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InterviewSolution
This section includes InterviewSolutions, each offering curated multiple-choice questions to sharpen your knowledge and support exam preparation. Choose a topic below to get started.
| 1651. |
The conductivity of 0.02 M KI solution is 4.37 × 10-4 Ω-1 cm-1. Hence its molar conductivity is :(a) 8.74 × 10-6 Ω-1 cm2 mol-1(b) 21.85 Ω-1 cm2 mol-1(c) 4.58 × 10-4 Ω-1 cm mol-1(d) 136.5 Ω-1 cm-1 mol-1 |
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Answer» Option : (b) 21.85 Ω-1 cm2 mol-1 |
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| 1652. |
The conductivity of 0.02 M AgNO3 at 25°C is 2.428 × 10-3Ω-1cm-1. What is its molar conductivity? |
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Answer» Given : Concentration of solution = C = 0.02 M AgNO3 Temperature = T = 273 + 25 = 298 K Conductivity = κ = 2.428 × 10-3Ω-1cm-1 (or S cm-1) Molar conductivity = ∧m = ? ∧m = \(\frac{k\times 1000}{C}\) = \(\frac{2.428\times 10^{-3}\times 1000}{0.02}\) = 121.4 Ω-1 cm2 mol-1 (or 121.4 S cm2 mol-1) ∴ Molar conductivity = ∧m = 121.4 Ω-1 cm2 mol-1. |
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| 1653. |
Out of the following matals that cannot be obtained by electrolysis of the aquenous solution of their salts isA. CuB. NaC. MgD. K |
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Answer» Correct Answer - A Na, K and Mg are placed above hydrogen in the electrochemical series. When the aqueous solution of these salts are electrolysed, hydrogen is released at the cathode instead of the respective metals. Cu is placed below hydrogen in the electrochemical series, when aqueous solution of copper is electrolysed, copper is deposited at the cathode. |
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| 1654. |
The questions consist of two atatements each, printed as Assertion and Reason. While answering these questions you are required to choose any one of the following four responses : The cell constant of a conductivity cell depends upon the nature of material of the electrodes . The electrodes of the cell are coated with platinum black to avoid polacrization effects.A. If both the assertion and reason are true but the reason is ont the correct explanation of assertionB. If both the assertion and reason are true but the reason is not the correct explanation of assertion.C. If the assertion is true but reason is false.D. If assertion is false but reason is rue |
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Answer» Correct Answer - D Correct Assertopm : The cell constant of the constant of a conductiveity cell depends upon the distance between the electrodes and the area of their cross-section and not on the material of the electrodes . |
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| 1655. |
The questions consist of two atatements each, printed as Assertion and Reason. While answering these questions you are required to choose any one of the following four responses : Specifice conductiviy of an electrolytic solution decreases with dilution , whereas molar conductiviy increase with dilution . Specific conductivirty is the conductance of a specific amount of the electorolyte, whereas molar conductivity is for `1` mole of the electrolyte.A. If both the assertion and reason are true but the reason is ont the correct explanation of assertionB. If both the assertion and reason are true but the reason is not the correct explanation of assertion.C. If the assertion is true but reason is false.D. If assertion is false but reason is rue |
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Answer» Correct Answer - C Correct Reason : Specific conductivity is the conductance of `1 cm^3` of the solution whereas molar conductivity is the conductance of a solution containing `1` mole of the electrolyte . |
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| 1656. |
The questions consist of two atatements each, printed as Assertion and Reason. While answering these questions you are required to choose any one of the following four responses : The cell potential of mercury cell is `1.35 V`, which remains constant . In mercury cell, the electrolute is a paste of KOH and ZnO.A. If both the assertion and reason are true but the reason is ont the correct explanation of assertionB. If both the assertion and reason are true but the reason is not the correct explanation of assertion.C. If the assertion is true but reason is false.D. If assertion is false but reason is rue |
