Question 1

How many seconds are required to produce 4.00 g of aluminum metal from the electrolysis of molten  with an electrical current of 12.0 A?

Accepted Answer

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Question 2

The standard emf for the cell using the overall cell reaction below is +2.20 V: 2 Al(s)+ 3 I₂(s)→ 2 Al³⁺(aq)+ 6 I^-(aq) The emf generated by the cell when [Al³⁺] = 4.5 × 10^-³ M and [ ] = 0.15 M is

Accepted Answer

The Nernst equation can be used to calculate the cell potential at non-standard conditions:
Ecell = E°cell - (RT/nF)*ln(Q)
where R is the gas constant, T is the temperature in Kelvin, n is the number of electrons transferred in the cell reaction, F is Faraday's constant, and Q is the reaction quotient.
Plugging in the given values:
Ecell = 2.20 - (0.0257/3)*ln((0.15)^6/(4.5*10^-4))
Ecell = 2.32 V (rounded to two significant figures)
Therefore, the answer is B.

Question 3

The standard cell potential (E°)of a voltaic cell constructed using the cell reaction below is 0.76 V: Zn(s)+ 2 H⁺(aq)→ Zn²⁺(aq)+ H₂(g) With = 1.0 atm and [Zn²⁺] = 1.0 M,the cell potential is 0.66 V.The concentration of in the cathode compartment is ________ M.

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Question 4

The standard emf for the cell using the overall cell reaction below is +0.48 V: Zn(s)+ Ni²⁺(aq)→ Zn²⁺(aq)+ Ni(s) The emf generated by the cell when [Ni²⁺] = 2.50 M and [Zn²⁺] = 0.100 M is

Accepted Answer

We can use the Nernst equation to calculate the cell potential:

Ecell = E°cell - (RT/nF) * ln(Q)

where R is the gas constant (8.314 J/K·mol), T is the temperature in Kelvin, n is the number of electrons transferred (in this case, 2), F is the Faraday constant (96,485 C/mol), and Q is the reaction quotient, which is:

Q = [Ni]/[Zn]

Plugging in the values:

Ecell = 0.48 V - (8.314 J/K·mol)(298 K)/(2*96,485 C/mol) * ln(2.50/0.100)
Ecell = 0.52 V

Therefore, the answer is C.

Question 5

Which of the following reactions would be the most spontaneous at 298 K?

Accepted Answer

The more positive the value of E°cell, the more spontaneous the reaction is. Therefore, choice D has the highest positive E°cell value of +1.22 V and is the most spontaneous at 298 K.

Question 6

How many electrons are transferred in the following reaction? (The reaction is unbalanced.) Ni²⁺(aq)+ Na(s)→ Ni(s)+ Na⁺(aq)

Accepted Answer

In the unbalanced reaction, NiS and NaS have a charge of -1, while Na has a charge of +1. Therefore, Ni²⁺(aq)+ Na(s) corresponds to an oxidation-reduction reaction where Ni gets reduced and Na gets oxidized. Each sodium atom loses one electron, while each nickel atom gains two electrons, which means overall two electrons are transferred. Hence the correct answer choice is B.

Question 7

How many grams of nickel metal are plated out when a constant current of 15.0 A is passed through aqueous NiCl₂ for 60.0 minutes?

Accepted Answer

To find the mass of nickel plated out, we use Faraday's laws of electrolysis. The amount of substance deposited at an electrode is directly proportional to the quantity of electricity that flows through the circuit. The charge (Q) in coulombs is given by Q = It, where I is the current in amperes and t is the time in seconds. Here, I = 15.0 A and t = 60.0 minutes = 3600 seconds, so Q = 15.0 A * 3600 s = 54000 C.The molar mass of nickel (Ni) is approximately 58.69 g/mol, and it has a valency of 2, meaning it requires 2 moles of electrons to deposit one mole of nickel. The charge per mole of electrons (Faraday's constant) is approximately 96485 C/mol. Therefore, the number of moles of nickel deposited is given by the total charge divided by twice the charge per mole of electrons (because Ni^2+ requires 2 electrons to become Ni metal):Moles of Ni = Q / (2 * 96485 C/mol) = 54000 C / (2 * 96485 C/mol) = 0.2796 molThe mass of nickel deposited can then be calculated by multiplying the moles of nickel by its molar mass:Mass of Ni = 0.2796 mol * 58.69 g/mol = 16.4 g

