Cu 2+ (aq) + Zn(s) → Cu(s) + Zn 2+ (aq) E⁰ cell = +1.10V Which of the following is true for the reaction shown? Select ALL that apply.

The equilibrium constant, K eq , is greater than 1.

The Gibbs Free Energy, ΔG, is negative.

If the concentration of Cr(NO 3 ) 3 is decreased from 1.0M to 0.1M at 25°C, does the cell voltage increase, decrease, or remain the same?

0.00V < E cell < +2.31V Q > 1 ∴ E cell DECREASES

E cell = +2.31V Q = 1 ∴ E cell SAME

E cell > +2.31V Q < 1 ∴ E cell INCREASES

If the concentration of Cr(NO 3 ) 3 is decreased from 1.0M to 0.1M, would the nonstandard cell power the device for the same time, a longer time, or a shorter time as compared with the standard cell? Justify your answer.

Shorter time. There is less reactant Cr 3+ in the nonstandard cell and will be used up more quickly.

Longer time. There is more reactant Cr 3+ in the nonstandard cell and will be used up less quickly.

Same time. The amount of time a cell runs is independent of the reactant concentrations.

If the concentration of Cr(NO 3 ) 3 is increased from 1.0M to 2.0M, would the nonstandard cell power the device for the same time, a longer time, or a shorter time as compared with the standard cell? Justify your answer.

Longer time. There is more reactant Cr 3+ in the nonstandard cell and will be used up less quickly.

Shorter time. There is less reactant Cr 3+ in the nonstandard cell and will be used up more quickly.

Same time. The amount of time a cell runs is independent of the reactant concentrations.

If the concentration of LiNO 3 is decreased from 1.0M to 0.1M at 25°C, does the cell voltage increase, decrease, or remain the same?

E cell > +2.31V Q < 1 ∴ E cell INCREASES

E cell = +2.31V Q = 1 ∴ E cell SAME

0.00V < E cell < +2.31V Q > 1 ∴ E cell DECREASES

If the half-cell containing 1.00 M Zn(NO 3 ) 2 (aq) in cells 1 and 3 is replaced with a half-cell containing 2.00M Zn(NO 3 ) 2 (aq), what will be the effect on the voltage of the two cells?

The voltage will decrease in cell 1 and increase in cell 3.

The voltage will increase in both cells.

The voltage will decrease in both cells.

The voltage will increase in cell 1 and decrease in cell 3.

In cells 1 and 3, which of the following takes place in half-cell Y?

Oxidation occurs in cell 1, and reduction occurs in cell 3.

Oxidation occurs in both cell 1 and cell 3.

Reduction occurs in both cell 1 and cell 3.

Reduction occurs in cell 1, and oxidation occurs in cell 3.

In the electrolytic refining of a metal, M, which of the following statements is correct?

The impure sample is the anode, and the pure metal is the cathode.

The pure metal is used as the anode, and the impure sample is the cathode.

Both the anode and cathode are pure sheets of the metal.

Both the anode and cathode are impure samples of the metal.

Based on the diagram shown select statement(s) that are correct. SELECT ALL THAT APPLY

The electrons are moving from the Sn electrode to the Cu electrode.

The potassium ions are moving into the cell where reduction is occurring.

Cu(s) + 4Cl⁻(aq) → CuCl₄²⁻(aq) + 2e⁻ Which of the following occurs in the reaction above?

Copper is oxidized from 0 to +2.

Copper is reduced from +2 to 0.

Copper is oxidized from +4 to 0.

Copper is oxidized from 0 to +4.

2 H 2 O(l) → O 2 (g) + 4 H + (aq) + 4 e – 4 H 2 O(l) + 4 e – → 2H 2 (g) + 4 OH – (aq) Which of the following best explains the difference in the water levels inside the two test tubes for the electrolysis of water? Which half reaction occurs at the cathode?

According to the balanced equation, twice as much H 2 as O 2 is produced. 2 H 2 O(l) + 4 e – → 2H 2 (g) + 4 OH – (aq)

According to the balanced equation, half as much H 2 as O 2 is produced. 2 H 2 O(l) + 4 e – → 2H 2 (g) + 4 OH – (aq)

According to the balanced equation, twice as much H 2 as O 2 is produced. 2 H 2 O(l) → O 2 (g) + 4 H + (aq) + 4 e –

According to the balanced equation, half as much H 2 as O 2 is produced. 2 H 2 O(l) → O 2 (g) + 4 H + (aq) + 4 e –

AP CHEM Unit 3 In Class Review

Quiz

•

Chemistry

•

11th Grade - University

•

Practice Problem

•

Medium

•

NGSS

HS-PS1-2, HS-PS1-7, HS-PS1-5

Standards-aligned

Patrick Boylan

Used 364+ times

FREE Resource

Student preview

26 questions

Show all answers

MULTIPLE CHOICE QUESTION

3 mins • 1 pt

In the reaction of permanganate anion with iodide in acidic solution
2MnO₄⁻+ 16H⁺ + 10 I⁻ → 2 Mn²⁺ + 8H₂O + 5 I₂
what has been reduced and what is its change in oxidation number?

iodine;

from −1 to 0

manganese;

from +7 to +2

oxygen;

from −1 to −2

hydrogen;

from +1 to 0

Tags

NGSS.HS-PS1-2

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

When the equation below is correctly balanced, the coefficients, in order, are:
_Li(s) + _Mg²⁺(aq) → _Li⁺(aq) + _Mg(s)

2, 1, 2, 1

1, 1, 1, 1

1, 1, 2, 1

1, 2, 1, 1,

Tags

NGSS.HS-PS1-7

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

3Sn²⁺(aq) + Cr₂O₇^2-(aq) + 14H⁺(aq) → 3Sn⁴⁺(aq) + 2Cr³⁺(aq) + 7H₂O(l)

The equation shown represents the reaction performed in a REDOX titration. Which of the following is true regarding the stoichiometry and the REDOX process in the equation?

Three times the number of Sn²⁺ ions are consumed as Cr₂O₇^2- ions consumed.

Sn²⁺ is oxidized to Sn⁴⁺.

One-third the number of Sn²⁺ ions are consumed as Cr₂O₇^2- ions consumed.

Sn²⁺ is oxidized to Sn⁴⁺.

Three times the number of Sn²⁺ ions are consumed as Cr₂O₇^2- ions consumed.

Sn²⁺ is reduced to Sn⁴⁺.

One-third the number of Sn²⁺ ions are consumed as Cr₂O₇^2- ions consumed.

Sn²⁺ is reduced to Sn⁴⁺.

Tags

NGSS.HS-PS1-2

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

6I^-(aq) + 4H₂O(l) + 2MnO₄^-(aq) → 3I₂(aq) + 2MnO₂(s) + 8OH^-(aq)

The equation shown represents the reaction performed in a REDOX titration. Which of the following is true regarding the stoichiometry and the REDOX process in the equation?

Three times the number of MnO₄^- ions are consumed as I^- ions consumed.

I^- is oxidized to I₂.

One-third the number of MnO₄^- ions are consumed as I^- ions consumed.

I^- is oxidized to I₂.

One-third the number of MnO₄^- ions are consumed as I^- ions consumed.

I^- is reduced to I₂.

Three times the number of MnO₄^- ions are consumed as I^- ions consumed.

I^- is reduced to I₂.

Tags

NGSS.HS-PS1-2

MULTIPLE CHOICE QUESTION

3 mins • 1 pt

In this electrochemical cell, if the salt bridge is removed what happens to the voltage?

E_cell = 0.00V

E_cell = +2.31V

0.00V < E_cell < +2.31V

E_cell > +2.31V

Tags

NGSS.HS-PS3-1

NGSS.HS-PS3-5

MULTIPLE CHOICE QUESTION

3 mins • 1 pt

In this electrochemical cell, if the Cr electrode is replaced with an inert electrode what happens to the voltage?

E_cell = 0.00V

E_cell = +2.31V

0.00V < E_cell < +2.31V

E_cell > +2.31V

Tags

NGSS.HS-PS1-2

MULTIPLE CHOICE QUESTION

3 mins • 1 pt

In this electrochemical cell, if the Li electrode is replaced with an inert electrode what happens to the voltage?

E_cell = 0.00V

E_cell = +2.31V

0.00V < E_cell < +2.31V

E_cell > +2.31V

Tags

NGSS.HS-PS1-2

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AP CHEM Unit 3 In Class Review

26 questions

In the reaction of permanganate anion with iodide in acidic solution
2MnO₄⁻+ 16H⁺ + 10 I⁻ → 2 Mn²⁺ + 8H₂O + 5 I₂
what has been reduced and what is its change in oxidation number?