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Answer» Correct Answer - A If both assertion and reason are true and the reason is the correct explanation of the assertion . |
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| 1657. |
The questions consist of two atatements each, printed as Assertion and Reason. While answering these questions you are required to choose any one of the following four responses : Conductiveity always always decreases with the decreased in concentration of both the weak and strong electrolytes. Number of ion per unit volume linearly decreases in both electrolytes.A. If both the assertion and reason are true but the reason is ont the correct explanation of assertionB. If both the assertion and reason are true but the reason is not the correct explanation of assertion.C. If the assertion is true but reason is false.D. If assertion is false but reason is rue |
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Answer» Correct Answer - C Nummber of ions per unit volme is linearly is linearly decreased in strong electolyte but not in weak electorlyte. |
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| 1658. |
The questions consist of two atatements each, printed as Assertion and Reason. While answering these questions you are required to choose any one of the following four responses : copper reacts with hudrochloric acid and ilberates hudrogen from the solution of dilute hydrochloric acid. Hydrogen is below copper in the electrochemical series.A. If both the assertion and reason are true but the reason is ont the correct explanation of assertionB. If both the assertion and reason are true but the reason is not the correct explanation of assertion.C. If the assertion is true but reason is false.D. If assertion is false but reason is rue |
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Answer» Correct Answer - D Cu does not react with HCl and placed below H in electorchemical series. |
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| 1659. |
Assertion: `E^(@)` for `Mn^(3+)//Mn^(2+)` is more positive than `Cr^(3+)//Cr^(2+)` Reason: The third ionisation energy of `Mn` is larger than that of `Cr`.A. If both the assertion and reason are true but the reason is ont the correct explanation of assertionB. If both the assertion and reason are true but the reason is not the correct explanation of assertion.C. If the assertion is true but reason is false.D. If assertion is false but reason is rue |
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Answer» Correct Answer - B `Mn^(2+)` has half -filled d-subshell and more stable thud easily formed or ` E_(Mn^(3+)//Mn)^(2+) gt E_(Cr^(3+)//Cr^(2+)`. |
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| 1660. |
Observe the given diagram and fill in the blanks by choosing the correct option. A. `{:(x,y,z),(H_(2(g))"at 1 atm", 10^(-2) MH^+ , "Finely divided Pt"):}`B. `{:(x,y,z),(H_(2(g))"at 1 bar", 1.00 MH^+ , "Finely divided Pt"):}`C. `{:(x,y,z),( 1.00 MH^+ ,H_(2(g))"at 1 bar", "Finely divided Ni"):}`D. `{:(x,y,z),(H_(2(g))"at 1 bar", 1.00 MH^+ , "Pt granules "):}` |
| Answer» Correct Answer - B | |
| 1661. |
Which of the following reaction is possible at anode ?A. `2Cr^(3+) + 7H_2O to Cr_2O_7^(2-) + 14 H^+`B. `F_2 to 2F^-`C. `(1//2)O_2 + 2H^(+) to H_2O`D. None of these |
| Answer» Correct Answer - A | |
| 1662. |
Which of the following statement is correct about the given Daniell cell? A. This cell converts the electrical energy liberted during the redox reaction to chemical energy.B. This cell has an electricel potential greater that 1.1 v when concertation of `Zn^(2+)` and `Cu^(2+)` ions is unity (1 mol `dm^(-3)` )C. In this cell, copper is acting as cathode and zinc is acting as anode.D. Redox reaction occurring in this cell is `Cu_((s))+Zn_((aq))^(2+) to Cu_((aq))^(2+) +Zn_((s))` |
| Answer» Correct Answer - C | |
| 1663. |
The cell reaction of the galvanic cell : `Cu_((s))|Cu_((aq))^(2+) ||Hg_((aq))^(2+) |Hg_((l))` isA. `Hg+Cu^(2+) to Hg^(2+) +Cu`B. `Hg+Cu^(2+) to Cu^(+) +Hg^+`C. `Cu+Hg to CuHg`D. `Cu+ Hg^(2+) to Cu^(2+) + Hg` |
| Answer» Correct Answer - D | |
| 1664. |