Question 8

Using the following standard reduction potentials, Fe³⁺(aq)+ e^- → Fe²⁺(aq)E° = +0.77 V Ni²⁺(aq)+ 2 e^- → Ni(s)E° = -0.23 V Calculate the standard cell potential for the galvanic cell reaction given below,and determine whether or not this reaction is spontaneous under standard conditions. Ni²⁺(aq)+ 2 Fe²⁺(aq)→ 2 Fe³⁺(aq)+ Ni(s)

Accepted Answer

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Question 9

How many electrons are transferred in the following reaction? (The reaction is unbalanced.) Ni(s)+ Cr³⁺(aq)→ Cr(s)+ Ni²⁺(aq)

Accepted Answer

Ni loses two electrons to form Ni²⁺, and Cr³⁺ gains one electron to form Cr. So, a total of 3 electrons are transferred.

Question 10

The electrolysis of molten AlCl₃ for 3.25 hr with an electrical current of 15.0 A produces ________ g of aluminum metal.

Accepted Answer

The mass of aluminum produced can be calculated using Faraday's law of electrolysis. The molar mass of aluminum (Al) is 26.98 g/mol, and it has a valency of 3, meaning 3 moles of electrons are required to produce 1 mole of aluminum. The total charge (Q) passed through the electrolyte is current (I) times time (t), Q = I × t = 15.0 A × 3.25 × 3600 s = 175500 C. Since 1 mole of electrons corresponds to 96500 C (Faraday constant), the moles of electrons used are 175500 C / 96500 C/mol = 1.818 moles. Since it takes 3 moles of electrons to produce 1 mole of Al, the moles of Al produced are 1.818 moles of electrons / 3 = 0.606 moles of Al. Finally, the mass of Al produced is 0.606 moles × 26.98 g/mol = 16.4 g.

Question 11

For a galvanic cell that uses the following two half-reactions, Cr₂O₇^2-(aq)+ 14 H⁺(aq)+ 6 e^- → 2 Cr³⁺(aq)+ 7 H₂O(l) Sn(s)→ Sn²⁺(aq)+ 2 e^- How many moles of Sn(s)are oxidized by four moles of Cr₂O₇^2-?

Accepted Answer

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Question 12

How many kilowatt-hours of electricity are used to produce 3.00 kg of magnesium in the electrolysis of molten  with an applied emf of 4.50 V?

Accepted Answer

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Question 13

Given that E°_red = -0.40 V for Cd²⁺/Cd at 25°C,find E° and E for the concentration cell expressed using shorthand notation below. Cd(s)∣ Cd²⁺(1.0 × 10^-5 M)∣∣ Cd²⁺(0.100 M)∣ Cd(s)

Accepted Answer

The shorthand notation represents a concentration cell where the anode and cathode compartments have different concentrations of the same species. In this case, the anode compartment has a concentration of 1.0 × 10-5 M CdS1P12+S/0.1 M Cd, while the cathode compartment has a concentration of 0.1 M CdS1P12+S/0.1 M Cd.

To find E° and E, we need to use the Nernst equation:

E = E° - (RT/nF) ln(Q)

where Q is the reaction quotient, defined as the product of the concentrations of the species on the right side of the half-reaction over the product of the concentrations of the species on the left side of the half-reaction.

For the anode half-reaction:

CdS1P12+S + 2e- → Cd + S1P0

we have:

E°anode = -0.40 V
n = 2
Qanode = [Cd2+]/[CdS1P12+S][S1P0]2

Since the anode compartment has an excess of Cd, [Cd2+] = 0.1 M, while [CdS1P12+S] and [S1P0] are as given above. Therefore:

Qanode = (0.1 M)/(1.0 × 10-5 M)(0.1 M)2 = 1000

For the cathode half-reaction:

CdS1P12+S + 2e- → Cd + S1P0

we have:

E°cathode = 0.00 V
n = 2
Qcathode = [Cd2+]/[CdS1P12+S][S1P0]2

Since the cathode compartment has a lower concentration of CdS1P12+S, [CdS1P12+S] = 0.1 M, while [Cd2+] and [S1P0] are as given above. Therefore:

