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Exam 3 hw

Marks: 1

The ___________ is outside of the region of focus and includes everything but the region of focus.

Choose one answer.

	A. surroundings
	B. system
	C. universe

Question

Marks: 1

The ___________ is the region of focus (usually where the reaction is occuring).

Choose one answer.

	A. system
	B. surroundings
	C. universe

Question

Marks: 1

How much heat (in kJ) is evolved (under standard conditions) when 191.78 g of copper reacts to form copper(II) oxide?

Answer:

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Marks: 1

What is the change in enthalpy (in kJ) under standard conditions when 11.22 g of benzene is combusted?

Answer:

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What is the change in enthalpy (in kJ) under standard conditions when 245.02 g of sodium sulfate dissolves in water?

Answer:

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What mass (in g) of aluminum is needed to evolve 1026.2 kJ of heat under standard conditions as it forms aluminum oxide?

Answer:

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What mass (in g) of iron is needed to evolve 913.6 kJ of heat under standard conditions as it forms iron(III) oxide?

Answer:

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Marks: 1

A system which allows for an transfer of energy but not matter is

Choose one answer.

	A. closed.
	B. open.
	C. isolated.

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Marks: 1

A system which does not allow for an transfer of matter or energy is

Choose one answer.

	A. isolated.
	B. closed.
	C. open.

Question

Marks: 1

What is the enthalpy of combustion (in kJ/mol) for acetone (CH3COCH3) under standard conditions (water is produced as a liquid)? Use the appendix in your textbook, do not enter units, and answer with 5 significant digits.

Answer:

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Marks: 1

What is the enthalpy of combustion (in kJ/mol) for carbon under standard conditions? Use the appendix in your textbook, do not enter units, and answer with 4 significant digits.

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Marks: 1

What is the enthalpy of formation of butane (C4H10) if the enthalpy of combustion for butane is -2876.9 kJ/mol (water is produced as a liquid)? Use the appendix in your textbook, do not enter units, and answer with 3 significant digits.

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Marks: 1

What is the sum of the stoichimetric coefficients for the formation reaction of magnesium carbonate? Enter any fraction as a decimal (to two significant digits).

Answer:

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What is the sum of the stoichiometric coefficients the formation reaction for methanol (CH3OH)? Enter any fraction as a decimal.

Answer:

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Marks: 1

What is the coefficient for oxygen in the formation reaction for methanol (CH3OH)? Enter any fraction as a decimal.

Answer:

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Marks: 1

What is the enthalpy of combustion (in kJ/mol) for methanol (CH3OH) under standard conditions (water is produced as a liquid)? Use the appendix in your textbook, do not enter units, and answer with 4 significant digits.

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Marks: 1

What is the enthalpy of formation of propylene (C3H6) if the enthalpy of combustion for propylene is -2058.3 kJ/mol (water is produced as a liquid)? Use the appendix in your textbook, do not enter units, and answer with 3 significant digits.

Answer:

Question

Marks: 1

Which processes are spontaneous?

Choose at least one answer.

	a. dissolved sodium chloride in water forming solid sodium chloride
	b. solid sodium chloride dissolving in water
	c. dissolved sugar in water forming solid sugar
	d. solid sugar dissolving in water

Question

Marks: 1

How many different ways can four particles be placed in two different (equally probable) containers?

Answer:

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Marks: 1

Using Appendix 2 in your textbook, what is the standard change in entropy (in J/K) at 25oC of the reaction:

2C6H6(l) + 15O2(g) --> 12CO2(g) + 6H2O(l)?

Answer:

Marks: 1

Using Appendix 2 in your textbook, what is the standard change in entropy (in J/K) at 25oC of the reaction:

2NO(g) + N2(g) --> 2N2O(g)?

Answer:

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Marks: 1

Using Appendix 2 in your textbook, what is the standard change in entropy (in J/K) at 25oC of the reaction:

2O3(g) --> 3O2(g)?

