Calculate the equilibrium constant for the reaction below at 25 S1U1P1$\circ$S1S1P0C, Co(s)+ 2 Cr3+(aq)$\to$Co2+(aq)+ 2 Cr2+(aq) Given the following thermodynamic information. Co2+(aq)+ 2 e- $\to$Co(s)$~~~~~~~~$ES1U1P1$\circ$S1S1P0= -0.28 V Cr3+(aq)+ e- $\to$ Cr2+(aq)$~~~~~~~~$ES1U1P1$\circ$S1S1P0= -0.41 V

A) 4.0 $\times$ 10-5 B) 2.5 $\times$ 104 C) 1.0 $\times$ 105 D) 1.2 $\times$ 105 E) 1.3 $\times$ 105 A) 4.0 $\times$ 10-5 B) 2.5 $\times$ 104 C) 1.0 $\times$ 105 D) 1.2 $\times$ 105 E) 1.3 $\times$ 105

Calculate $\Delta$rGS1U1P1$\circ$S1S1P0 for the disproportionation reaction of Cu+ at 25 S1U1P1$\circ$S1S1P0C, 2 Cu+(aq)$\to$Cu2+(aq)+ Cu(s) Given the following thermodynamic information. Cu+(aq)+ e- $\to$ Cu(s)$~~~~~~~~$ES1U1P1$\circ$S1S1P0 = +0.518 V Cu2+(aq)+ 2 e- $\to$Cu(s)$~~~~~~~~$ES1U1P1$\circ$S1S1P0 = +0.337 V

A) -165 kJ/mol.rxn B) -135 kJ/mol.rxn C) -34.9 kJ/mol.rxn D) +17.5 kJ/mol.rxn E) +135 kJ/mol.rxn A) -165 kJ/mol.rxn B) -135 kJ/mol.rxn C) -34.9 kJ/mol.rxn D) +17.5 kJ/mol.rxn E) +135 kJ/mol.rxn

The following reaction occurs spontaneously. 2 H+(aq)+ Ca(s)$\to$ Ca2+(aq)+ H2(g) Write the balanced oxidation half-reaction.

A) 2 H+(aq)+ 2 e- $\to$ H2(g) B) 2 H+(aq)$\to$H2(g)+ 2 e- C) H2(g)$\to$ 2 H+(aq)+ 2 e- D) Ca(s)+ 2 e- $\to$ Ca2+(aq) E) Ca(s)$\to$Ca2+(aq)+ 2 e- A) 2 H+(aq)+ 2 e- $\to$ H2(g) B) 2 H+(aq)$\to$H2(g)+ 2 e- C) H2(g)$\to$ 2 H+(aq)+ 2 e- D) Ca(s)+ 2 e- $\to$ Ca2+(aq) E) Ca(s)$\to$Ca2+(aq)+ 2 e-

When an aqueous solution of sodium sulfate is electrolyzed,what are the expected products? Reduction Half-Reaction$~~~~~~~~$$~~~~~~~~$E° (V) $\to$ Na(s) $~~~~~~~~$$~~~~~~~~$$~~~~~~~~$-2.71 2H2O(l)+ 2e- $\to$ H2(g)+ 2OH-(aq) $~~~~ ~~$$~ ~$-0.83 2H+(aq)+ 2e- $\to$ H2(g) $~~~~~~~~$$~~~~~~~~$$~~~~~~~~$0.00 O2(g)+ 4H+(aq)+ 4e- $\to$ 2H2O(l) $~~~~~~~~$$~~ ~ $1.23 S2O82-(aq)+ 2e- $\to$ 2SO42-(aq) $~~~~~~~~$$~~~~~~ ~$2.01

A) Na(s)and H2(g) B) H2(g),OH-(aq),O2(g),and H+(aq) C) O2(g),H+(aq),and Na(s) D) H2(g),OH-(aq),and Na(s) E) H2(g),OH-(aq),and S2O82-(aq) A) Na(s)and H2(g) B) H2(g),OH-(aq),O2(g),and H+(aq) C) O2(g),H+(aq),and Na(s) D) H2(g),OH-(aq),and Na(s) E) H2(g),OH-(aq),and S2O82-(aq)

Which of the following statements is true concerning the electrochemical cell below, Ba(s)| Ba2+(aq,1.0 M)|| Mn2+(aq,1.0 M)| Mn(s) And given the following standard reduction potentials? Ba2+(aq)+ 2e- $\to$ Ba(s); $~~~~~~~~$$~~~~~~~~$E° = -2.91 V Mn2+(aq)+ 2e-$\to$ Mn(s); $~~~~~~~~$$~~~~~~~~$E° = -1.19 V

A) The cell reaction is spontaneous with a standard cell potential of -4.10 V. B) The cell reaction is spontaneous with a standard cell potential of 1.72 V. C) The cell reaction is nonspontaneous with a standard cell potential of 1.72 V. D) The cell reaction is nonspontaneous with a standard cell potential of -4.10 V. E) The cell reaction is spontaneous with a standard cell potential of -1.72 V. A) The cell reaction is spontaneous with a standard cell potential of -4.10 V. B) The cell reaction is spontaneous with a standard cell potential of 1.72 V. C) The cell reaction is nonspontaneous with a standard cell potential of 1.72 V. D) The cell reaction is nonspontaneous with a standard cell potential of -4.10 V. E) The cell reaction is spontaneous with a standard cell potential of -1.72 V.

One kind of battery used in watches contains mercury(II)oxide.As current flows,the mercury(II)oxide is reduced to mercury. HgO(s)+ H2O( )+ 2 e- $\to$ Hg( )+ 2 OH-(aq) If 2.3 $\times$ 10-5 amperes flows continuously for 1200 days,what mass of Hg( )is produced?

A) 2.5 g B) 5.0 g C) 9.9 g D) 13 g E) 15 g A) 2.5 g B) 5.0 g C) 9.9 g D) 13 g E) 15 g

The electrochemical reaction which powers a lead-acid storage battery is as follows: Pb(s)+ PbO2(s)+ 4H+(aq)+ 2SO42-(aq)$\to$ 2PbSO4(s)+ 2H2O(l) A single cell of this battery consists of a Pb electrode and a PbO2 electrode,each submerged in sulfuric acid.What reaction occurs at the cathode during discharge?

A) Pb(s)is reduced to PbSO4(s). B) PbO2(s)is reduced to PbSO4(s). C) PbO2(s)is oxidized to PbSO4(s). D) Pb(s)is oxidized to PbSO4(s). E) H+ is oxidized to H2O(l). A) Pb(s)is reduced to PbSO4(s). B) PbO2(s)is reduced to PbSO4(s). C) PbO2(s)is oxidized to PbSO4(s). D) Pb(s)is oxidized to PbSO4(s). E) H+ is oxidized to H2O(l).

Consider the following half-reactions: Ag+(aq)+ e- $\to$ Ag(s)$~~~~~~~~$$~~~~~~~~$ES1U1P1$\circ$S1S1P0 = +0.80 V Cu2+(aq)+ 2 e- $\to$ Cu(s)$~~~~~~~~$$~ ~~ ~$ES1U1P1$\circ$S1S1P0 = +0.34 V Pb2+(aq)+ 2 e- $\to$ Pb(s)$~~~~~~~~$$~~ ~ ~~$ES1U1P1$\circ$S1S1P0 = -0.13 V Fe2+(aq)+ 2 e- $\to$ Fe(s)$~~~~~~~~$$~~ ~ ~~$ES1U1P1$\circ$S1S1P0 = -0.44 V Al3+(aq)+ 3 e- $\to$ Al(s)$~~~~~~~~$$~~~ ~ ~$ES1U1P1$\circ$S1S1P0 = -1.66 V Which of the above metals or metal ions will oxidize Pb(s)?

A) Ag+(aq)and Cu2+(aq) B) Ag(s)and Cu(s) C) Fe2+(aq)and Al3+(aq) D) Fe(s)and Al(s) E) Cu2+(aq)and Fe2+(aq) A) Ag+(aq)and Cu2+(aq) B) Ag(s)and Cu(s) C) Fe2+(aq)and Al3+(aq) D) Fe(s)and Al(s) E) Cu2+(aq)and Fe2+(aq)

Given: Mn2+(aq)+ 2e- $\to$ Mn(s); E° = -1.18 V Cu2+(aq)+ 2e- $\to$ Cu(s); E° = 0.34 V Cr2O72-(aq)+ 14H+(aq)+ 6e- $\to$2Cr3+(aq)+ 7H2O(l); E° = 1.33 V Which of the following species is the strongest reducing agent?

A) Mn B) Cu C) Cr3+ D) Mn2+ E) Cr2O72- A) Mn B) Cu C) Cr3+ D) Mn2+ E) Cr2O72-

Calculate the equilibrium constant for the following reaction at 25 S1U1P1$\circ$S1S1P0C, 2 IO3-(aq)+ 5 Hg( )+ 12 H+(aq)$\to$ I2(s)+ 5 Hg2+(aq)+ 6 H2O( ) Given the following thermodynamic information. IO3-(aq)+ 6 H+(aq)+ 5 e- $\to$ I2(s)+ 3 H2O( )$~~~~~~~~$ES1U1P1$\circ$S1S1P0 = +1.20 V Hg2+(aq)+ 2 e- $\to$ Hg( )$~~~~~~~~$$~~~~~~~~$$~~~~~~~~$$~~~~~~~~$ES1U1P1$\circ$S1S1P0= +0.86 V

A) 3 $\times$ 10-58 B) 6 $\times$ 105 C) 3 $\times$ 1011 D) 6 $\times$ 1028 E) 3 $\times$ 1057 A) 3 $\times$ 10-58 B) 6 $\times$ 105 C) 3 $\times$ 1011 D) 6 $\times$ 1028 E) 3 $\times$ 1057

Exam 20: Principles of Reactivity: Electron Transfer Reactions

Calculate the equilibrium constant for the reaction below at 25 ^$\circ$C, Co(s)+ 2 Cr³⁺(aq) $\to$ Co²⁺(aq)+ 2 Cr²⁺(aq) Given the following thermodynamic information. Co²⁺(aq)+ 2 e^- $\to$ Co(s) $$ E^$\circ$= -0.28 V Cr³⁺(aq)+ e^- $\to$ Cr²⁺(aq) $$ E^$\circ$= -0.41 V

(Multiple Choice)

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Question 21

The fuel cells used aboard NASA's Space Shuttles are electrochemical cells that generate electricity from which overall chemical reaction?

(Multiple Choice)

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Question 22

Write a balanced chemical equation for the following reaction in a basic solution. ClO^-(aq)+ Cr(OH)₃(s) $\to$ Cl^-(aq)+ CrO₄^2-(aq)

(Multiple Choice)

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Question 23

Assuming the following reaction proceeds in the forward direction, Fe³⁺(aq)+ Co(s) $\to$ Fe²⁺(aq)+ Co²⁺(aq)

(Multiple Choice)

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Question 24

Calculate $\Delta$ _rG^$\circ$ for the disproportionation reaction of Cu⁺ at 25 ^$\circ$C, 2 Cu⁺(aq) $\to$ Cu²⁺(aq)+ Cu(s) Given the following thermodynamic information. Cu⁺(aq)+ e^- $\to$ Cu(s) $$ E^$\circ$ = +0.518 V Cu²⁺(aq)+ 2 e^- $\to$ Cu(s) $$ E^$\circ$ = +0.337 V

(Multiple Choice)

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Question 25

The following reaction occurs spontaneously. 2 H⁺(aq)+ Ca(s) $\to$ Ca²⁺(aq)+ H₂(g) Write the balanced oxidation half-reaction.

(Multiple Choice)

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Question 26

When an aqueous solution of sodium sulfate is electrolyzed,what are the expected products? Reduction Half-Reaction $$ $$ E° (V) $When an aqueous solution of sodium sulfate is electrolyzed,what are the expected products? Reduction Half-Reaction E° (V) \to Na(s) ~~~~~~~~~~~~~~ -2.71 2H2O(l)+ 2e- \to H2(g)+ 2OH-(aq) ~ ~ -0.83 2H+(aq)+ 2e- \to H2(g) ~~~~~~~~~~~~~~ 0.00 O2(g)+ 4H+(aq)+ 4e- \to 2H2O(l) ~ 1.23 S2O82-(aq)+ 2e- \to 2SO42-(aq) ~~~~~~~~~~~~~~ ~ 2.01$ $\to$ Na(s) $~~$ $$ $$ -2.71 2H₂O(l)+ 2e^- $\to$ H₂(g)+ 2OH^-(aq) $ $ $~ ~$ -0.83 2H⁺(aq)+ 2e^- $\to$ H₂(g) $~~$ $$ $$ 0.00 O₂(g)+ 4H⁺(aq)+ 4e^- $\to$ 2H₂O(l) $$ $ ~$ 1.23 S₂O₈^2-(aq)+ 2e^- $\to$ 2SO₄^2-(aq) $~~$ $ ~$ 2.01

(Multiple Choice)

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Question 27

Which of the following statements is true concerning the electrochemical cell below, Ba(s)| Ba²⁺(aq,1.0 M)|| Mn²⁺(aq,1.0 M)| Mn(s) And given the following standard reduction potentials? Ba²⁺(aq)+ 2e^- $\to$ Ba(s); $$ $$ E° = -2.91 V Mn²⁺(aq)+ 2e^- $\to$ Mn(s); $$ $$ E° = -1.19 V

(Multiple Choice)

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Question 28

Write a balanced chemical equation for the oxidation of Cd(s)by concentrated nitric acid,producing NO₂(g)and Cd²⁺(aq).

(Multiple Choice)

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Question 29

One kind of battery used in watches contains mercury(II)oxide.As current flows,the mercury(II)oxide is reduced to mercury. HgO(s)+ H₂O( $One kind of battery used in watches contains mercury(II)oxide.As current flows,the mercury(II)oxide is reduced to mercury. HgO(s)+ H2O( )+ 2 e- \to Hg( )+ 2 OH-(aq) If 2.3 \times 10-5 amperes flows continuously for 1200 days,what mass of Hg( )is produced?$ )+ 2 e^- $\to$ Hg( $One kind of battery used in watches contains mercury(II)oxide.As current flows,the mercury(II)oxide is reduced to mercury. HgO(s)+ H2O( )+ 2 e- \to Hg( )+ 2 OH-(aq) If 2.3 \times 10-5 amperes flows continuously for 1200 days,what mass of Hg( )is produced?$ )+ 2 OH^-(aq) If 2.3 $\times$ 10^-5 amperes flows continuously for 1200 days,what mass of Hg( $One kind of battery used in watches contains mercury(II)oxide.As current flows,the mercury(II)oxide is reduced to mercury. HgO(s)+ H2O( )+ 2 e- \to Hg( )+ 2 OH-(aq) If 2.3 \times 10-5 amperes flows continuously for 1200 days,what mass of Hg( )is produced?$ )is produced?

(Multiple Choice)

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Question 30

The electrochemical reaction which powers a lead-acid storage battery is as follows: Pb(s)+ PbO₂(s)+ 4H⁺(aq)+ 2SO₄^2-(aq) $\to$ 2PbSO₄(s)+ 2H₂O(l) A single cell of this battery consists of a Pb electrode and a PbO₂ electrode,each submerged in sulfuric acid.What reaction occurs at the cathode during discharge?

(Multiple Choice)

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Question 31

In an electrolytic cell,reduction occurs at the and oxidation occurs at the .

(Short Answer)

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Question 32

Balance the following half-reaction occurring in acidic solution. NO₃^-(aq) $\to$ HNO₂(aq)

(Multiple Choice)

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Question 33

Consider the following half-reactions: Ag⁺(aq)+ e^- $\to$ Ag(s) $$ $$ E^$\circ$ = +0.80 V Cu²⁺(aq)+ 2 e^- $\to$ Cu(s) $$ $~ ~~ ~$ E^$\circ$ = +0.34 V Pb²⁺(aq)+ 2 e^- $\to$ Pb(s) $~~~~~~$ $ ~ $ E^$\circ$ = -0.13 V Fe²⁺(aq)+ 2 e^- $\to$ Fe(s) $~~~~$ $ ~ $ E^$\circ$ = -0.44 V Al³⁺(aq)+ 3 e^- $\to$ Al(s) $~~~~$ $~ ~ ~$ E^$\circ$ = -1.66 V Which of the above metals or metal ions will oxidize Pb(s)?

(Multiple Choice)

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Question 34

Write a balanced chemical equation for the overall reaction represented by the cell notation below. Al(s)| Al³⁺(aq)|| Br^-(aq)| Br₂(g)| Pt(s)

(Multiple Choice)

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Question 35

Given: Mn²⁺(aq)+ 2e^- $\to$ Mn(s); E° = -1.18 V Cu²⁺(aq)+ 2e^- $\to$ Cu(s); E° = 0.34 V Cr₂O₇^2-(aq)+ 14H⁺(aq)+ 6e^- $\to$ 2Cr³⁺(aq)+ 7H₂O(l); E° = 1.33 V Which of the following species is the strongest reducing agent?

(Multiple Choice)

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Question 36

Balance the following oxidation-reduction occurring in acidic solution. MnO₄^-(aq)+ Cr²⁺(aq) $\to$ Mn²⁺(aq)+ Cr³⁺(aq)

(Multiple Choice)

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Question 37

Which of the following statements is true concerning the voltaic cell shown below?

(Multiple Choice)

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Question 38

Calculate the equilibrium constant for the following reaction at 25 ^$\circ$C, 2 IO₃^-(aq)+ 5 Hg( $Calculate the equilibrium constant for the following reaction at 25 \circ C, 2 IO3-(aq)+ 5 Hg( )+ 12 H+(aq) \to I2(s)+ 5 Hg2+(aq)+ 6 H2O( ) Given the following thermodynamic information. IO3-(aq)+ 6 H+(aq)+ 5 e- \to I2(s)+ 3 H2O( ) E \circ = +1.20 V Hg2+(aq)+ 2 e- \to Hg( ) E \circ = +0.86 V$ )+ 12 H⁺(aq) $\to$ I₂(s)+ 5 Hg²⁺(aq)+ 6 H₂O( $Calculate the equilibrium constant for the following reaction at 25 \circ C, 2 IO3-(aq)+ 5 Hg( )+ 12 H+(aq) \to I2(s)+ 5 Hg2+(aq)+ 6 H2O( ) Given the following thermodynamic information. IO3-(aq)+ 6 H+(aq)+ 5 e- \to I2(s)+ 3 H2O( ) E \circ = +1.20 V Hg2+(aq)+ 2 e- \to Hg( ) E \circ = +0.86 V$ ) Given the following thermodynamic information. IO₃^-(aq)+ 6 H⁺(aq)+ 5 e^- $\to$ I₂(s)+ 3 H₂O( $Calculate the equilibrium constant for the following reaction at 25 \circ C, 2 IO3-(aq)+ 5 Hg( )+ 12 H+(aq) \to I2(s)+ 5 Hg2+(aq)+ 6 H2O( ) Given the following thermodynamic information. IO3-(aq)+ 6 H+(aq)+ 5 e- \to I2(s)+ 3 H2O( ) E \circ = +1.20 V Hg2+(aq)+ 2 e- \to Hg( ) E \circ = +0.86 V$ ) $$ E^$\circ$ = +1.20 V Hg²⁺(aq)+ 2 e^- $\to$ Hg( $Calculate the equilibrium constant for the following reaction at 25 \circ C, 2 IO3-(aq)+ 5 Hg( )+ 12 H+(aq) \to I2(s)+ 5 Hg2+(aq)+ 6 H2O( ) Given the following thermodynamic information. IO3-(aq)+ 6 H+(aq)+ 5 e- \to I2(s)+ 3 H2O( ) E \circ = +1.20 V Hg2+(aq)+ 2 e- \to Hg( ) E \circ = +0.86 V$ ) $$ $$ $$ $$ E^$\circ$= +0.86 V

(Multiple Choice)

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Question 39

Balance the following half-reaction occurring in basic solution. MnO₂(s) $\to$ Mn(OH)₂(s)

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Question 40

Showing 21 - 40 of 86

Exam 20: Principles of Reactivity: Electron Transfer Reactions

The fuel cells used aboard NASA's Space Shuttles are electrochemical cells that generate electricity from which overall chemical reaction?

Write a balanced chemical equation for the following reaction in a basic solution. ClO-(aq)+ Cr(OH)3(s) →\to→ Cl-(aq)+ CrO42-(aq)

Assuming the following reaction proceeds in the forward direction, Fe3+(aq)+ Co(s) →\to→ Fe2+(aq)+ Co2+(aq)

The following reaction occurs spontaneously. 2 H+(aq)+ Ca(s) →\to→ Ca2+(aq)+ H2(g) Write the balanced oxidation half-reaction.

Write a balanced chemical equation for the oxidation of Cd(s)by concentrated nitric acid,producing NO2(g)and Cd2+(aq).

One kind of battery used in watches contains mercury(II)oxide.As current flows,the mercury(II)oxide is reduced to mercury. HgO(s)+ H2O( )+ 2 e- →\to→ Hg( )+ 2 OH-(aq) If 2.3 ×\times× 10-5 amperes flows continuously for 1200 days,what mass of Hg( )is produced?

In an electrolytic cell,reduction occurs at the ________ and oxidation occurs at the ________.

Balance the following half-reaction occurring in acidic solution. NO3-(aq) →\to→ HNO2(aq)

Write a balanced chemical equation for the overall reaction represented by the cell notation below. Al(s)| Al3+(aq)|| Br-(aq)| Br2(g)| Pt(s)

Given: Mn2+(aq)+ 2e- →\to→ Mn(s); E° = -1.18 V Cu2+(aq)+ 2e- →\to→ Cu(s); E° = 0.34 V Cr2O72-(aq)+ 14H+(aq)+ 6e- →\to→ 2Cr3+(aq)+ 7H2O(l); E° = 1.33 V Which of the following species is the strongest reducing agent?

Balance the following oxidation-reduction occurring in acidic solution. MnO4-(aq)+ Cr2+(aq) →\to→ Mn2+(aq)+ Cr3+(aq)

Which of the following statements is true concerning the voltaic cell shown below?

Balance the following half-reaction occurring in basic solution. MnO2(s) →\to→ Mn(OH)2(s)

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Write a balanced chemical equation for the following reaction in a basic solution. ClO^-(aq)+ Cr(OH)₃(s) $\to$ Cl^-(aq)+ CrO₄^2-(aq)

Assuming the following reaction proceeds in the forward direction, Fe³⁺(aq)+ Co(s) $\to$ Fe²⁺(aq)+ Co²⁺(aq)

The following reaction occurs spontaneously. 2 H⁺(aq)+ Ca(s) $\to$ Ca²⁺(aq)+ H₂(g) Write the balanced oxidation half-reaction.

Write a balanced chemical equation for the oxidation of Cd(s)by concentrated nitric acid,producing NO₂(g)and Cd²⁺(aq).

In an electrolytic cell,reduction occurs at the and oxidation occurs at the .

Balance the following half-reaction occurring in acidic solution. NO₃^-(aq) $\to$ HNO₂(aq)

Write a balanced chemical equation for the overall reaction represented by the cell notation below. Al(s)| Al³⁺(aq)|| Br^-(aq)| Br₂(g)| Pt(s)

Given: Mn²⁺(aq)+ 2e^- $\to$ Mn(s); E° = -1.18 V Cu²⁺(aq)+ 2e^- $\to$ Cu(s); E° = 0.34 V Cr₂O₇^2-(aq)+ 14H⁺(aq)+ 6e^- $\to$ 2Cr³⁺(aq)+ 7H₂O(l); E° = 1.33 V Which of the following species is the strongest reducing agent?

Balance the following oxidation-reduction occurring in acidic solution. MnO₄^-(aq)+ Cr²⁺(aq) $\to$ Mn²⁺(aq)+ Cr³⁺(aq)

Balance the following half-reaction occurring in basic solution. MnO₂(s) $\to$ Mn(OH)₂(s)