the quantity of electricity required to reduce 12.3g of nitro benzene to aniline assuming 50% current efficiency is

1) 115800C

2) 57900C

3) 231600C

4) 28950C

Which change requires an oxidising agent?

1- 2S2O3 ---------- S4O6(2-)

2-Zn2+ -------------- Zn

3- ClO- --------- Cl-

4- SO3 -------- SO4(2-)

how to know?

rusting of iron is quicker in saline water than ordinary water.why

Calculate the cell potential for the following cell:

Pb/Pb²⁺ (1x10^-3 M) // Pt, 1/2 Cl₂ (1 bar) / Cl^- (0.1 M)

GIVEN: E⁰ Pb²⁺/Pb= -0.13V and E⁰1/2 Cl₂/Cl^-= 1.358V

The equilibrium constant of the reaction

Cu(s) +2Ag(aq) ---- Cu2+(aq) +2Ag(s) E(standard)cell = 0.46V at 298K is

1- 2 x 10^10 2- 4 x 10^10

3- 4 x 10^15 4- 2.4 x 10^10

Represent the cell in which the following reaction takes place

Mg(s) + 2Ag⁺(0.0001M) ------ Mg²⁺(0.130M) + 2Ag(s)

Calculate its E_(cell) if E⁰_(cell)=3.17 V.

Trick to learn electrochemical series.

Its very urgent due to chemistry first term on Saturday.......

A voltaic cell is set up at 25C with the half-cells Al | Al3+ (0.001 M) and Ni | Ni2+ (0.50 M).

Write the equation for the reaction that occurs when the cell generates an electric current and determine the cell potential.

a current of 0.965 ampere is passed through 500ml of 0.2M solution of ZnSO₄ for 10 min . the molarity of Zn⁺² after deposition of zinc is

1) 0.1M

2) 0.5M3) 0.194M

what is order of a photochemical reaction?Explain in detail.

Total charge required for oxidation of 2 moles Mn₃O₄ into MnO₄^2- in the presence of alkaline medium is:

Q1. During electrolysisof aqueous solution of a salt pH in the space near one of the electrodes is increased. Which of the following salt solution was electrolyzed?
(1) KCL(2) CuCl₂ (3) Cu(NO₃)₂ (4) CuSO₄
​
Q2. The ionic mbilityof alkali metal ions in aqueous solution is maximum for
(1) Na⁺ (2) K⁺ (3) Rb⁺​ (4) Li⁺

Q3. During the recharging of lead acid storage cell the reaction at anode is
(1) Pb^​2+ coverts toPb (2)Pb^​2+coverts toPb​⁴⁺ (3)Pbcoverts toPb​²⁺(4) Pb^​4+ converts to Pb²⁺

Q4. Standard cell voltage for cell Pb/Pb²⁺||Sn²⁺/Snis -0.01V. If the cell is to exhibit E_cell=0, the value of log[Sn²⁺]/[Pb²⁺] should be
(1) 0.33 (2) 0.5 (3) 1.5 (4) -0.5

Q5.The hydrogen electrode is dipped in a solution of pH = 3 at 25^oC. The reduction potential of the electrode would be
(1) 0.177V (2) 0.087V (3) -0.177V (4) 0.059V

Q6. What would be the emf of the given cell?
Pt | H2(P1) | H⁺_(aq) | H_2(P2) |Pt​
(1) RT/ F ln P₁ / P₂(2)RT/ 2FlnP₁/ P₂(3)RT/ FlnP2/ P₁(4)RT/ 2FlnP2/ P₁

For the disproportionation of copper 2Cu+------ Cu2+ + Cu, E(standard)cell is (given E for Cu2+/Cu is 0.34V and E for Cu2+/Cu+ is 0.15V)

1- 0.49V 2- -0.19V

3- 0.38V 4- -0.38V

Zn rod is placed in 100ml of 1M CuSO₄ solution so that molarity of Cu⁺² changes to 0.7M . the molarity of SO₄-- at this stage will be

or reaction , 4Al(s) + 3O₂(g) + 6H₂O + 4OH^- ===== 4[Al(OH)^-]; E^o_cell = 2.73 V. If ΔG^o_f(OH^-)= -157kj/mol and ΔG^of(H₂O) = -237.2 kj/mol , determine ΔG^o_f[Al(OH^-)₄].

