?
When water is electrolysed, hydrogen and oxygen gases are produced. If $1.008\ g$ of $H _{2}$ is liberated at cathode, what mass of $O _{2}$ is formed at the anode?
Zn metal reduces ${SO _{3}}^{2-}$ ions into $H _{2}S$in presence of concentrated $H _{2}SO _{4}$ What weight of Zn is required for
reduction of 6.3 g $Na _{2}SO _{3}$ in presence of concentrated acid.
$Zn\left( s \right) \left|\ Zn{ { \left( CN \right) } } _{ 4 }^{ 2- }\ \left( 0.5\ M \right) ,{ CN }^{ - }\left( 0.01 \right) \right| \left|\ Cu{ \left( { NH } _{ 3 } \right) } _{ 4 }^{ 2+ }\ \left( 0.5\ M \right) ,{ NH } _{ 3 }\left( 1\ M \right) \right|\ Cu\left( s \right) $
Given: ${ K } _{ f }$ of $Zn{ { \left( CN \right) } } _{ 4 }^{ -2\ }=\ { 10 }^{ 16 }$, $\quad \quad \quad$ ${ K } _{ f }$ of $Cu{ \left( { NH } _{ 3 } \right) } _{ 4 }^{ 2+ }\ =\ { 10 }^{ 12 }$
$\displaystyle \quad \quad \ \ { E } _{ Zn|{ Zn }^{ -2 } }\ =\ 0.76V\ ;\ { E } _{ { Cu }^{ +2 }|Cu }\ =\ 0.34V\ ,\ \dfrac { 2.303RT }{ F } =0.06$
The emf of above cell is:
Calculate the mass of Ag deposited at cathode when a current of 2A was passed through a solution of $Ag{ NO } _{ 3 }$ for 15 min.
(Given : Molar mass of $Ag = 108\ g\ { mol }^{ -\ 1 }$ $\ 1F=96500\ C\ { mol }^{ -1 }$).
The electrochemical equivalent of silver is $0.0011180g$. When an electric current of $0.5$ ampere is passed through an aqueous silver nitrate solution for $200sec$, the amount of silver deposited is:
Brine solution on electrolysis will not give__________.
$H _2(g)$ and $O _2(g)$ , can be produced by the electrolysis of water. What total volume (in $L$) of $O _2$ and $H _2$ are produced at $STP$ when a current of $30$ A is passed through a $K _2SO _4\, (aq)$ solution for 193 minutes?
During the mid ninteenth century, Daguerro-type portraits were very popular. A portrait image of a person was made on silver plated copper by developing the image with ?
Silver can be spread as a thin sheet on another metal by electroplating. The film of silver sticks strongly to the metal. Which of the following metals cannot be properly plated with silver?
In electroplating of copper by silver, the silver acts as an :
Electrolysis of brine produces Na at cathode.
In the silver plating of copper, $K[Ag(CN) _2]$ is used instead of $AgNO _3$. The reason is:
In $Ag$ - $CuSO _{4}$ cell, silver electrode will serve as:
Electrolysis of a solution of $Mn{ SO } _{ 4 }$ in aqueous sulphuric acid is a method for the preparation of $MnO _ 2$. Passing a current of $27A$ for $24$ hours gives $1kg$ of $MnO _2$. The current efficiency in this process is:
Consider the reaction : $Cr _2O _7^{2-} + 14H^+ + 6e^- \to 2Cr^{3+}+7H _2O$
What is the quantity of electricity in coulombs needed to reduced $1\ mol$ of $Cr _2O _7^{2-}$?
Calculate the amounts of Na and chlorine gas produced during the electrolysis of fused $NaCl$ by the passage of 1 ampere current for 25 minutes.
A current of $13.4\mathrm { A }$ is passed through $1.0\mathrm { L }$ of $1.0\mathrm { M }$ $HCl$ solution by using $Pt$ electrodes for $1.0\ \mathrm { hr }.$ The $pH$ of the solution after the experiment is over at $298 K$ will be about.
A solution of ${ AgNO } _{ 3 }$ is a good electrolyte but is not used for electroplating an article with silver because :