Answer:

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Marks: 1

What is the sign on the change in entropy for the process: 2N2(g) + O2(g)--> 2N2O(g)

Choose one answer.

	a. entropy is increasing
	b. entropy is unchanged
	c. entropy is decreasing
	d. entropy cannot be approximated

Question

Marks: 1

What is the sign on the change in entropy for the process: 2N2O5(g)--> 4NO2(g) + O2(g)

Choose one answer.

	a. entropy is increasing
	b. entropy is unchanged
	c. entropy is decreasing
	d. entropy cannot be approximated

Question

Marks: 1

What is the sign on the change in entropy for the process: Cgraphite(s) at 0oC --> Cgraphite(s) at 25oC

Choose one answer.

	a. entropy is increasing
	b. entropy is unchanged
	c. entropy is decreasing
	d. entropy cannot be approximated

Question

Marks: 1

What is the sign on the change in entropy for the process: H2O(g) --> H2O(l)

Choose one answer.

	a. entropy is increasing
	b. entropy is unchanged
	c. entropy is decreasing
	d. entropy cannot be approximated

Question

Marks: 1

What is the sign on the change in entropy for the process: KBr(s) --> K+(aq) + Br-(aq)

Choose one answer.

	a. entropy is increasing
	b. entropy is unchanged
	c. entropy is decreasing
	d. entropy cannot be approximated

Question

Marks: 1

What is the sign on the change in entropy for the process: PCl5(g) --> PCl3(g) + Cl2(g)

Choose one answer.

	a. entropy is increasing
	b. entropy is unchanged
	c. entropy is decreasing
	d. entropy cannot be approximated

Question

Marks: 1

What is the order of the lowest entropy (1 = lowest) to highest entropy (3 = highest)?

H2O(g)

Choose...	1 = lowest	3 = highest	2 = moderate
H2O(l)	Choose...	1 = lowest	3 = highest	2 = moderate
H2O(s)	Choose...	1 = lowest	3 = highest	2 = moderate

Question

Marks: 1

What is the order of the lowest entropy (1 = lowest) to highest entropy (3 = highest)?

Br2(g)

Choose...	3 = highest	1 = lowest	2 = moderate
Cl2(g)	Choose...	3 = highest	1 = lowest	2 = moderate
F2(g)	Choose...	3 = highest	1 = lowest	2 = moderate

Question

Marks: 1

What is the order of the lowest entropy (1 = lowest) to highest entropy (3 = highest)?

C2H4(g)

Choose...	3 = highest	2 = moderate	1 = lowest
C3H6(g)	Choose...	3 = highest	2 = moderate	1 = lowest
C4H8(g)	Choose...	3 = highest	2 = moderate	1 = lowest

Question

Marks: 1

What combination will always result in a spontaneous process?

Choose one answer.

	a. The entropy of the system increases and the entropy of the surroundings decreases.
	b. The entropy of the system decreases but the entropy of the surroundings increases.
	c. The entropy of the system increases but the entropy of the surroundings decreases.
	d. The entropy of the system increases and the entropy of the surroundings increases.

Question

Marks: 1

What is the second law of thermodynamics?

Choose one answer.

	a. The entropy of the universe is constant for a spontaneous process.
	b. The entropy of the universe increases for a spontaneous process.
	c. The entropy of the universe decreases for a spontaneous process.
	d. The entropy of the universe is zero for a spontaneous process.

Question

Marks: 1

What will result is a process being spontaneous?

(More than one answer can be correct - each correct answer will result in full credit)

Choose one answer.

	a. Both the change in entropy of the system and the change in entropy of the surroundings are greater than zero.
	b. Both the change in entropy of the system and the change in entropy of the surroundings are less than zero.
	c. The change in entropy of the system is greater than zero while the change in entropy of the surroundings is less than zero and the change in entropy of the system is greater in magnitude than the change in entropy of the surroundings.
	d. The change in entropy of the system is greater than zero while the change in entropy of the surroundings is less than zero and the change in entropy of the system is lower in magnitude than the change in entropy of the surroundings.

Question

Marks: 1

Which describes an endothermic system in which the entropy of the universe is increasing (spontaneous)?

Choose one answer.

	a. Enthalpy of the surroundings decreases and the entropy of the system decreases
	b. Enthalpy of the surroundings decreases and the entropy of the system increases
	c. Enthalpy of the surroundings increases and the entropy of the system decreases
	d. Enthalpy of the surroundings increases and the entropy of the system increases

Question

Marks: 1

For the reaction, 2CO(g) + O2(g) --> 2CO2(g), which statement is true?

Choose one answer.

	a. This reaction is always spontaneous.
	b. This reaction is never spontaneous.
	c. This reaction is spontaneous at low temperatures and not spontaneous at high temperatures.
	d. This reaction is not spontaneous at low temperatures and spontaneous at high temperatures.