Please explain briefly .

aluminium metal cannot be produced by electrolysis of aqueous solution of aluminium salt.give reason.

What type of a cell is the lead storage battery? Write the anode and the cathode reactions and the overall reaction occurring in a lead storage battery while operating

can 1M NiSO4 be stored in a vessel made up of copper ?

given: E(Ni2+/Ni ) = -1.20V and E (Cu2+/Cu) =0.34V

my doubt- as I know (plz correct if am wrong) that E (cell) finally should come out to be positive . if E is positive then reaction will be spontaneous. so the ans will beYES , hence proved.

but if reaction is occuring between NiSO4 and Cu , then HOW NiSO4can be stored in Cu????

plzz clear it.

Two half cell reactions of an electrochemical cell are given below:

What is the electrode potential of a copper wire dipped in 0.1 M CuSO₄solution at 25C if the standard electrode potential of copper is 0.34 volt? PLS EXPLAIN how to know the cell reaction in this question ...

A hydrogen gas electrode is made by dipping platinum wire in a solution of HCl of pH = 10 and by passing hydrogen gas around the platinum wire at one atm pressure, The oxidation potential of electrode would be

1- 0.59V 2- 0.118V

3- 1.18V 4- 0.059V

in SHE , the pH of acid solution should be

1) 7

2) 14

3) 0

CONDUCTIVITY OF 0.12M CUSO4 SOLUTION AT 298K IS 1.8*10 RAISE TO -2 S CM . CALCULATE ITS EQUIVALENT CONDUCTIVITY.

Pleaseexplain the Nernst equation for a general electrochemical reaction of the type

aA+bB--ne--cC+dD

in detail?

the conductivity of pure water in a conductivity cell with electrodes of cross-sectional area 4cm² placed at a distance 2 cm apart in 8 x 10^-7 S cm^-1. calculate the resistanceof conductuvity cell ...........

Standard free energies of formation (in KJ/mol) at 298K are -237.2, -394.4, and -8.2 for H2O(l), CO2(g) and pentane (g) respectively. The value of E(standard)cell for pentane oxygen fuel cell is?

1- 0.0968V 2- 1.968V

3- 2.0968V 4- 0.059V

PbO2 ------- PbO dG(298k)

SnO2 ------- SnO dG(298k) 0

Most probable oxidation state of Pb and Sn will be

1- Pb4+ , Sn4+ 2- Pb4+,Sn2+

3- Pb2+, Sn2+ 4- Pb2+, Sn4+

give a chemical reaction of anode and cathode of corrosion?

For what concentration of Ag+ will the EMF of te given cell be zero at 25 C .If the concentration of Cu²⁺ is 0.1 M. E^oAg⁺ = 0.80v and E^o Cu²⁺ = 0.34 V

Consider the reaction Cr2O72- +14H+ + 6e- gives 2Cr3+ +8H2O

What is the quantity of electricity in coulombs needed to reduce 1 mol of Cr2O72-

During the electrolysis of water 4 mol of electrons were transferred from anode to cathode. the total volume of gases produced at STP will be approximately

The equivalent conductance of M/32 solution of a weak monobasic acid is 8.0 mhos cm^2 and at infinite dilution is 400 mhos cm^2. The dissociation constant of the acid is

1- 1.25 x 10^-4 2- 1.25 x 10^-5

3- 1.25 x 10^-6 4- 6.25 x 10^-4

in two vessel containing 500ml water , 0.5 mol of aniline (Kb = 10^-9) and 25 mmol of HCl are added seperately . Two hydrogen electrodes are constructed using these solutions. Calculate the emf of cell made by connecting them appropriately.

Answer :0.395V

Please explain briefly .

Given

1- Cu2+ + 2e- ----- Cu, E(standard) = 0.337V

2- Cu2+ + e- ------- Cu+ , E(standard) = 0.153V

Electrode potential , E(standard) for the reaction , Cu+ + e- ------ Cu, will be

1- 0.38V 2- 0.52V

3- 0.90V 4-0.30V

the electrolysis of an acetate solution produces ethane and carbon dioxide acc to the reaction

2CH3COO- gives C2H6+2CO2+2e-

The efficiency of reaction is 82%. What volume of C2H6 and CO2 would be produced at 27oCand 740mm pressure if a current of 0.5 ampere is passed through the solution for 7hours?

