Question 1

The standard cell potential (E°_cell)of the reaction below is -0.55 V. The value of ΔG° for the reaction is __________ J/mol. I₂ (s)+ 2Br^- (aq)→ 2I^- (aq)+ Br₂ (l)

Accepted Answer

The relationship between ΔG° and E° is given by the equation: 
ΔG° = -nF E° where n is the number of electrons transferred and F is Faraday's constant.
In this case, n = 2 because two electrons are transferred in the reaction. 
Substituting the given values, we get : 
ΔG° = -2 × 96485 × (-0.55) = 106458 J/mol 
Rounding off to the nearest integer, we get: 
ΔG° = 1.1 × 10^5 J/mol. 
Therefore, the correct choice is D.

Question 2

Corrosion of iron is retarded by __________.

Accepted Answer

Corrosion of iron is slowed down in high pH conditions because alkaline environments tend to form protective oxide layers on the iron, reducing its rate of corrosion.

Question 3

The standard cell potential (E°_cell)of the reaction below is +1.34 V. The value of ΔG° for the reaction is __________ kJ/mol. 3Cu (s)+ 2MnO₄^- (aq)+ 8H⁺ (aq)→ 3Cu²⁺ (aq)+ 2MnO₂ (s)+ 4H₂O (l)

Accepted Answer

The answer of The standard cell potential (E°_cell)of the reaction...

Question 4

The standard cell potential (E°_cell)for the voltaic cell based on the reaction below is __________ V. 3Sn⁴⁺ (aq)+ 2Cr (s)→ 2Cr³⁺ (aq)+ 3Sn²⁺ (aq)

Accepted Answer

To determine the standard cell potential (E°cell) for the given reaction, we need to use the standard reduction potentials for the half-reactions involved. 
The half-reactions are: 
Sn4+(aq) + 2e- → Sn2+(aq)      E° = +0.15 V 
Cr3+(aq) + e- → Cr2+(aq)        E° = -0.41 V 
We reverse the second half-reaction and multiply it by 2 to balance the electrons: 
Cr(s) → 2Cr3+(aq) + 6e-     E° = +0.82 V 
Now we add the two half-reactions to get the overall reaction and the standard potential for the cell: 
3Sn4+(aq) + 2Cr(s) → 2Cr3+(aq) + 3Sn2+(aq)         E°cell = +0.15 V + (+0.82 V) = +0.97 V 
Therefore, the standard cell potential for the given reaction is +0.97 V, which is closest to choice B (+0.89 V).

Question 5

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.

Question 6

The most useful ore of aluminum is bauxite, in which Al is present as hydrated oxides, Al₂O₃ × H₂O. 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. The molar mass of aluminum is 26.98 g/mol, so 4.00 kg of aluminum is approximately 148.3 moles. The total charge required is 3 times the number of moles of aluminum times Faraday's constant (96485 C/mol). The energy in kilowatt-hours is calculated using the formula: Energy (kWh) = (Charge in Coulombs × Voltage in Volts) / (3600 × 1000). Plugging in the values gives approximately 59.6 kWh.

Question 7

The standard cell potential (E°_cell)for the reaction below is +0.63 V. The cell potential for this reaction is __________ V when [Zn²⁺] = 3.5 M and [Pb²⁺] = 2.0 × 10^-4 M. Pb²⁺ (aq)+ Zn (s)→ Zn²⁺ (aq)+ Pb (s)

Accepted Answer

The Nernst equation is used to calculate the cell potential under non-standard conditions: E = E° - (RT/nF) * ln(Q). Here, E° = 0.63 V, n = 2, and Q = [Zn²⁺]/[Pb²⁺] = 3.5/(2.0 × 10⁻⁴). Plugging in these values and using R = 8.314 J/mol·K, T = 298 K, and F = 96485 C/mol, the calculated E is approximately 0.50 V.

Question 8

The lead-containing reactant(s)consumed during recharging of a lead-acid battery is/are __________.

Accepted Answer

The answer of The lead-containing reactant(s)consumed during recharging of a...