A metal is known to form fluoride `MF_(2)`. When `10` ampere electricity is passed through a molten salt for `330` sec, `1.95 g` metal is deposited. Find out the atomic weight of metal. What will be the quantity of charge required to deposit the same mass of `Cu` from `CuSO_(4)(aq.)`? (`At. wt.` of `Cu = 63.6`)A. 57.02B. 148C. 228D. 114 |
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Answer» Correct Answer - D i=10 amp , t = 330 sec , w = 1.95 gm , E = ? `W = (ixxt xx E)/(96500)` `therefore E = (W xx 96500)/(ixxt) = (1.95 xx 96500)/(10 xx 330) = 57.02` Molten salt is `MF_(2)` Valency of fluorine = `(-1) xx 2 = -2` `therefore` Valency of M= + 2 `E = ("At. mass")/("valency")` `therefore` At. mass = `E xx` valency `= 57.02 xx 2 = 114.04 = 114` |
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| 1665. |
A metal is known to form fluoride `MF_(2)`. When `10` ampere electricity is passed through a molten salt for `330` sec, `1.95 g` metal is deposited. Find out the atomic weight of metal. What will be the quantity of charge required to deposit the same mass of `Cu` from `CuSO_(4)(aq.)`? (`At. wt.` of `Cu = 63.6`) |
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Answer» Eq. of metal `= (i.t)/(96500)` `(i = 10 "ampere", t = 330 sec.)` `(1.95)/(E) = (10 xx 330 sec)/(96500)` `E_("metal") = 57.0` `At. wt.` of metal `= 57.0 xx 2 = 114.0` metal is bivalent as salt is `MF_(2)` Also, if `w_(Cu) = 1.95 g`, then or `(1.95)/(63.6//2) = (i.t)/(96500)` `:. i.t = Q = 5917.45` coulomb |
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| 1666. |
3A current was passed through an aqueous solution of an unknown salt of `Pd` for 1hr. `2.977 g` of `Pd^(+n)` was deposited at cathode. Find n. |
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Answer» Correct Answer - `n =4` `Pd^(+n) +nE rarr Pd` `n_(Pd) = (2.977)/(106.4)` `n_(Pd) = 0.028` `n_(E) = 0.028 xx n` `= (0.0238 xx n xx 96500)/(3600) =3 [1=(q)/(t)]` `n = 4` |
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| 1667. |
The emf of a cell containing sodium/copper electrode is 3.05 V, if the electrode potential of copper electrode is +0.34 V, the electrode potential of sodium is :A. `-2.71 V`B. `+2.71 V`C. `-3.71 V`D. `+3.71 V` |
| Answer» Correct Answer - A | |
| 1668. |
The number of moles of oxygen obtained by the electrolytic decomposition of 90g water is :A. `2.5`B. `5.0`C. `7.5`D. `10.0` |
| Answer» Correct Answer - B | |
| 1669. |
How many coulombs are required for the oxidation of `1 mol` of `H_(2)O` to `O_(2)`?A. `1.93xx10^(5)C`B. `96500C`C. `(92500)/(2)C`D. `19.30xx10^(5)C`. |
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Answer» Correct Answer - a Oxidation of `H_(2)O` to `O_(2)` `2H_(2)Orarr4H^(+)+O_(2)+4e^(-)` 2 mol 4 mol 1 m ol 2 mol `therefore` one mole of water release 2 moles of electrons on oxidation 1 mol of electron =96500C 2 moles of electrons =`2xx96500C` |
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| 1670. |
The cost of electricity required to deposit 1 g of Mg is Rs.3.00. The cost of deposit 8 g of Al is (al.mass Al = 27 , Mg = 24)A. Rs.`12.00`B. Rs. `24.00`C. Rs. `32.00`D. Rs.`42.50` |
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Answer» Correct Answer - C `(W_(Al))/(W_(Mg)) = (E_(Mg))/(E_(Al))` `therefore (W_(Al))/(1) = (24//2)/(27//3) = (12)/(9)` `therefore W_(Al) = (12)/(9)` gms. When 1 gm of Mg deposited at the same time , `(12)/(9)` gm of Al deposited by passing same quantity of electricity For 1 gm Mg `-=` it cost three rupees `therefore (12)/(9) g Al -= x : x = (3 xx (12//9))/(1) = 4` rupees `therefore` For 8 gm of Al `-= 8 xx 4 = 32` rupees |
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| 1671. |
To deposit 1 mol of aluminium from molten `Al_(2)O_(3)`. What is the amount of electricity (in coulombs) required ? |
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Answer» Correct Answer - `2.895xx10^(5) C` `Al_(2)O_(3)(l) to 2Al(s)+3//2O_(2)(g)` The ionic equation for the reaction is : `Al^(3+)(aq)+underset(3xx96500C)(3e^(-)) to underset(1" mol")Al(s)` `=3xx96500C=2.895xx10^(65)" C"`. |
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| 1672. |
How long will it take for a current of 3 amperes to decompose 36g of water? (Eq. wt. of hydrogen is 1 and that of oxygen is 8)A. 36 hors apporxB. 18hours approx.C. 9 hours approxD. 4-5 hours approx. |
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Answer» Correct Answer - A `W=Z I t` Eq. mass of water `=("Mol.mass")/(2)=(18)/(2)=9` `Z=("Eq. mass of water")/(96500)=(9)/(96500)` `36g=(9)/(96500)xx3xxt `therefore t=128866.7s=36` hours. |