Question

Marks: 1

Using Appendix 2 in your textbook, at what temperature (in K) will the reaction, 2CO(g) + O2(g) --> 2CO2(g), change in spontaneity?

Assume standard change in enthalpy and standard change in entropy do not change with temperature.

Answer:

Question

Marks: 1

Using Appendix 2 in your textbook, what is the value for the standard change in Gibbs free energy (in kJ) at 25oC of the reaction:

2C6H6(l) + 15O2(g) --> 12CO2(g) + 6H2O(l)?

Answer:

Question

Marks: 1

Using Appendix 2 in your textbook, what is the value for the standard change in Gibbs free energy (in kJ) at 25oC of the reaction:

2NO(g) + N2(g) --> 2N2O(g)?

Answer:

Question

Marks: 1

Using Appendix 2 in your textbook, what is the value for the standard change in Gibbs free energy (in kJ) at 25oC of the reaction:

2O3(g) --> 3O2(g)?

Answer:

Marks: 1

Using Appendix 2 in your textbook, what is the value for the standard change in Gibbs free energy (in kJ) at 25oC of the reaction:

C2H4(g) + H2(g) --> C2H6(g)?

Answer:

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Marks: 1

What is the value for the standard change in Gibbs free energy (in kJ), when the standard change in enthalpy is (-571.8) kJ and the standard change in entropy is (-149.73) J/K at 25oC?

Answer:

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Marks: 1

What is the value for the standard change in Gibbs free energy (in kJ), when the standard change in enthalpy is 559.7 kJ and the standard change in entropy is 130.62 J/K at 25oC?

Answer:

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Marks: 1

Which combination will result in a system that is always spontaneous?

Choose one answer.

	a. ΔHsys< 0 and ΔSsys< 0
	b. ΔHsys< 0 and ΔSsys > 0
	c. ΔHsys > 0 and ΔSsys< 0
	d. ΔHsys > 0 and ΔSsys > 0

Question

Marks: 1

Which combination will result in a system that is never spontaneous?

Choose one answer.

	a. ΔHsys< 0 and ΔSsys< 0
	b. ΔHsys< 0 and ΔSsys > 0
	c. ΔHsys > 0 and ΔSsys< 0
	d. ΔHsys > 0 and ΔSsys > 0

Question

Marks: 1

Which combination will result in a system that is spontaneous at high temperatures only?

Choose one answer.

	a. ΔHsys< 0 and ΔSsys< 0
	b. ΔHsys< 0 and ΔSsys > 0
	c. ΔHsys > 0 and ΔSsys< 0
	d. ΔHsys > 0 and ΔSsys > 0

Question

Marks: 1

Which combination will result in a system that is spontaneous at low temperatures only?

Choose one answer.

	a. ΔHsys< 0 and ΔSsys< 0
	b. ΔHsys< 0 and ΔSsys > 0
	c. ΔHsys > 0 and ΔSsys< 0
	d. ΔHsys > 0 and ΔSsys > 0

Question

Marks: 1

Given the Ka of benzoic acid from Chapter 16 in your textbook, what is the value of change in Gibbs free energy (in kJ/mol) at 25oC for this process?

Answer:

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Marks: 1

Given the Kb of urea from Chapter 16 in your textbook, what is the value of change in Gibbs free energy (in kJ/mol) at 25oC for this process?

Answer:

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Marks: 1

Given the Ksp of cobalt(II) sulfide from Chapter 17 in your textbook, what is the value of change in Gibbs free energy (in kJ/mol) at 25oC for this process?

Answer:

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Marks: 1

Given the Kw of water from Chapter 16 in your textbook, what is the value of change in Gibbs free energy (in kJ/mol) at 25oC for this process?

Answer:

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Marks: 1

What is true for a spontaneous process?

Choose one answer.

	a. ΔGsys< 0 and K < 1
	b. ΔGsys > 0 and K < 1
	c. ΔGsys< 0 and K > 1
	d. ΔGsys > 0 and K > 1

Question

Marks: 1

When ΔGo > 0 and Q > K,

Choose one answer.

	a. ΔG > 0 and the reaction will shift to the right.
	b. ΔG > 0 and the reaction will shift to the left.
	c. ΔG < 0 and the reaction will shift to the right.
	d. ΔG < 0 and the reaction will shift to the left.