Question 9

The standard cell potential (E°_cell)of the reaction below is -0.34 V. The value of ΔG° for the reaction is __________ kJ/mol. Cu (s)+ 2H⁺ (aq)→ Cu²⁺ (aq)+ H₂ (g)

Accepted Answer

The answer of The standard cell potential (E°_cell)of the reaction...

Question 10

The standard cell potential (E°_cell)for the voltaic cell based on the reaction below is __________ V. 2Cr (s)+ 3Fe²⁺ (aq)→ 3Fe (s)+ 2Cr³⁺ (aq)

Accepted Answer

The answer of The standard cell potential (E°_cell)for the voltaic...

Question 11

The standard cell potential (E°_cell)for the reaction below is +1.10 V. The cell potential for this reaction is __________ V when the concentration of [Cu²⁺] = 1.0 × 10^-5 M and [Zn²⁺] = 3.5 M. Zn (s)+ Cu²⁺ (aq)→ Cu (s)+ Zn²⁺ (aq)

Accepted Answer

The cell potential can be calculated using the Nernst equation:
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 balanced equation, F is Faraday's constant, Q is the reaction quotient.
Firstly, calculate the value of Q
Q = ([Cu2+]/[Zn2+]) = ([1.0 × 10^-5]/[3.5]) = 2.86 × 10^-6
Next, substitute the given values:
Ecell = +1.10 - (0.0257/2)ln(2.86 × 10^-6)
Ecell = 0.94 V
Therefore, the best choice is C.

Question 12

Galvanized iron is iron coated with __________.

Accepted Answer

Galvanized iron is iron coated with zinc. This is done to protect the iron from rusting and corrosion. Magnesium, chromium, and phosphate are not commonly used to coat iron, and iron oxide is a form of rust that galvanization is meant to prevent.

Question 13

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 ________ V.

Accepted Answer

The Nernst equation is:E = E° - (RT/nF)ln(Q)where:E is the cell potential in voltsE° is the standard cell potential in voltsR is the ideal gas constant (8.314 J/mol·K)T is the temperature in Kelvinn is the number of moles of electrons transferred in the balanced chemical equationF is the Faraday constant (96,485 C/mol)Q is the reaction quotientIn this case, the balanced chemical equation is:Zn (s)+ Ni²⁺ (aq)→ Zn²⁺ (aq)+ Ni (s)and n = 2.Substituting the given values into the Nernst equation, we get:E = 0.48 V - (0.0257 V/K)(298 K)/2ln(0.100 M/2.50 M)E = 0.48 V - 0.039 VE = 0.52 VTherefore, the correct answer is C) 0.52 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

To calculate the cell EMF, we need to use the Nernst equation:

E = E° - (RT/nF) ln(Q)

where:
E° = -0.763 V (given)
R = 8.314 J/mol*K (gas constant)
T = 298 K (room temperature, 25°C)
n = 2 (because two electrons are transferred in the half-reaction)
F = 96,485 C/mol (Faraday constant)
Q = [Zn2+]cathode / [Zn2+]anode = (5.50 M) / (1.11 × 10^-2 M) = 4.95 × 10^2

Plugging in the values:

E = -0.763 V - (8.314 J/mol*K / (2 * 96,485 C/mol)) ln(4.95 × 10^2)
E ≈ 0.0798 V

Therefore, the answer is C: 0.0798.

Question 15

The standard cell potential (E°_cell)of the reaction below is +0.126 V. The value of ΔG° for the reaction is __________ kJ/mol. Pb (s)+ 2H⁺ (aq)→ Pb²⁺ (aq)+ H₂ (g)

Accepted Answer

The answer of The standard cell potential (E°_cell)of the reaction...

Question 16

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

Accepted Answer

To solve the problem, we can use the Nernst equation: E = E° - (RT/nF) × ln(Q) where: E° = standard emf = +2.20 V R = gas constant = 8.314 J/mol·K T = temperature in Kelvin n = moles of electrons transferred in the balanced equation (in this case, n = 6) F = Faraday's constant = 96,485 C/mol Q = reaction quotient = [Al³⁺]²/[I^-]³ Substituting the given values, we get: E = 2.20 - (8.314 × 298/6 × 96,485) × ln[(4.5 × 10⁻¹³)²/(0.15)³] E = 2.32 V Therefore, the answer is B) 2.32.