Qcathode = (0.1 M)/(0.1 M)(0.1 M)2 = 1

Substituting into the Nernst equation, we get:

Eanode = -0.40 V - (0.0257 V/K)(298 K)/(2 F) ln(1000) = -0.64 V
Ecathode = 0.00 V - (0.0257 V/K)(298 K)/(2 F) ln(1) = 0.00 V

The overall cell potential is given by:

Ecell = Ecathode - Eanode = 0.64 V

And since the shorthand notation represents a concentration cell, we know that E°cell = 0.00 V, so:

E° = E°cell - (RT/nF) ln(Kcell)

where Kcell = [Cd2+]anode/[Cd2+]cathode = 1000/1 = 1000

Substituting the values and solving for E°, we get:

E° = 0.00 V - (0.0257 V/K)(298 K)/(2 F) ln(1000) = -0.64 V

Therefore, the answer is B: E° = 0.00 V and E = +0.12 V.

Question 14

A voltaic cell is constructed with two Zn²⁺-Zn electrodes,where the half-reaction is Zn²⁺ + 2e^- → Zn(s)E° = -0.763 V The concentrations of zinc ion in the two compartments are 5.50 M and 1.11 × 10^-2 M,respectively.The cell emf is ________ V.

Accepted Answer

The cell emf can be calculated using the Nernst equation. Since both electrodes are the same, the standard cell potential is 0 V. The Nernst equation is E = E° - (RT/nF) * ln(Q), where Q is the reaction quotient. For this cell, E = 0 - (0.0257/2) * ln(1.11 × 10^-2 / 5.50), which calculates to approximately 0.0798 V.

Question 15

Based on the following information, I₂(s)+ 2 e^- → 2 I^-(aq)E° = +0.54 V Cd²⁺(aq)+ 2 e^- → Cd (s)E° = -0.40 V Which of the following chemical species is the strongest reducing agent?

Accepted Answer

The strongest reducing agent is the one that is most easily oxidized. Cd(s) has the lowest (most negative) standard reduction potential, indicating it is the strongest reducing agent among the given species.

Question 16

How many electrons are transferred in the following reaction? (The reaction is unbalanced.) Br₂(s)+ Fe(s)→ Fe³⁺(aq)+ Br⁻(aq)

Accepted Answer

In the reaction, each Fe atom loses 3 electrons to become Fe³⁺, and each Br₂ molecule gains 2 electrons to form 2 Br⁻ ions. To balance the electrons transferred, 3 Br₂ molecules are needed to accept 6 electrons from 2 Fe atoms, resulting in a total of 6 electrons transferred.

Question 17

How many grams of chromium metal are plated out when a constant current of 8.00 A is passed through an aqueous solution containing Cr³⁺ ions for 320.minutes?

Accepted Answer

The amount of chromium plated out can be calculated using Faraday's laws of electrolysis. The mass of a substance deposited or liberated at an electrode is directly proportional to the quantity of electricity that passes through the electrolyte. The quantity of electricity (Q) can be calculated as Q = I × t, where I is the current in amperes and t is the time in seconds. Here, I = 8.00 A and t = 320 minutes = 320 × 60 seconds = 19200 seconds. So, Q = 8.00 × 19200 = 153600 C.The molar mass of chromium (Cr) is approximately 52 g/mol, and the valency of chromium in the Cr^3+ ion is 3. The charge of one mole of electrons (the Faraday constant) is approximately 96485 C/mol. Therefore, the mass (m) of chromium deposited can be calculated using the formula m = (M × Q) / (n × F), where M is the molar mass, Q is the total charge, n is the valency, and F is the Faraday constant.Substituting the values, we get m = (52 g/mol × 153600 C) / (3 × 96485 C/mol) ≈ 27.6 g.

Question 18

The gas OF₂ can be produced from the electrolysis of an aqueous solution of KF,as shown in the equation below. OF₂(g)+ 2 H⁺(aq)+ 4 e^- → H₂O(l)+ 2 F^-(aq)E° = +2.15 V Using the given standard reduction potential,calculate the amount of OF₂ that is produced,and the electrode at which the OF₂ is produced,upon the passage of 0.480 faradays through an aqueous KF solution.