Question

Marks: 1

When ΔGo < 0 and Q < K,

Choose one answer.

	a. ΔG > 0 and the reaction will shift to the right.
	b. ΔG > 0 and the reaction will shift to the left.
	c. ΔG < 0 and the reaction will shift to the right.
	d. ΔG < 0 and the reaction will shift to the left.

Question

Marks: 1

When ΔGo < 0 and the system is at equilibrium,

Choose one answer.

	a. ΔG = 0 and Q = K.
	b. ΔG = 0 and Q = 0.
	c. ΔG = ΔGo and Q = K.
	d. ΔG = ΔGo and Q = 0.

Question

Marks: 1

In the reaction of bromine with potassium iodide to produce potassium bromide and iodine, what is reduced and what is the reducing agent?

Choose one answer.

	A. bromine is reduced and potassium iodide is the reducing agent
	B. bromine is reduced and bromine is the reducing agent
	C. iodine is reduced and potassium iodide is the reducing agent
	D. iodine is reduced and bromine is the reducing agent
	E. potassium is reduced and potassium iodide is the reducing agent
	F. potassium is reduced and bromine is the reducing agent

Question

Marks: 1

In the reaction of sodium with water to produce sodium hydroxide and hydrogen gas, what is reduced and what is the reducing agent?

Choose one answer.

	A. hydrogen is reduced and sodium is the reducing agent
	B. hydrogen is reduced and water is the reducing agent
	C. sodium is reduced and sodium is the reducing agent
	D. sodium is reduced and water is the reducing agent
	E. oxygen is reduced and sodium is the reducing agent
	F. oxygen is reduced and water is the reducing agent

Question

Marks: 1

In which reaction is iron reduced?

Choose one answer.

	A. iron(III) oxide reacting with carbon monoxide to form liquid iron and carbon dioxide
	B. iron(II) chloride reacting with potassium nitrate and hydrochloric acid to form nitric oxide (NO), iron(III) chloride, potassium chloride and water
	C. iron(II) nitrate reacting with sodium hydroxide to form iron(II) hydroxide and sodium nitrate
	D. iron reacting with nitric acid to form iron(II) nitrate and hydrogen gas
	E. iron reacting with nickel(II) chloride to form iron(II) chloride and nickel
	F. iron(III) acetate reacting with potassium sulfide to form iron(III) sulfide and potassium acetate

Question

Marks: 1

In which reaction is nitrogen reduced?

Choose one answer.

	A. iron(II) chloride reacting with potassium nitrate and hydrochloric acid to form nitric oxide (NO), iron(III) chloride, potassium chloride and water
	B. nitrogen reacting with hydrogen to form ammonia
	C. copper(II) nitrate reacting with potassium sulfide to form the precipitate copper(II) sulfide and aqueous potassium nitrate
	D. nitrous acid reacting with potassium hydroxide to form potassium nitrite and water
	E. iron reacting with nitric acid to form iron(II) nitrate and hydrogen gas
	F. iron(II) nitrate reacting with sodium hydroxide to form iron(II) hydroxide and sodium nitrate

Question

Marks: 1

Which reactions are redox reactions?

Choose at least one answer.

	A. hydrochloric acid reacting with nickel metal to form hydrogen gas and aqueous nickel(II) chloride
	B. sodium bromide reacting with chlorine to form sodium chloride and bromine
	C. sodium hydroxide reacting with aluminum chloride to form solid aluminum hydroxide and sodium chloride
	D. sodium hydroxide reacting with hydrochloric acid to form water and sodium chloride
	E. sodium hydroxide reacting with potassium to form potassium hydroxide and sodium
	F. acetic acid reacting with sodium bicarbonate to form carbon dioxide, water and sodium acetate

Marks: 1

Which substance is the strongest oxidizing agent?

Choose one answer.

	A. Ag+
	B. Sn2+
	C. Ni2+
	D. Fe2+
	E. Cr3+
	F. Na+

Question

Marks: 1

Which substance is the strongest reducing agent?

Choose one answer.

	A. Mg
	B. Al
	C. Cd
	D. Fe
	E. Pb
	F. H2

Question

Marks: 1

How many electrons are transferred in the redox reaction taking place in acidic solution:

Sn2+(aq) + Cr2O72-(aq) --> Cr3+(aq) + Sn4+(aq)?

Answer:

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Marks: 1

How many electrons are transferred in the redox reaction taking place in basic solution:

Cr(s) + ClO4-(aq) --> ClO3-(aq) + Cr3+(aq)?