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| 1673. |
The charge required to liberate 11.5 g sodium from fused sodium chloride isA. 1 FaradayB. 0.5FaradayC. 1.5FaradayD. 96500 Coulomb. |
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Answer» Correct Answer - A For 23 g Na, charge required =1 Faraday For 11.5g Na. charge required `=(1)/(23)xx11.5=0.5` Faraday. |
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| 1674. |
the number of electrons required to deposit 1g equivalent aluminium (At. Wt. =27) from a solution of aluminium chloride will beA. 1B. 2C. 3D. 4 |
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Answer» Correct Answer - A `Al^(3+)+3e^(-)rarrAl` For 27g Al electrons needed=3 For `(27)/(3)g Al` elec trons needed `=(3)/(27)xx(27)/(3)=1` electron |
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| 1675. |
The variation of `E_("cell")` with temperature i.e., `((deltaE)/(deltaT))_(P)` is equal to :A. `(DeltaS)/(nF)`B. `(DeltaH-DeltaG)/(nFT)`C. `[n(DeltaH)/(nF)]//T`D. All of these |
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Answer» Correct Answer - D `DeltaG = DeltaH + T ((partialDeltaG)/(partialT))` and `DeltaG = DeltaH - TDeltaS` and `DeltaG = -nEF` |
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| 1676. |
In an aqueous solution, hydrogen `(H_(2))` will not reduce:A. `Fe^(3+)`B. `Cu^(2+)`C. `Zn^(2+)`D. `Ag^(+)` |
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Answer» Correct Answer - C Only `Zn` and `Fe` are above `H`, Also `Fe^(3+)` can be reduced to `Fe^(2+)` by `H`. |
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| 1677. |
A student made the following observations in the laboratory: (i) Clean copper metal did not react with `1` molar `Pb(NO_(3))_(2)` solution (ii) Clean lead metal dissolved in a `1` molar `AgNO_(3)` solution and crystals of `Ag` metal appeared (iii) Clean silver metal did not react with `1` molar `Cu(NO_(3))_(2)` solutions.A. `Cu, Pb, Ag`B. `Cu, Ag, Pb`C. `Pb, Cu, Ag`D. `Pb, Ag, Cu` |
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Answer» Correct Answer - C Metal having more `E_(OP)^(@)` replaces the other form its salt solutions. |
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| 1678. |
A student made the following observations in the laboratory i) clean copper metal did not react with 1 molar Pb `(NO_(3))_(2)` solution ii) clean lead metal dissolved in a 1 molar `AgNO_(3)` solution and crystals of Ag metal appeared iii) clean silver metal did not react with 1 molar `Cu(NO_(3))_(2)` solution The order of decreasing reducing character of the three metals isA. Cu , Pb , AgB. Cu , Ag , PbC. Pb , Cu , AgD. Pb , Ag , Cu |
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Answer» Correct Answer - C Metal placed below in electrochemical series replaces the other from its salt solutions . |
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| 1679. |
When the same electric current is passed through the solution of different electrolytes in series, the amounts of elements deposited on the electrodes are in the ratio of theirA. at.noB. at.massC. sp.gravityD. eq.mass |
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Answer» Correct Answer - D `w prop E ` , if Q = constant . |
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| 1680. |
An electric current is passed through following aqueous solutions . Which one shall decomposeA. ureaB. glucoseC. silver nitrateD. ethyl alcohol |
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Answer» Correct Answer - C `AgNO_(3)` is an electrolyte . |
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| 1681. |
Among `Na, Hg, S, Pt` and graphite, which can be used as electrodes in electrolystic cells having aqueous solutions?A. Na and SB. Na, Hg and PtC. Na, Hg and SD. Hg, Pt and graphite |
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Answer» Correct Answer - D Na cannot be used in aqueous solution as it reacts violently with water . |
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| 1682. |
Molar conductivity of inic solution depends on ........A. temperatureB. distance between electrodesC. concentration of electrolysis in solutionD. surface area of electrodes |
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Answer» Molar conductivity due to ions furnished by one mole of electrolyte in solution. Molar conductivity of ionic solution depends on (i) Temperature Molar conductivity of electrolyte solution increases with increase in temperature . (ii) Concentarton of electrolytes in solution As concentration of electrolysis increases. molar conductivity decreases. ltbr. `therefore lambda=(k)/(c)` |
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| 1683. |
Which of the following is used widely in the manufacture of lead storage batteryA. ArsenicB. LithiumC. BismuthD. Antimony |
| Answer» Correct Answer - D | |
| 1684. |
Molar conductivity of inic solution depends on ........A. temperatureB. distance between electrodesC. concentration of electrolytes in solutionD. surface area of electrodes. |
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Answer» Correct Answer - A::C (a, c) are both correct options. |
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| 1685. |
In the reaction `Cu_((s))+2Ag_((aq))^(+)toCu_((aq))^(2+)+2Ag_((s))` the reduction half-cell reaction is:-A. `Cu+2e^(-)toCu^(2-)`B. `Cu-2e^(-)toCu^(2+)`C. `Ag^(+)+e^(-)toAg`D. `Ag-e^(-)toAg^(+)` |
| Answer» Correct Answer - C | |
| 1686. |
Which of the following condition will increase the voltage of the cell, represented by the equation `Cu_((s))+2Ag_((aq))^(+)toCu_((aq))^(2+)+2Ag_((s))`A. Increase in the concentration of `Ag^(+)` ionB. Increase in the concentration of `Cu^(+)` ionC. Increase in the dimension of silver electrodeD. Increase in the dimension of copper electrode |
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Answer» Correct Answer - A Increase in the concentration of `Ag^(+)` ion increase the voltage of the cell. |
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| 1687. |
Conductivity k, is equal to ......A. `(1)/(R)(l)/(A)`B. `(G^(*))/(R)`C. `Lambda_(m)`D. `(l)/(A)` |
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Answer» As we know that, conductance is reciprocal of resistance an d conductivity is the conductance of `1cm^(3)` of substance Also, conductivity is reciprocal of resistivity. `k=(1)/(rho)` `R=rho(l)/(A)` `rho=(R.A)/(l)rArrk=(1)/((R.A)/(l))` `k=(1)/(R).(l)/(A)=(1)/(R)xx(G^(*))/(R)` Hence, options (a) and (b) are the correct choices. |
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| 1688. |
Conductivity k, is equal toA. `(1)/(R )(l)/(A)`B. `(G^(**))/(R )`C. `Lambda_(m)`D. `(l)/(A)` |
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Answer» Correct Answer - A::B (a, b) are both correct options. |
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| 1689. |
Dilution of an electrolyte helps in increasing its electrical conductivity. But it has an adverse effect as well. Discuss. |
| Answer» On dilution of the electrolyte, the ions get hydrated e.g., `Na^(+)(aq)` and `Cl^(-)(aq)`. As a result, their size increases and mobility decreases. This will result in decreasing the electrical conductivity. | |
| 1690. |
In electrolysis , oxidation takes place atA. anodeB. cathodeC. both at the anode as well as cathodeD. the surface of electrolyte solution |
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Answer» Correct Answer - A Anode is electrode at which oxidation occurs . |
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| 1691. |
When a molten ionic hydride is electrolysed.A. Hydrogen is liberted at the cathodeB. H-ions produced migrate to the cathodeC. There is no reasctionD. Hydrogen is liberted at the anode |
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Answer» Correct Answer - D On elctrolysis molten ionic hydride liberates `H_2` at the anlde. |
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| 1692. |
Explain the effect of dilution of solution on conductivity ? |
Answer»
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| 1693. |
Which loses charge at cathodeA. ionsB. cationsC. anionsD. both anions and cations |
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Answer» Correct Answer - B Cations carrying positive charge move towards cathode where they get discharged . |
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| 1694. |
The passage of 0.95 A current for 40 minutes deposited 0.7493 g Cu from CuSO4 solution. Calculate the molar mass of Cu. |
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Answer» Given : Electric current = I = 0.95 A Time = f = 40 min = 40 × 60 = 2400 s Mass of Cu deposited = 0.7493 g Molar mass of Cu = ? Reduction half reaction, \(Cu^{2+}_{(aq)}\) + 2e- ⟶Cu(s) Quantity of electricity = Q = I × t = 0.95 × 2400 = 2280 C Number of moles of electrons = \(\frac{2280}{96500}\) = 0.02362 mol ∵ 2 mol electrons deposit 1 mol Cu ∴ 0.02362 mol electrons will deposit, \(\frac{0.02362}{2}\) = 0.01181 mol Cu Now, 0.01181 mol Cu weighs 0.7493 g ∴ 1 mol of Cu weigh, \(\frac{0.7493\times 1}{0.01181}\) = 63.44 g Hence molar mass of Cu 63.44 g mol-1 ∴ Molar mass of Cu = 63.44 g mol-1. |
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| 1695. |
What will happen during the electrolysis of aqueous solution of `CuSO_(4)` in thee presence of Cu electrodes?A. Copper will deposit at cathode.B. Copper will dissolve at anode.C. Oxygen will be released at anode.D. Copper will deposit at anode. |
| Answer» Correct Answer - A::B | |
| 1696. |
In the electrolysis of a `40L CuSO_(4)` solution, there are two possible reactions at anode `:` `i. Cu rarr Cu^(2+)+2e^(-)` `ii. 2H_(2)O rarr 4H^(o+)+4e^(-)+O_(2)` A current of `1.07 A ` is passed for 2 hours. The loss in the mass of `Cu` at anode was `1.27 g`. `(` Atomic weight of `Cu =63.5g mol ^(1))`. Which of the following statement`(s)` is `//` are correct ?A. `0.08 mol` of electrons are passed through the solution during entire electrolysisB. `224mL` of `O_(2)(g)` is liberated at `STP` at anode.C. Fraction of current in the production of `Cu^(2+)` ions `=0.5.`D. `pH` drops to 3 |
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Answer» Correct Answer - a,b,c,d `a.` Statement `(a)` is correct Amound of `Cu` converted to `Cu^(2+)` ions `=(1.27g)/(63.5g mol^(-1))` `[2F-=1 mol `of `Cu^(2+)]` Amount of electrons involved `=2xx0.02=0.04 mol`. Amount of electrons actually passed through solution `=(1.07xx2xx60xx60)/(96500)` `0.08 mol` `b.` Statement `(b)` is correct Amount of electrons involved is converting `H_(2)O` to `O_(2)` `=0.08-0.04` `=0.04 mol` Amount of `O_(2)` liberated at anode `=(1)/(4)xx0.04` `=0.01mol` `:.` Volume of `O_(2)` produced at `STP` at anode `=0.01xx22400mL=224 mL` `c.` Statement `(c)` is correct Fraction of current used in the production of `Cu^(2+)` ions `=(0.04)/(.08)=0.5` `d.` Statement `(d)` is correct `:` `:gt `Mol of `H^(o+)` ions produced at andoe `=0.04 mol` `:. [H^(o+)]_(anode)=(0.04 mol)/(40L)=10^(-3)mol L^(-1)` `:. pH=-log(10^(-3))=3` |
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| 1697. |
What will happen during the electrolysis of aqu eous solution of `CuSO_(4)` in the presence of Cu electrodes?A. Copper will deposit at cathodeB. Copper will deposit at anodeC. Oxygen will be released at anodeD. Copper will deposit at anode |
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Answer» Correct Answer - A::B (a, b) are both correct options. |
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| 1698. |
What will happen during the electrolysis of aqu eous solution of `CuSO_(4)` in the presence of Cu electrodes?A. Copper will deposit at cathodeB. Copper will disolve at anodeC. Oxygen will be released at anodeD. Copper will deposit at anode |
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Answer» Electrolysis of `CuSO_(4)` can be represented by two half cell reactions these occuring at cathode and anode respectively as At cathode `Cu^(2+)+2e^(-)rarrCu(s)` At anode `Cu(s)rarrCu^(2+)+2e^(-)` Here, Cu will deposit at cathode while copper will dissolved at anode. Hence, options a and b are the correct choices. |
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| 1699. |
Which one of the following is not the correct representation?A. `E_("cell")^(@)` = Red. Pot. Of cathode + Oxide pot. of anodeB. `E_("cell")^(@)` = Red. Pot of cathode - Oxid. pot. of anodeC.D. `E_("cell")^(@)` = Red. Pot of cathode - Red. pot of anode |
| Answer» Correct Answer - B | |
| 1700. |
STATEMENT-1: 1 coulomb charge deposits 1 g-equivalent of a substance. STATEMENT-2: 1 faraday is charge is charge on 1 mole of electrons.A. If both assertion and reason are correct and reason is correct explanation for assertion.B. If both assertion and reason are correct but reason is not correct explanation for assertion.C. If assertion is correct but reason is incorrect.D. If assertion and reason both are incorrect. |
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Answer» Correct Answer - C (c ) Correct reason : One Faraday deposits one gram equivalent of the substance. |
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