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Question 19

The most useful ore of aluminum is bauxite,in which Al is present as hydrated oxides,Al₂O₃ ∙ xH₂O.The number of kilowatt-hours of electricity required to produce 4.00 kg of aluminum from electrolysis of compounds from bauxite is ________ when the applied emf is 5.00 V.

Accepted Answer

The production of aluminum from bauxite requires electrolysis, which involves the conversion of Al3+ ions to aluminum metal. The process requires 3 moles of electrons per mole of aluminum. Using Faraday's laws of electrolysis, the charge required can be calculated, and then the energy in kilowatt-hours can be determined using the given voltage. The correct calculation leads to 59.6 kWh.

Question 20

A voltaic cell is constructed with two silver-silver chloride electrodes,where the half-reaction is AgCl(s)+ e^- → Ag(s)+ Cl^-(aq)E° = +0.222 V The concentrations of chloride ion in the two compartments are 0.0222 M and 2.22 M,respectively.The cell emf is ________ V.

Accepted Answer

The Nernst equation for the given half-reaction is Ecell = E° - (0.0592/n) log Q, where n is the number of electrons transferred and Q is the reaction quotient. In this case, n is 1 since only 1 electron is transferred. The reaction quotient can be calculated as Q = [Ag+]/[Cl-]. At standard conditions, both compartment have [Ag+] = [Cl-] = 1 M, so Q = 1. At non-standard conditions, the anode compartment has [Cl-] = 0.0222 M and the cathode compartment has [Cl-] = 2.22 M, so Q = 0.01. Thus, Ecell = 0.222 - (0.0592/1) log 0.01 = 0.118 V. The correct answer is B.

Quiz 19: Electrochemistry

How many seconds are required to produce 4.00 g of aluminum metal from the electrolysis of molten with an electrical current of 12.0 A?

The standard emf for the cell using the overall cell reaction below is +2.20 V: 2 Al(s) + 3 I₂(s) → 2 Al³⁺(aq) + 6 I^-(aq) The emf generated by the cell when [Al³⁺] = 4.5 × 10^-³ M and [ ] = 0.15 M is

The standard cell potential (E°) of a voltaic cell constructed using the cell reaction below is 0.76 V: Zn(s) + 2 H⁺(aq) → Zn²⁺(aq) + H₂(g) With = 1.0 atm and [Zn²⁺] = 1.0 M,the cell potential is 0.66 V.The concentration of in the cathode compartment is ________ M.

The standard emf for the cell using the overall cell reaction below is +0.48 V: Zn(s) + Ni²⁺(aq) → Zn²⁺(aq) + Ni(s) The emf generated by the cell when [Ni²⁺] = 2.50 M and [Zn²⁺] = 0.100 M is

Which of the following reactions would be the most spontaneous at 298 K?

How many electrons are transferred in the following reaction? (The reaction is unbalanced.) Ni²⁺(aq) + Na(s) → Ni(s) + Na⁺(aq)

How many grams of nickel metal are plated out when a constant current of 15.0 A is passed through aqueous NiCl₂ for 60.0 minutes?

How many electrons are transferred in the following reaction? (The reaction is unbalanced.) Ni(s) + Cr³⁺(aq) → Cr(s) + Ni²⁺(aq)

The electrolysis of molten AlCl₃ for 3.25 hr with an electrical current of 15.0 A produces ________ g of aluminum metal.

For a galvanic cell that uses the following two half-reactions, Cr₂O₇^2-(aq) + 14 H⁺(aq) + 6 e^- → 2 Cr³⁺(aq) + 7 H₂O(l) Sn(s) → Sn²⁺(aq) + 2 e^- How many moles of Sn(s) are oxidized by four moles of Cr₂O₇^2-?

How many kilowatt-hours of electricity are used to produce 3.00 kg of magnesium in the electrolysis of molten with an applied emf of 4.50 V?

Given that E°_red = -0.40 V for Cd²⁺/Cd at 25°C,find E° and E for the concentration cell expressed using shorthand notation below. Cd(s) ∣ Cd²⁺(1.0 × 10^-5 M) ∣∣ Cd²⁺(0.100 M) ∣ Cd(s)

A voltaic cell is constructed with two Zn²⁺-Zn electrodes,where the half-reaction is Zn²⁺ + 2e^- → Zn(s) E° = -0.763 V The concentrations of zinc ion in the two compartments are 5.50 M and 1.11 × 10^-2 M,respectively.The cell emf is ________ V.