Answer:

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Marks: 1

How many electrons are transferred in the redox reaction:

Pb2+(aq) + Ni(s) --> Pb(s) + Ni2+(aq)?

Answer:

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Marks: 1

How many electrons are transferred in the redox reaction:

Zn(s) + Fe3+(aq) --> Zn2+(aq) + Fe(s)?

Answer:

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Marks: 1

What is the stoichiometric coefficient for the hydrogen ion in the balanced redox reaction of:

Cl-(aq) + NO3-(aq) --> NO(g) + Cl2(g) when balanced in acidic solution?

Answer:

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Marks: 1

What is the stoichiometric coefficient for the hydrogen ion in the balanced redox reaction of:

Zn(s) + NO3-(aq) --> NO2(g) + Zn2+(aq) when balanced in acidic solution?

Answer:

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Marks: 1

What is the stoichiometric coefficient for the hydroxide ion in the balanced redox reaction of:

In+(aq) + ClO-(aq) --> Cl-(aq) + In3+(aq) when balanced in basic solution?

Answer:

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Marks: 1

What is the stoichiometric coefficient for the hydroxide ion in the balanced redox reaction of:

Cr(s) + ClO4-(aq) --> ClO3-(aq) + Cr3+(aq) when balanced in basic solution?

Answer:

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Marks: 1

What is the stoichiometric coefficient for the hydroxide ion in the balanced redox reaction of:

Na(s) + H2O(l) --> Na+(aq) + H2(g) when balanced in basic solution?

Answer:

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Marks: 1

What is the stoichiometric coefficient for the substance oxidized (as a reactant) in the balanced redox reaction of:

Fe(s) + MnO4-(aq) --> Mn2+(aq) + Fe3+(aq) when balanced in acidic solution?

Answer:

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Marks: 1

What is the stoichiometric coefficient for the substance oxidized (as a reactant) in the balanced redox reaction of:

Pb(s) + MnO42-(aq) --> MnO2(s) + Pb2+(aq) when balanced in basic solution?

Answer:

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Marks: 1

What is the stoichiometric coefficient for the substance reduced (as a reactant) in the balanced redox reaction of:

Fe(s) + MnO4-(aq) --> Mn2+(aq) + Fe3+(aq) when balanced in acidic solution?

Answer:

Question

Marks: 1

What is the stoichiometric coefficient for the substance reduced (as a reactant) in the balanced redox reaction of:

Pb(s) + MnO42-(aq) --> MnO2(s) + Pb2+(aq) when balanced in basic solution?

Answer:

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Marks: 1

What is the stoichiometric coefficient for water in the balanced redox reaction of:

In+(aq) + ClO-(aq) --> Cl-(aq) + In3+(aq) when balanced in basic solution?

Answer:

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Marks: 1

What is the stoichiometric coefficient for water in the balanced redox reaction of:

Cr(s) + ClO4-(aq) --> ClO3-(aq) + Cr3+(aq) when balanced in basic solution?

Answer:

Question

A galvanic cell consists of a iron electrode in 1.0 M Fe(NO3)2 and a copper electrode in 1.0 M Cu(NO3)2. What is the standard cell potential (emf, in V) of this cell at 25oC?

Answer:

Question

A galvanic cell consists of a lead electrode in 1.0 M Pb(NO3)2 and a aluminum electrode in 1.0 M Al(NO3)3. What is the standard cell potential (emf, in V) of this cell at 25oC?

Answer:

Question

A galvanic cell consists of a lead electrode in 1.0 M Pb(NO3)2 and a aluminum electrode in 1.0 M Al(NO3)3. What is the standard Gibbs free energy (in kJ) of this cell at 25oC?

Answer:

A galvanic cell consists of a silver electrode in 1.0 M AgNO3 and a chromium electrode in 1.0 M Cr(NO3)3. What is the standard Gibbs free energy (in kJ) of this cell at 25oC?

Answer:

Question

A galvanic cell consists of a tin electrode in 1.0 M Sn(NO3)2 and a cadmium electrode in 1.0 M Cd(NO3)2. What is the standard cell potential (emf, in V) of this cell at 25oC?

Answer:

Question

A galvanic cell consists of a zinc electrode in 1.0 M Zn(NO3)2 and a nickel electrode in 1.0 M Ni(NO3)2. What is the standard cell potential (emf, in V) of this cell at 25oC?

