Question 1

Write a balanced net ionic equation for the overall reaction represented by the following cell notation. Cu(s) | Cu²⁺(aq) || Mn²⁺(aq) | Mn(s)

Accepted Answer

The overall reaction can be split into two half-reactions: Cu(s) → Cu²⁺(aq) + 2 e- (oxidation) Mn²⁺(aq) + 2 e- → Mn(s) (reduction) When combined, these two half-reactions give the balanced net ionic equation: Cu(s) + Mn²⁺(aq) → Mn(s) + Cu²⁺(aq)

Question 2

Given the following two half-reactions, write the overall reaction in the direction in which it is product-favored, and calculate the standard cell potential. Pb²⁺(aq) + 2 e^- ? Pb(s) E° = -0.126 V Fe³⁺(aq) + e^- ? Fe²⁺(s) E° = +0.771 V

Accepted Answer

The answer of Given the following two half-reactions, write the...

Question 3

Consider the following half-reactions. Ag⁺(aq) + e^- → Ag(s) E° = +0.80 V Cu²⁺(aq) + 2 e^- → Cu(s) E° = +0.34 V Pb²⁺(aq) + 2 e^- → Pb(s) E° = -0.13 V Fe²⁺(aq) + 2 e^- → Fe(s) E° = -0.44 V Al³⁺(aq) + 3 e^- → Al(s) E° = -1.66 V Which of the following species will oxidize lead, Pb(s)?

Accepted Answer

Species with a higher reduction potential (E°) can oxidize species with a lower reduction potential. Ag^+ (E° = +0.80 V) and Cu^2+ (E° = +0.34 V) have higher reduction potentials than Pb^2+ (E° = -0.13 V), meaning they can accept electrons from Pb(s), oxidizing it.

Question 4

According to the cell notation below, which of the following species is undergoing reduction? Ni | Ni²⁺(aq) || Mn²⁺(aq) | MnO₂(s) | Pt(s)

Accepted Answer

The answer of According to the cell notation below, which...

Question 5

Use the following standard reduction potentials to determine which species is the best oxidizing agent. 
$$\begin{array} { l l } 
\mathrm { O } _ { 2 } ( \mathrm {~g} ) + 4 \mathrm { H } ^ { + } ( \mathrm { aq } ) + 4 \mathrm { e } ^ { - } \rightarrow 2 \mathrm { H } _ { 2 } \mathrm { O } ( \ell ) & E ^ { \circ } = + 1.229 \mathrm {~V} \
\mathrm {{ Hg } _ { 2 }} ^ { 2 + } ( \mathrm { aq } ) + 2 \mathrm { e } ^ { - } \rightarrow 2 \mathrm { Hg } ( \ell ) & E ^ { \circ } = + 0.789 \mathrm {~V} \
\mathrm { I } _ { 2 } ( \mathrm {~s} ) + 2 \mathrm { e } ^ { - } \rightarrow 2 \mathrm { I } ^ { - } ( \mathrm { aq } ) & E ^ { \circ } = + 0.535 \mathrm {~V}
\end{array}$$

Accepted Answer

The standard reduction potential of O₂(g) is the highest, indicating that it is the best oxidizing agent among the given species.

Question 6

Which of the following is the cell notation for a cell in which the hydrogen electrode is the anode and the cathode half-reaction is Co³⁺(aq) + e− → Co²⁺(aq)?

Accepted Answer

The anode is the hydrogen electrode, which is represented as Pt(s)| H2(g)| H+(aq). The cathode half-reaction is Co³⁺(aq)+ e− → Co²⁺(aq), which can be rearranged as Co²⁺(aq)| Co³⁺(aq). Therefore, the cell notation is Pt(s)| H₂(g)| H⁺(aq)|| Co³⁺(aq),Co²⁺(aq)| Pt(s).

Question 7

Which of the following is the cell notation for a voltaic cell based on the following reaction? Cu²⁺(aq) + Pb(s) + SO₄^2-(aq) → Cu(s) + PbSO₄(s)

Accepted Answer

The answer of Which of the following is the cell...

Question 8

In the given electrochemical cell, which of the following is the cathode half-reaction? Zn(s) | Zn²⁺(aq) || Fe³⁺(aq), Fe²⁺(aq) | Pt(s)

Accepted Answer

The cathode is where reduction occurs, and option A correctly shows the reduction of Fe^3+ to Fe^2+, which is consistent with the behavior of a cathode in an electrochemical cell.

Question 9

Which of the following is the balanced overall reaction and standard cell potential of an electrochemical cell constructed from half-cells with the given half reactions? Pt²⁺(aq) + 2 e- ? Pt(s); E° = 1.180 V Pb²⁺(aq) + 2 e- ? Pb(s); E° = -0.130 V

Accepted Answer

The correct answer is A because the overall reaction is the sum of the two half-reactions, and the standard cell potential is the difference between the standard reduction potentials of the two half-reactions.

Question 10

Calculate the standard cell potential ( $E _ { \text {cell } } ^ { \circ }$ ) for the reaction 2 Ag(s) + Co²⁺(aq) ? 2 Ag⁺(aq) + Co(s). The standard reduction potentials are as follows: Ag⁺(aq) + e^-? Ag(s) E° = 0.8 V Co²⁺(aq) +2 e^-? Co(s) E° = -0.277 V

Accepted Answer

The standard cell potential is calculated using the formula:$E _ { \text {cell } } ^ { \circ }$ = $E _ { \text {red } } ^ { \circ }$ (cathode) - $E _ { \text {red } } ^ { \circ }$ (anode)In this case, the cathode is the reduction of Ag⁺ to Ag, and the anode is the oxidation of Co to Co²⁺. Therefore, the standard cell potential is:$E _ { \text {cell } } ^ { \circ }$ = 0.8 V - (-0.277 V) = 1.077 VTherefore, the correct answer is A.

Question 11

Write a balanced net ionic equation for the overall reaction represented by the following cell notation. Al(s) | Al³⁺(aq) || Cl₂(g) | Cl-(aq) | Pt(s)

Accepted Answer

The correct net ionic equation involves aluminum solid reacting with chlorine gas to form aluminum ions in solution and chloride ions in solution, with the coefficients ensuring the charge and atoms are balanced.

Question 12

Calculate $E _ { \text {cell } } ^ { \circ }$ for the electrochemical cell Ag(s) | AgCl(s) | Cl^-(aq, 1.0 M) || Cu²⁺(aq, 1.0 M) | Cu(s). The standard reduction potentials are as follows: Cu²⁺(aq) + 2 e^- ? Cu(s) E° = +0.337 V AgCl(s) + e^- ? Ag(s) + Cl^-(aq) E° = +0.222 V

Accepted Answer

The cell potential is calculated by subtracting the anode potential from the cathode potential: $E _ { \text {cell } } ^ { \circ } = E _ { \text {cathode } } ^ { \circ } - E _ { \text {anode } } ^ { \circ }$. Here, the cathode is Cu with $E° = +0.337 \, \text{V}$ and the anode is AgCl with $E° = +0.222 \, \text{V}$. Thus, $E _ { \text {cell } } ^ { \circ } = 0.337 \, \text{V} - 0.222 \, \text{V} = +0.115 \, \text{V}$.

Question 13

An SHE electrode has been assigned a standard reduction potential, E°, of 0.00 volts. Which of the following reactions will occur at this electrode?

Accepted Answer

The SHE (Standard Hydrogen Electrode) is defined by the half-reaction 2 H⁺(aq) + 2 e⁻ → H₂(g), which has a standard reduction potential of 0.00 volts.

Question 14

Consider the following half-reactions. Cl₂(g) + 2 e^- → 2 Cl^-(aq) E° = +1.36 V Ag⁺(aq) + e^- → Ag(s) E° = +0.80 V Cu²⁺(aq) + 2 e^- → Cu(s) E° = +0.34 V Sn²⁺(aq) + 2 e^- → Sn(s) E° = -0.14 V Al³⁺(aq) + 3 e^- → Al(s) E° = -1.66 V Which of the following species will reduce Cu²⁺(aq) ion?

Accepted Answer

The answer of Consider the following half-reactions. Cl₂(g) + 2...

Question 15

Use the following standard reduction potentials to determine which species is the strongest oxidizing agent. Fe²⁺(aq) + 2 e^- ? Fe(s); E° = -0.41 V Pt²⁺(aq) + 2 e^- ? Pt(s); E° = 1.18 V Cr₂O₇^2-(aq) + 14 H⁺(aq) + 6 e^- ? 2 Cr³⁺(aq) + 7 H₂O( $\ell$ ); E° = 1.33 V

Accepted Answer

The answer of Use the following standard reduction potentials to...

Question 16

Use the following standard reduction potentials to determine which species is the strongest reducing agent. 2 H⁺(aq) + 2 e^- → H₂(g); 0.00 V K⁺(aq) + e^- → K(s); -2.93 V F₂(g) + 2 e^- → 2 F^-(aq); 2.87 V Al³⁺(aq) + 3 e^- → Al(s); -1.66 V Pb²⁺(aq) + 2 e^- → Pb(s); -0.13 V

Accepted Answer

The strongest reducing agent is the one with the most negative standard reduction potential, which is potassium (K) with a potential of -2.93 V.

Question 17

Calculate $E _ { \text {cell } } ^ { \circ }$ for the electrochemical cell Pb(s) |PbCl₂(s) | Cl^-(aq, 1.0 M) || Fe³⁺(aq, 1.0 M), Fe²⁺(aq, 1.0 M) | Pt(s). The standard reduction potentials are as follows: Pb²⁺(aq) + 2 e^- ? Pb(s) E° = -0.126 V PbCl₂(s) + 2 e^- ? Pb(s) + 2 Cl^-(aq) E° = -0.267 V Fe³⁺(aq) + e^- ? Fe²⁺(aq) E° = +0.771 V Fe²⁺(aq) + e^- ? Fe(s) E° = -0.44 V

Accepted Answer

The answer of Calculate \(E _ { \text {cell }...

Question 18

Which of the following species are likely to behave as oxidizing agents? Li(s), H₂(g), MnO₄^-(aq), and Cl^-(aq)

Accepted Answer

The answer of Which of the following species are likely...

Question 19

The unit for electromotive force, emf, is the volt. 1 volt is equal to _____.

Accepted Answer

The unit for electromotive force, emf, is the volt. 1 volt is equal to one joule of energy per coulomb of charge moved. Therefore, 1 volt can also be written as 1 joule per coulomb.

Question 20

Calculate E°_cell for the cell for the reaction 2 Ga(s) + 3 Sn⁴⁺(aq) → 3 Sn²⁺(aq) +2 Ga³⁺(aq). The standard reduction potentials are as follows: Ga³⁺(aq) + 3 e− → Ga(s) E° = -0.55 V Sn⁴⁺(aq) + 2 e− → Sn²⁺(aq) E° = 0.15V

Accepted Answer

The standard cell potential (E°cell) is calculated by subtracting the standard reduction potential of the anode (the more negative value) from the standard reduction potential of the cathode (the more positive value). Here, Ga is oxidized (anode reaction) and Sn2+ is reduced (cathode reaction). Thus, E°cell = 0.15 V (for Sn2+/Sn) - (-0.55 V) (for Ga3+/Ga) = 0.70 V.

Quiz 20: Principles of Chemical Reactivity: Electron Transfer Reactions

Write a balanced net ionic equation for the overall reaction represented by the following cell notation. Cu(s) | Cu²⁺(aq) || Mn²⁺(aq) | Mn(s)

Given the following two half-reactions, write the overall reaction in the direction in which it is product-favored, and calculate the standard cell potential. Pb²⁺(aq) + 2 e^- ? Pb(s) E° = -0.126 V Fe³⁺(aq) + e^- ? Fe²⁺(s) E° = +0.771 V

According to the cell notation below, which of the following species is undergoing reduction? Ni | Ni²⁺(aq) || Mn²⁺(aq) | MnO₂(s) | Pt(s)

Which of the following is the cell notation for a cell in which the hydrogen electrode is the anode and the cathode half-reaction is Co³⁺(aq) + e− → Co²⁺(aq) ?

Which of the following is the cell notation for a voltaic cell based on the following reaction? Cu²⁺(aq) + Pb(s) + SO₄^2-(aq) → Cu(s) + PbSO₄(s)

In the given electrochemical cell, which of the following is the cathode half-reaction? Zn(s) | Zn²⁺(aq) || Fe³⁺(aq) , Fe²⁺(aq) | Pt(s)

Which of the following is the balanced overall reaction and standard cell potential of an electrochemical cell constructed from half-cells with the given half reactions? Pt²⁺(aq) + 2 e- ? Pt(s) ; E° = 1.180 V Pb²⁺(aq) + 2 e- ? Pb(s) ; E° = -0.130 V

Calculate the standard cell potential ( $E _ { \text {cell } } ^ { \circ }$ ) for the reaction 2 Ag(s) + Co²⁺(aq) ? 2 Ag⁺(aq) + Co(s) . The standard reduction potentials are as follows: Ag⁺(aq) + e^-? Ag(s) E° = 0.8 V Co²⁺(aq) +2 e^-? Co(s) E° = -0.277 V

Write a balanced net ionic equation for the overall reaction represented by the following cell notation. Al(s) | Al³⁺(aq) || Cl₂(g) | Cl-(aq) | Pt(s)

Calculate $E _ { \text {cell } } ^ { \circ }$ for the electrochemical cell Ag(s) | AgCl(s) | Cl^-(aq, 1.0 M) || Cu²⁺(aq, 1.0 M) | Cu(s) . The standard reduction potentials are as follows: Cu²⁺(aq) + 2 e^- ? Cu(s) E° = +0.337 V AgCl(s) + e^- ? Ag(s) + Cl^-(aq) E° = +0.222 V

An SHE electrode has been assigned a standard reduction potential, E°, of 0.00 volts. Which of the following reactions will occur at this electrode?

Use the following standard reduction potentials to determine which species is the strongest oxidizing agent. Fe²⁺(aq) + 2 e^- ? Fe(s) ; E° = -0.41 V Pt²⁺(aq) + 2 e^- ? Pt(s) ; E° = 1.18 V Cr₂O₇^2-(aq) + 14 H⁺(aq) + 6 e^- ? 2 Cr³⁺(aq) + 7 H₂O( $\ell$ ) ; E° = 1.33 V

Use the following standard reduction potentials to determine which species is the strongest reducing agent. 2 H⁺(aq) + 2 e^- → H₂(g) ; 0.00 V K⁺(aq) + e^- → K(s) ; -2.93 V F₂(g) + 2 e^- → 2 F^-(aq) ; 2.87 V Al³⁺(aq) + 3 e^- → Al(s) ; -1.66 V Pb²⁺(aq) + 2 e^- → Pb(s) ; -0.13 V

Which of the following species are likely to behave as oxidizing agents? Li(s) , H₂(g) , MnO₄^-(aq) , and Cl^-(aq)

The unit for electromotive force, emf, is the volt. 1 volt is equal to _____.

Calculate E°_cell for the cell for the reaction 2 Ga(s) + 3 Sn⁴⁺(aq) → 3 Sn²⁺(aq) +2 Ga³⁺(aq) . The standard reduction potentials are as follows: Ga³⁺(aq) + 3 e− → Ga(s) E° = -0.55 V Sn⁴⁺(aq) + 2 e− → Sn²⁺(aq) E° = 0.15V

Quiz 20: Principles of Chemical Reactivity: Electron Transfer Reactions

Write a balanced net ionic equation for the overall reaction represented by the following cell notation. Cu(s) | Cu2+(aq) || Mn2+(aq) | Mn(s)

Given the following two half-reactions, write the overall reaction in the direction in which it is product-favored, and calculate the standard cell potential. Pb2+(aq) + 2 e- ? Pb(s) E° = -0.126 V Fe3+(aq) + e- ? Fe2+(s) E° = +0.771 V

Consider the following half-reactions. Ag+(aq) + e- → Ag(s) E° = +0.80 V Cu2+(aq) + 2 e- → Cu(s) E° = +0.34 V Pb2+(aq) + 2 e- → Pb(s) E° = -0.13 V Fe2+(aq) + 2 e- → Fe(s) E° = -0.44 V Al3+(aq) + 3 e- → Al(s) E° = -1.66 V Which of the following species will oxidize lead, Pb(s) ?

According to the cell notation below, which of the following species is undergoing reduction? Ni | Ni2+(aq) || Mn2+(aq) | MnO2(s) | Pt(s)

Which of the following is the cell notation for a cell in which the hydrogen electrode is the anode and the cathode half-reaction is Co3+(aq) + e− → Co2+(aq) ?

Which of the following is the cell notation for a voltaic cell based on the following reaction? Cu2+(aq) + Pb(s) + SO42-(aq) → Cu(s) + PbSO4(s)

In the given electrochemical cell, which of the following is the cathode half-reaction? Zn(s) | Zn2+(aq) || Fe3+(aq) , Fe2+(aq) | Pt(s)

Which of the following is the balanced overall reaction and standard cell potential of an electrochemical cell constructed from half-cells with the given half reactions? Pt2+(aq) + 2 e- ? Pt(s) ; E° = 1.180 V Pb2+(aq) + 2 e- ? Pb(s) ; E° = -0.130 V

Calculate the standard cell potential ( Ecell ∘E _ { \text {cell } } ^ { \circ }Ecell ∘​ ) for the reaction 2 Ag(s) + Co2+(aq) ? 2 Ag+(aq) + Co(s) . The standard reduction potentials are as follows: Ag+(aq) + e-? Ag(s) E° = 0.8 V Co2+(aq) +2 e-? Co(s) E° = -0.277 V

Write a balanced net ionic equation for the overall reaction represented by the following cell notation. Al(s) | Al3+(aq) || Cl2(g) | Cl-(aq) | Pt(s)

Calculate Ecell ∘E _ { \text {cell } } ^ { \circ }Ecell ∘​ for the electrochemical cell Ag(s) | AgCl(s) | Cl-(aq, 1.0 M) || Cu2+(aq, 1.0 M) | Cu(s) . The standard reduction potentials are as follows: Cu2+(aq) + 2 e- ? Cu(s) E° = +0.337 V AgCl(s) + e- ? Ag(s) + Cl-(aq) E° = +0.222 V

An SHE electrode has been assigned a standard reduction potential, E°, of 0.00 volts. Which of the following reactions will occur at this electrode?

Consider the following half-reactions. Cl2(g) + 2 e- → 2 Cl-(aq) E° = +1.36 V Ag+(aq) + e- → Ag(s) E° = +0.80 V Cu2+(aq) + 2 e- → Cu(s) E° = +0.34 V Sn2+(aq) + 2 e- → Sn(s) E° = -0.14 V Al3+(aq) + 3 e- → Al(s) E° = -1.66 V Which of the following species will reduce Cu2+(aq) ion?

Use the following standard reduction potentials to determine which species is the strongest oxidizing agent. Fe2+(aq) + 2 e- ? Fe(s) ; E° = -0.41 V Pt2+(aq) + 2 e- ? Pt(s) ; E° = 1.18 V Cr2O72-(aq) + 14 H+(aq) + 6 e- ? 2 Cr3+(aq) + 7 H2O( ℓ\ellℓ ) ; E° = 1.33 V

Use the following standard reduction potentials to determine which species is the strongest reducing agent. 2 H+(aq) + 2 e- → H2(g) ; 0.00 V K+(aq) + e- → K(s) ; -2.93 V F2(g) + 2 e- → 2 F-(aq) ; 2.87 V Al3+(aq) + 3 e- → Al(s) ; -1.66 V Pb2+(aq) + 2 e- → Pb(s) ; -0.13 V

Which of the following species are likely to behave as oxidizing agents? Li(s) , H2(g) , MnO4-(aq) , and Cl-(aq)

The unit for electromotive force, emf, is the volt. 1 volt is equal to _____.

Calculate E°cell for the cell for the reaction 2 Ga(s) + 3 Sn4+(aq) → 3 Sn2+(aq) +2 Ga3+(aq) . The standard reduction potentials are as follows: Ga3+(aq) + 3 e− → Ga(s) E° = -0.55 V Sn4+(aq) + 2 e− → Sn2+(aq) E° = 0.15V ​

Write a balanced net ionic equation for the overall reaction represented by the following cell notation. Cu(s) | Cu²⁺(aq) || Mn²⁺(aq) | Mn(s)

Given the following two half-reactions, write the overall reaction in the direction in which it is product-favored, and calculate the standard cell potential. Pb²⁺(aq) + 2 e^- ? Pb(s) E° = -0.126 V Fe³⁺(aq) + e^- ? Fe²⁺(s) E° = +0.771 V

According to the cell notation below, which of the following species is undergoing reduction? Ni | Ni²⁺(aq) || Mn²⁺(aq) | MnO₂(s) | Pt(s)

Which of the following is the cell notation for a cell in which the hydrogen electrode is the anode and the cathode half-reaction is Co³⁺(aq) + e− → Co²⁺(aq) ?

Which of the following is the cell notation for a voltaic cell based on the following reaction? Cu²⁺(aq) + Pb(s) + SO₄^2-(aq) → Cu(s) + PbSO₄(s)

In the given electrochemical cell, which of the following is the cathode half-reaction? Zn(s) | Zn²⁺(aq) || Fe³⁺(aq) , Fe²⁺(aq) | Pt(s)

Which of the following is the balanced overall reaction and standard cell potential of an electrochemical cell constructed from half-cells with the given half reactions? Pt²⁺(aq) + 2 e- ? Pt(s) ; E° = 1.180 V Pb²⁺(aq) + 2 e- ? Pb(s) ; E° = -0.130 V

Calculate the standard cell potential ( $E _ { \text {cell } } ^ { \circ }$ ) for the reaction 2 Ag(s) + Co²⁺(aq) ? 2 Ag⁺(aq) + Co(s) . The standard reduction potentials are as follows: Ag⁺(aq) + e^-? Ag(s) E° = 0.8 V Co²⁺(aq) +2 e^-? Co(s) E° = -0.277 V

Write a balanced net ionic equation for the overall reaction represented by the following cell notation. Al(s) | Al³⁺(aq) || Cl₂(g) | Cl-(aq) | Pt(s)

Calculate $E _ { \text {cell } } ^ { \circ }$ for the electrochemical cell Ag(s) | AgCl(s) | Cl^-(aq, 1.0 M) || Cu²⁺(aq, 1.0 M) | Cu(s) . The standard reduction potentials are as follows: Cu²⁺(aq) + 2 e^- ? Cu(s) E° = +0.337 V AgCl(s) + e^- ? Ag(s) + Cl^-(aq) E° = +0.222 V

Use the following standard reduction potentials to determine which species is the strongest oxidizing agent. Fe²⁺(aq) + 2 e^- ? Fe(s) ; E° = -0.41 V Pt²⁺(aq) + 2 e^- ? Pt(s) ; E° = 1.18 V Cr₂O₇^2-(aq) + 14 H⁺(aq) + 6 e^- ? 2 Cr³⁺(aq) + 7 H₂O( $\ell$ ) ; E° = 1.33 V

Which of the following species are likely to behave as oxidizing agents? Li(s) , H₂(g) , MnO₄^-(aq) , and Cl^-(aq)

Calculate E°_cell for the cell for the reaction 2 Ga(s) + 3 Sn⁴⁺(aq) → 3 Sn²⁺(aq) +2 Ga³⁺(aq) . The standard reduction potentials are as follows: Ga³⁺(aq) + 3 e− → Ga(s) E° = -0.55 V Sn⁴⁺(aq) + 2 e− → Sn²⁺(aq) E° = 0.15V