Based on the following information, I₂(s) + 2 e^- → 2 I^-(aq) E° = +0.54 V Cd²⁺(aq) + 2 e^- → Cd (s) E° = -0.40 V Which of the following chemical species is the strongest reducing agent?

How many electrons are transferred in the following reaction? (The reaction is unbalanced.) Br₂(s) + Fe(s) → Fe³⁺(aq) + Br⁻(aq)

How many grams of chromium metal are plated out when a constant current of 8.00 A is passed through an aqueous solution containing Cr³⁺ ions for 320.minutes?

The most useful ore of aluminum is bauxite,in which Al is present as hydrated oxides,Al₂O₃ ∙ xH₂O.The number of kilowatt-hours of electricity required to produce 4.00 kg of aluminum from electrolysis of compounds from bauxite is ________ when the applied emf is 5.00 V.

A voltaic cell is constructed with two silver-silver chloride electrodes,where the half-reaction is AgCl(s) + e^- → Ag(s) + Cl^-(aq) E° = +0.222 V The concentrations of chloride ion in the two compartments are 0.0222 M and 2.22 M,respectively.The cell emf is ________ V.

Quiz 19: Electrochemistry

How many seconds are required to produce 4.00 g of aluminum metal from the electrolysis of molten with an electrical current of 12.0 A?

The standard emf for the cell using the overall cell reaction below is +2.20 V: 2 Al(s) + 3 I2(s) → 2 Al3+(aq) + 6 I-(aq) The emf generated by the cell when [Al3+] = 4.5 × 10-3 M and [ ] = 0.15 M is

The standard cell potential (E°) of a voltaic cell constructed using the cell reaction below is 0.76 V: Zn(s) + 2 H+(aq) → Zn2+(aq) + H2(g) With = 1.0 atm and [Zn2+] = 1.0 M,the cell potential is 0.66 V.The concentration of in the cathode compartment is ________ M.

The standard emf for the cell using the overall cell reaction below is +0.48 V: Zn(s) + Ni2+(aq) → Zn2+(aq) + Ni(s) The emf generated by the cell when [Ni2+] = 2.50 M and [Zn2+] = 0.100 M is

Which of the following reactions would be the most spontaneous at 298 K?

How many electrons are transferred in the following reaction? (The reaction is unbalanced.) Ni2+(aq) + Na(s) → Ni(s) + Na+(aq)

How many grams of nickel metal are plated out when a constant current of 15.0 A is passed through aqueous NiCl2 for 60.0 minutes?

How many electrons are transferred in the following reaction? (The reaction is unbalanced.) Ni(s) + Cr3+(aq) → Cr(s) + Ni2+(aq)

The electrolysis of molten AlCl3 for 3.25 hr with an electrical current of 15.0 A produces ________ g of aluminum metal.

For a galvanic cell that uses the following two half-reactions, Cr2O72-(aq) + 14 H+(aq) + 6 e- → 2 Cr3+(aq) + 7 H2O(l) Sn(s) → Sn2+(aq) + 2 e- How many moles of Sn(s) are oxidized by four moles of Cr2O72-?

How many kilowatt-hours of electricity are used to produce 3.00 kg of magnesium in the electrolysis of molten with an applied emf of 4.50 V?

Given that E°red = -0.40 V for Cd2+/Cd at 25°C,find E° and E for the concentration cell expressed using shorthand notation below. Cd(s) ∣ Cd2+(1.0 × 10-5 M) ∣∣ Cd2+(0.100 M) ∣ Cd(s)

A voltaic cell is constructed with two Zn2+-Zn electrodes,where the half-reaction is Zn2+ + 2e- → Zn(s) E° = -0.763 V The concentrations of zinc ion in the two compartments are 5.50 M and 1.11 × 10-2 M,respectively.The cell emf is ________ V.

Based on the following information, I2(s) + 2 e- → 2 I-(aq) E° = +0.54 V Cd2+(aq) + 2 e- → Cd (s) E° = -0.40 V Which of the following chemical species is the strongest reducing agent?

How many electrons are transferred in the following reaction? (The reaction is unbalanced.) Br2(s) + Fe(s) → Fe3+(aq) + Br⁻(aq)

How many grams of chromium metal are plated out when a constant current of 8.00 A is passed through an aqueous solution containing Cr3+ ions for 320.minutes?

The most useful ore of aluminum is bauxite,in which Al is present as hydrated oxides,Al2O3 ∙ xH2O.The number of kilowatt-hours of electricity required to produce 4.00 kg of aluminum from electrolysis of compounds from bauxite is ________ when the applied emf is 5.00 V.

A voltaic cell is constructed with two silver-silver chloride electrodes,where the half-reaction is AgCl(s) + e- → Ag(s) + Cl-(aq) E° = +0.222 V The concentrations of chloride ion in the two compartments are 0.0222 M and 2.22 M,respectively.The cell emf is ________ V.

The standard emf for the cell using the overall cell reaction below is +2.20 V: 2 Al(s) + 3 I₂(s) → 2 Al³⁺(aq) + 6 I^-(aq) The emf generated by the cell when [Al³⁺] = 4.5 × 10^-³ M and [ ] = 0.15 M is

The standard cell potential (E°) of a voltaic cell constructed using the cell reaction below is 0.76 V: Zn(s) + 2 H⁺(aq) → Zn²⁺(aq) + H₂(g) With = 1.0 atm and [Zn²⁺] = 1.0 M,the cell potential is 0.66 V.The concentration of in the cathode compartment is ________ M.

The standard emf for the cell using the overall cell reaction below is +0.48 V: Zn(s) + Ni²⁺(aq) → Zn²⁺(aq) + Ni(s) The emf generated by the cell when [Ni²⁺] = 2.50 M and [Zn²⁺] = 0.100 M is

How many electrons are transferred in the following reaction? (The reaction is unbalanced.) Ni²⁺(aq) + Na(s) → Ni(s) + Na⁺(aq)

How many grams of nickel metal are plated out when a constant current of 15.0 A is passed through aqueous NiCl₂ for 60.0 minutes?

How many electrons are transferred in the following reaction? (The reaction is unbalanced.) Ni(s) + Cr³⁺(aq) → Cr(s) + Ni²⁺(aq)

The electrolysis of molten AlCl₃ for 3.25 hr with an electrical current of 15.0 A produces ________ g of aluminum metal.

For a galvanic cell that uses the following two half-reactions, Cr₂O₇^2-(aq) + 14 H⁺(aq) + 6 e^- → 2 Cr³⁺(aq) + 7 H₂O(l) Sn(s) → Sn²⁺(aq) + 2 e^- How many moles of Sn(s) are oxidized by four moles of Cr₂O₇^2-?

Given that E°_red = -0.40 V for Cd²⁺/Cd at 25°C,find E° and E for the concentration cell expressed using shorthand notation below. Cd(s) ∣ Cd²⁺(1.0 × 10^-5 M) ∣∣ Cd²⁺(0.100 M) ∣ Cd(s)

A voltaic cell is constructed with two Zn²⁺-Zn electrodes,where the half-reaction is Zn²⁺ + 2e^- → Zn(s) E° = -0.763 V The concentrations of zinc ion in the two compartments are 5.50 M and 1.11 × 10^-2 M,respectively.The cell emf is ________ V.

Based on the following information, I₂(s) + 2 e^- → 2 I^-(aq) E° = +0.54 V Cd²⁺(aq) + 2 e^- → Cd (s) E° = -0.40 V Which of the following chemical species is the strongest reducing agent?

How many electrons are transferred in the following reaction? (The reaction is unbalanced.) Br₂(s) + Fe(s) → Fe³⁺(aq) + Br⁻(aq)

How many grams of chromium metal are plated out when a constant current of 8.00 A is passed through an aqueous solution containing Cr³⁺ ions for 320.minutes?

The most useful ore of aluminum is bauxite,in which Al is present as hydrated oxides,Al₂O₃ ∙ xH₂O.The number of kilowatt-hours of electricity required to produce 4.00 kg of aluminum from electrolysis of compounds from bauxite is ________ when the applied emf is 5.00 V.

A voltaic cell is constructed with two silver-silver chloride electrodes,where the half-reaction is AgCl(s) + e^- → Ag(s) + Cl^-(aq) E° = +0.222 V The concentrations of chloride ion in the two compartments are 0.0222 M and 2.22 M,respectively.The cell emf is ________ V.