Question 17

The standard cell potential (E°_cell)for the voltaic cell based on the reaction below is __________ V. Cr (s)+ 3Fe³⁺ (aq)→ 3Fe²⁺ (aq)+ Cr³⁺ (aq)

Accepted Answer

To find the standard cell potential, we need to use the standard reduction potentials of each half-cell reaction. Looking at the reduction potentials table, we can find the reduction potentials for each half-reaction:

Cr3+(aq) + 3e- → Cr(s)   E° = -0.74 V
Fe3+(aq) + e- → Fe2+(aq)  E° = +0.77 V

To calculate the overall potential, we need to subtract the reduction potential of the anode from the reduction potential of the cathode:

E°cell = E°cathode - E°anode
E°cell = (+0.77 V) - (-0.74 V)
E°cell = +1.51 V

Therefore, the standard cell potential for this voltaic cell is +1.51 V, which corresponds to answer choice C.

Question 18

How many kilowatt-hours of electricity are used to produce 3.00 kg of magnesium in the electrolysis of molten MgCl₂ with an applied emf of 4.50 V?

Accepted Answer

To solve this problem, we need to use the equation:
energy = voltage x charge

We can find the charge by using the equation:
moles of electrons = moles of magnesium
moles of electrons = mass of magnesium / molar mass of magnesium * 2 (because Mg2+ gains two electrons)
moles of electrons = 3.00 kg / 24.31 g/mol * 2 = 0.246 mol of electrons

Charge = moles of electrons x Faraday's constant
Charge = 0.246 mol x 96,485 C/mol = 2.37 x 10^4 C

Now we can find the energy by plugging in the values:
energy = 4.50 V x 2.37 x 10^4 C
energy = 1.0665 x 10^5 J

To convert to kilowatt-hours, we need to divide by 3.6 x 10^6 J/kWh:
energy = 1.0665 x 10^5 J / 3.6 x 10^6 J/kWh
energy = 0.0296 kWh

Therefore, the answer is D) 29.8.

Question 19

The standard cell potential (E°)of a voltaic cell constructed using the cell reaction below is 0.76 V: Zn (s)+ 2H⁺ (aq)→ Zn²⁺ (aq)+ H₂ (g) With PH₂ = 1.0 atm and [Zn²⁺] = 1.0 M, the cell potential is 0.66 V. The concentration of H⁺ in the cathode compartment is __________ M.

Accepted Answer

The Nernst equation relates the cell potential to the concentrations of the reactants and products. Solving for [H⁺] using the given potentials and conditions, we find it to be 2.0 × 10⁻² M.

Question 20

The relationship between the change in Gibbs free energy and the emf of an electrochemical cell is given by __________.

Accepted Answer

The relationship between the change in Gibbs free energy (ΔG) and the emf (E) of an electrochemical cell is given by the equation ΔG = -nFE, where n is the number of moles of electrons transferred and F is the Faraday constant. This equation relates the thermodynamic property (ΔG) to the electrochemical property (E) of the cell.

Quiz 20: Electrochemistry

The standard cell potential (E°_cell) of the reaction below is -0.55 V. The value of ΔG° for the reaction is __________ J/mol. I₂ (s) + 2Br^- (aq) → 2I^- (aq) + Br₂ (l)

Corrosion of iron is retarded by __________.

The standard cell potential (E°_cell) of the reaction below is +1.34 V. The value of ΔG° for the reaction is __________ kJ/mol. 3Cu (s) + 2MnO₄^- (aq) + 8H⁺ (aq) → 3Cu²⁺ (aq) + 2MnO₂ (s) + 4H₂O (l)

The standard cell potential (E°_cell) for the voltaic cell based on the reaction below is __________ V. 3Sn⁴⁺ (aq) + 2Cr (s) → 2Cr³⁺ (aq) + 3Sn²⁺ (aq)

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 most useful ore of aluminum is bauxite, in which Al is present as hydrated oxides, Al₂O₃ × H₂O. 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.