When the equation below is correctly balanced, the coefficients, in order, are:
_Li(s) + _Mg²⁺(aq) → _Li⁺(aq) + _Mg(s)

3Sn²⁺(aq) + Cr₂O₇^2-(aq) + 14H⁺(aq) → 3Sn⁴⁺(aq) + 2Cr³⁺(aq) + 7H₂O(l)

The equation shown represents the reaction performed in a REDOX titration. Which of the following is true regarding the stoichiometry and the REDOX process in the equation?

6I^-(aq) + 4H₂O(l) + 2MnO₄^-(aq) → 3I₂(aq) + 2MnO₂(s) + 8OH^-(aq)

The equation shown represents the reaction performed in a REDOX titration. Which of the following is true regarding the stoichiometry and the REDOX process in the equation?

In this electrochemical cell, if the salt bridge is removed what happens to the voltage?

In this electrochemical cell, if the Cr electrode is replaced with an inert electrode what happens to the voltage?

In this electrochemical cell, if the Li electrode is replaced with an inert electrode what happens to the voltage?

If E° is positive, ∆G° must be _ and K must be _ than 1.

Which of the following expressions is correct for the time, in seconds, required to deposit 5.90 grams of cobalt from aqueous Co(NO₃)₃ using a constant current of 4.0 amperes?
1 faraday = 96,500 coulombs

Cu²⁺(aq) + Zn(s) → Cu(s) + Zn²⁺(aq)
E⁰_cell= +1.10V
Which of the following is true for the reaction shown? Select ALL that apply.

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AP CHEM Unit 3 In Class Review

26 questions

In the reaction of permanganate anion with iodide in acidic solution2MnO4− + 16H+ + 10 I− → 2 Mn2+ + 8H2O + 5 I2what has been reduced and what is its change in oxidation number?

When the equation below is correctly balanced, the coefficients, in order, are:___Li(s) + ___Mg2+(aq) → ___Li+(aq) + ___Mg(s)

3Sn2+(aq) + Cr2O72-(aq) + 14H+(aq) → 3Sn4+(aq) + 2Cr3+(aq) + 7H2O(l)The equation shown represents the reaction performed in a REDOX titration. Which of the following is true regarding the stoichiometry and the REDOX process in the equation?

6I-(aq) + 4H2O(l) + 2MnO4-(aq) → 3I2(aq) + 2MnO2(s) + 8OH-(aq)The equation shown represents the reaction performed in a REDOX titration. Which of the following is true regarding the stoichiometry and the REDOX process in the equation?

In this electrochemical cell, if the salt bridge is removed what happens to the voltage?

In this electrochemical cell, if the Cr electrode is replaced with an inert electrode what happens to the voltage?

In this electrochemical cell, if the Li electrode is replaced with an inert electrode what happens to the voltage?

If E° is positive, ∆G° must be _____________ and K must be _____________ than 1.

Which of the following expressions is correct for the time, in seconds, required to deposit 5.90 grams of cobalt from aqueous Co(NO₃)₃ using a constant current of 4.0 amperes?1 faraday = 96,500 coulombs

Cu2+(aq) + Zn(s) → Cu(s) + Zn2+(aq) E⁰cell= +1.10VWhich of the following is true for the reaction shown? Select ALL that apply.

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In the reaction of permanganate anion with iodide in acidic solution
2MnO₄⁻+ 16H⁺ + 10 I⁻ → 2 Mn²⁺ + 8H₂O + 5 I₂
what has been reduced and what is its change in oxidation number?

When the equation below is correctly balanced, the coefficients, in order, are:
_Li(s) + _Mg²⁺(aq) → _Li⁺(aq) + _Mg(s)

3Sn²⁺(aq) + Cr₂O₇^2-(aq) + 14H⁺(aq) → 3Sn⁴⁺(aq) + 2Cr³⁺(aq) + 7H₂O(l)

The equation shown represents the reaction performed in a REDOX titration. Which of the following is true regarding the stoichiometry and the REDOX process in the equation?

6I^-(aq) + 4H₂O(l) + 2MnO₄^-(aq) → 3I₂(aq) + 2MnO₂(s) + 8OH^-(aq)

The equation shown represents the reaction performed in a REDOX titration. Which of the following is true regarding the stoichiometry and the REDOX process in the equation?

If E° is positive, ∆G° must be _ and K must be _ than 1.

Which of the following expressions is correct for the time, in seconds, required to deposit 5.90 grams of cobalt from aqueous Co(NO₃)₃ using a constant current of 4.0 amperes?
1 faraday = 96,500 coulombs

Cu²⁺(aq) + Zn(s) → Cu(s) + Zn²⁺(aq)
E⁰_cell= +1.10V
Which of the following is true for the reaction shown? Select ALL that apply.