Two electrolytic cells containing AgNo3 solution and dil.H2SO4 solution are connected in series.A steady current of 2.5 amp was passed till 1.078g of silver was deposited.

a)How much electricity was produced?

b)What was the weight of O2 liberated?

Define molar conductivity of a substance and describe how for weak and strong electrolytes, molar conductivity changes with concentration of solute. How is such change explained?

The electrode potentials for Cu2+ + e- -------- Cu+(aq) and Cu+(aq) + e- ------- Cu(s) are +0.15V and +0.50V respectively. The value of ECu2+/Cu will be?

1- 0.15V 2- 0.5V

3-0.325V 4- 0.650V

Al2O3 is reduced by electrolysis at low potentials and high currents . If 4.0 x 10^4 amperes of current is passed through molten Al2O3 for 6 hours, What mass of aluminium is produced?( Assume 100% current efficiency, At. mass of Al= 27g mol^-1)

1- 1.3 x 10^4g

2- 9 x 10^3 g

3- 8.1 x 10^4 g

4- 2.4 x 10^5 g

During the discharge of lead storage battery the density of sulphuric acid fell from 1.294 to 1.139gcm^-3. The sulphuric acid of density 1.294gcm^-3 is 39% H₂SO₄by mass and that of density 1.139gcm^-3 is 20% by mass. The battery holds 3.5L of acid and the volume remains practically constant duing discharge. Calculate the no. of amper-hours for which battery must have been used.

Equinormal solution of two weak acids , HA(pKa= 3) and HB (pKb = 5) are each placed in contact with standard hydrogen electrode at 25^oC. When a cell is construsted by interconnecting them through a salt bridge , find the emf of the cell.

Answer : E = 0.059

what is the source of electrical energy in galvanic ccell ?

Calculate the emf of the cell in which the following reactions takes place:

Ni(s) + 2Ag⁺(0.002M) ------- Ni²⁺(0.160M) +2Ag(s)

Given that E⁰_(cell) = 1.05 V

phosphorus pentoxide , P4O10 has each phosphorus linked to

1. 5 oxygen atoms with P-P bonds.
2. 5 oxygen atoms
3. 4 oxygen atoms
4. 4 oxygen atoms with P-P bonds

Resistance of 0.2M solution of an eletrolyte is 50ohm. The specific conductance of the solution is 1.4S/m. The resistance of 0.5 M solution of the same electrolyte is 280ohm. The molar conductivity of 0.5 M solution of the electrolyte in Sm2/mol is?

1.5 A current is reduced to 10 minutes in a solution of CuSO4,

How many mass of copper is deposited on the cathode?

One gm metal M3+ was discharging by the passage of 1.81 *1023 electrons.What is the atomic weight of metal?

For both weak and strong electrolytes, molar conductivity increases with decrease in concentration.

how?

1. a) calculate gibbs free energy for the following reaction at 25 degree celcius Au(s)+Ca(2+ 1 aq)----------------- Au(3+ aq 1M)+Ca(s)

EAu(3+)/Au=+1.50 V; E Ca(2+)/Ca=-2.87 V

b)Predict whether the reaction will be spontaneous or not

The number of degenerate orbitals present in an energy level of H-atom characterized by E=-R/16 where R is the Rydberg constant ?

0.1 mole of acetic acid will have better conduction of electricity or 1mole of acetic acid???

1. 56 ml
2. 224 ml
3. 112 ml
4. 448 ml

do non-electrolytes conduct electricity in any form ? metals are non electrolytes or not ?

The reaction, N2(g) + O2(g) 2NO(g) contributes to air pollution whenever a fuel is burnt in air at a high temperature. At 1500 K, equilibrium constant K for it is 1.0 × 105. Suppose in a case [N2] = 0.80 mol L1 and [O2] = 0.20 mol L1 before any reaction occurs. Calculate the equilibrium concentrations of the reactants and the product after the mixture has been heated to 1500 K.

how may minutes it take to plate out 5.0 g of Cr from cr2(So4)3 solution using a current of 1.50 A? (At. Weight ; Cr = 52)