The standard cell potential (E°_cell) for the reaction below is +0.63 V. The cell potential for this reaction is __________ V when [Zn²⁺] = 3.5 M and [Pb²⁺] = 2.0 × 10^-4 M. Pb²⁺ (aq) + Zn (s) → Zn²⁺ (aq) + Pb (s)

The lead-containing reactant(s) consumed during recharging of a lead-acid battery is/are __________.

The standard cell potential (E°_cell) of the reaction below is -0.34 V. The value of ΔG° for the reaction is __________ kJ/mol. Cu (s) + 2H⁺ (aq) → Cu²⁺ (aq) + H₂ (g)

The standard cell potential (E°_cell) for the voltaic cell based on the reaction below is __________ V. 2Cr (s) + 3Fe²⁺ (aq) → 3Fe (s) + 2Cr³⁺ (aq)

The standard cell potential (E°_cell) for the reaction below is +1.10 V. The cell potential for this reaction is __________ V when the concentration of [Cu²⁺] = 1.0 × 10^-5 M and [Zn²⁺] = 3.5 M. Zn (s) + Cu²⁺ (aq) → Cu (s) + Zn²⁺ (aq)

Galvanized iron is iron coated with __________.

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 ________ V.

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.

The standard cell potential (E°_cell) of the reaction below is +0.126 V. The value of ΔG° for the reaction is __________ kJ/mol. Pb (s) + 2H⁺ (aq) → Pb²⁺ (aq) + H₂ (g)

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

The standard cell potential (E°_cell) for the voltaic cell based on the reaction below is __________ V. Cr (s) + 3Fe³⁺ (aq) → 3Fe²⁺ (aq) + Cr³⁺ (aq)

How many kilowatt-hours of electricity are used to produce 3.00 kg of magnesium in the electrolysis of molten MgCl₂ with an applied emf of 4.50 V?

The standard cell potential (E°) of a voltaic cell constructed using the cell reaction below is 0.76 V: Zn (s) + 2H⁺ (aq) → Zn²⁺ (aq) + H₂ (g) With PH₂ = 1.0 atm and [Zn²⁺] = 1.0 M, the cell potential is 0.66 V. The concentration of H⁺ in the cathode compartment is __________ M.

The relationship between the change in Gibbs free energy and the emf of an electrochemical cell is given by __________.

Quiz 20: Electrochemistry

The standard cell potential (E°cell) of the reaction below is -0.55 V. The value of ΔG° for the reaction is __________ J/mol. I2 (s) + 2Br- (aq) → 2I- (aq) + Br2 (l)

Corrosion of iron is retarded by __________.

The standard cell potential (E°cell) of the reaction below is +1.34 V. The value of ΔG° for the reaction is __________ kJ/mol. 3Cu (s) + 2MnO4- (aq) + 8H+ (aq) → 3Cu2+ (aq) + 2MnO2 (s) + 4H2O (l)

The standard cell potential (E°cell) for the voltaic cell based on the reaction below is __________ V. 3Sn4+ (aq) + 2Cr (s) → 2Cr3+ (aq) + 3Sn2+ (aq)

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 most useful ore of aluminum is bauxite, in which Al is present as hydrated oxides, Al2O3 × H2O. 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.

The standard cell potential (E°cell) for the reaction below is +0.63 V. The cell potential for this reaction is __________ V when [Zn2+] = 3.5 M and [Pb2+] = 2.0 × 10-4 M. Pb2+ (aq) + Zn (s) → Zn2+ (aq) + Pb (s)

The lead-containing reactant(s) consumed during recharging of a lead-acid battery is/are __________.

The standard cell potential (E°cell) of the reaction below is -0.34 V. The value of ΔG° for the reaction is __________ kJ/mol. Cu (s) + 2H+ (aq) → Cu2+ (aq) + H2 (g)

The standard cell potential (E°cell) for the voltaic cell based on the reaction below is __________ V. 2Cr (s) + 3Fe2+ (aq) → 3Fe (s) + 2Cr3+ (aq)

The standard cell potential (E°cell) for the reaction below is +1.10 V. The cell potential for this reaction is __________ V when the concentration of [Cu2+] = 1.0 × 10-5 M and [Zn2+] = 3.5 M. Zn (s) + Cu2+ (aq) → Cu (s) + Zn2+ (aq)

Galvanized iron is iron coated with __________.

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 ________ V.

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.

The standard cell potential (E°cell) of the reaction below is +0.126 V. The value of ΔG° for the reaction is __________ kJ/mol. Pb (s) + 2H+ (aq) → Pb2+ (aq) + H2 (g)

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

The standard cell potential (E°cell) for the voltaic cell based on the reaction below is __________ V. Cr (s) + 3Fe3+ (aq) → 3Fe2+ (aq) + Cr3+ (aq)

How many kilowatt-hours of electricity are used to produce 3.00 kg of magnesium in the electrolysis of molten MgCl2 with an applied emf of 4.50 V?

The standard cell potential (E°) of a voltaic cell constructed using the cell reaction below is 0.76 V: Zn (s) + 2H+ (aq) → Zn2+ (aq) + H2 (g) With PH2 = 1.0 atm and [Zn2+] = 1.0 M, the cell potential is 0.66 V. The concentration of H+ in the cathode compartment is __________ M.

The relationship between the change in Gibbs free energy and the emf of an electrochemical cell is given by __________.

The standard cell potential (E°_cell) of the reaction below is -0.55 V. The value of ΔG° for the reaction is __________ J/mol. I₂ (s) + 2Br^- (aq) → 2I^- (aq) + Br₂ (l)

The standard cell potential (E°_cell) of the reaction below is +1.34 V. The value of ΔG° for the reaction is __________ kJ/mol. 3Cu (s) + 2MnO₄^- (aq) + 8H⁺ (aq) → 3Cu²⁺ (aq) + 2MnO₂ (s) + 4H₂O (l)

The standard cell potential (E°_cell) for the voltaic cell based on the reaction below is __________ V. 3Sn⁴⁺ (aq) + 2Cr (s) → 2Cr³⁺ (aq) + 3Sn²⁺ (aq)

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 most useful ore of aluminum is bauxite, in which Al is present as hydrated oxides, Al₂O₃ × H₂O. 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.

The standard cell potential (E°_cell) for the reaction below is +0.63 V. The cell potential for this reaction is __________ V when [Zn²⁺] = 3.5 M and [Pb²⁺] = 2.0 × 10^-4 M. Pb²⁺ (aq) + Zn (s) → Zn²⁺ (aq) + Pb (s)

The standard cell potential (E°_cell) of the reaction below is -0.34 V. The value of ΔG° for the reaction is __________ kJ/mol. Cu (s) + 2H⁺ (aq) → Cu²⁺ (aq) + H₂ (g)

The standard cell potential (E°_cell) for the voltaic cell based on the reaction below is __________ V. 2Cr (s) + 3Fe²⁺ (aq) → 3Fe (s) + 2Cr³⁺ (aq)

The standard cell potential (E°_cell) for the reaction below is +1.10 V. The cell potential for this reaction is __________ V when the concentration of [Cu²⁺] = 1.0 × 10^-5 M and [Zn²⁺] = 3.5 M. Zn (s) + Cu²⁺ (aq) → Cu (s) + Zn²⁺ (aq)

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 ________ V.

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.

The standard cell potential (E°_cell) of the reaction below is +0.126 V. The value of ΔG° for the reaction is __________ kJ/mol. Pb (s) + 2H⁺ (aq) → Pb²⁺ (aq) + H₂ (g)

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

The standard cell potential (E°_cell) for the voltaic cell based on the reaction below is __________ V. Cr (s) + 3Fe³⁺ (aq) → 3Fe²⁺ (aq) + Cr³⁺ (aq)

How many kilowatt-hours of electricity are used to produce 3.00 kg of magnesium in the electrolysis of molten MgCl₂ with an applied emf of 4.50 V?

The standard cell potential (E°) of a voltaic cell constructed using the cell reaction below is 0.76 V: Zn (s) + 2H⁺ (aq) → Zn²⁺ (aq) + H₂ (g) With PH₂ = 1.0 atm and [Zn²⁺] = 1.0 M, the cell potential is 0.66 V. The concentration of H⁺ in the cathode compartment is __________ M.