Answer:

Question

For a galvanic cell,

Choose one answer.

	a. Eo > 0.
	b. Eo = 0.
	c. Eo< 0.
	d. Eo cannot be approximated.

Question

For a galvanic cell, Eo equals

Choose one answer.

	a. Eocathode - Eoanode, where each value is the standard reduction potential
	b. Eoanode - Eocathode, where each value is the standard reduction potential
	c. Eocathode + Eoanode, where each value is the standard reduction potential
	d. Eoanode * Eocathode, where each value is the standard reduction potential

Question

What direction do the electrons and the cations flow in a galvanic cell?

Choose one answer.

	a. the electrons flow from the cathode to the anode and the cations flow from the oxidation half-reaction to the reduction half-reaction to charge balance
	b. the electrons flow from the anode to the cathode and the cations flow from the oxidation half-reaction to the reduction half-reaction to charge balance
	c. the electrons flow from the cathode to the anode and the cations flow from the reduction half-reaction to the oxidation half-reaction to charge balance
	d. the electrons flow from the anode to the cathode and the cations flow from the reduction half-reaction to the oxidation half-reaction to charge balance

Question

What is the standard cell potential (emf, in V) of this cell at 25oC?

Cr |Cr3+ (1.0 M) ǁ H2SO4 (1 M) |SO2 (1 atm) |Pt(s)

Answer:

Question

What is the standard cell potential (emf, in V) of this cell at 25oC?

Mn | Mn2+(1.0 M) ǁ H2SO4 (1 M) |SO2 (1 atm) |Pt(s)

Answer:

Question

What is the standard Gibbs free energy (in kJ) of this cell at 25oC?

Cr |Cr3+ (1.0 M) ǁ H2SO4 (1 M) |SO2 (1 atm) |Pt(s)

Answer:

Question

What is the standard Gibbs free energy (in kJ) of this cell at 25oC?

Mn | Mn2+(1.0 M) ǁ H2SO4 (1 M) |SO2 (1 atm) |Pt(s)

Answer:

Question

What occurs at the anode?

Choose one answer.

	a. oxidation and electrons are consumed
	b. oxidation and electrons are produced
	c. reduction and electrons are consumed
	d. reduction and electrons are produced

Question

What occurs at the cathode?

Choose one answer.

	a. oxidation and electrons are consumed
	b. oxidation and electrons are produced
	c. reduction and electrons are consumed
	d. reduction and electrons are produced

Question

A galvanic cell consists of a iron electrode in 1 M Fe(NO3)2 and a copper electrode in 1 M Cu(NO3)2. What is the equilibrium constant for this reaction at 25oC?

Enter you answer with 2 significant digits, using the syntax of "1.0x10(22)" for "1.0x1022"

Answer:

Question

For a galvanic cell,

Choose one answer.

	a. Eo > 0 and ΔGo > 0.
	b. Eo > 0 and ΔGo< 0.
	c. Eo< 0 and ΔGo > 0.
	d. Eo< 0 and ΔGo< 0.

Question

Which reaction is not spontaneous under standard conditions?

Choose one answer.

	a. Co(s) + H2O(l) --> Co2+(aq) + H2(g)
	b. Na(s) + H2O(l) --> Na+(aq) + H2(g)
	c. Sn(s) + H2O(l) --> Sn2+(aq) + H2(g)
	d. Zn(s) + H2O(l) --> Zn2+(aq) + H2(g)

Question

A galvanic cell consists of a iron electrode in 0.0412 M Fe(NO3)2 and a copper electrode in 0.275 M Cu(NO3)2. What is the cell potential (emf, in V) of this cell at 25oC?

Answer:

Question

A galvanic cell consists of a zinc electrode in 0.0270 M Zn(NO3)2 and a nickel electrode in 0.321 M Ni(NO3)2. What is the cell potential (emf, in V) of this cell at 25oC?

Answer:

Question

What is the cell potential (emf, in V) of this cell at 25oC?

Cu |Cu2+ (0.0359 M) ǁ Br2 |Br- (0.525 M)

Answer:

Question

What mass (in g) of aluminum can be electroplated when 0.430 amps are used for 1.021 hours using a solution of aluminum nitrate?

Answer:

Question

100

What mass (in g) of silver can be electroplated when 0.966 amps are used for 1.079 hours using a solution of silver nitrate?

Answer: