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Refer to this table of reduction potentials to answer the questions. Reduction half-reaction Potential (V) F2(g)+2e−→2F−(aq)...

Refer to this table of reduction potentials to answer the questions. Reduction half-reaction Potential (V) F2(g)+2e−→2F−(aq) +2.87 O2(g)+4H+(aq)+4e−→2H2O(l) +1.23 Br2(l)+2e−→2Br−(aq) +1.07 Ag++e−→Ag(s) +0.80 2H2O(l)+2e−→H2(g)+2OH−(aq) −0.83 Na+(aq)+e−→Na(s) −2.71 What is produced at each electrode in the electrolysis of an aqueous solution of both NaBr and AgF? Drag the appropriate items to their respective bins. Na(s) H2(g) F2(g) O2(g) Ag(s) Br2(l)

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queen_honey_blossom answered 4 months ago
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Refer to this table of reduction potentials to answer the questions. Reduction half-reaction Potential (V) F2(g)+2e−→2F−(aq)...
Refer to this table of reduction potentials to answer the questions. Reduction half-reaction Potential (V) F2(g)+2e−→2F−(aq) +2.87 O2(g)+4H+(aq)+4e−→2H2O(l) +1.23 Br2(l)+2e−→2Br−(aq) +1.07 Ag++e−→Ag(s) +0.80 2H2O(l)+2e−→H2(g)+2OH−(aq) −0.83 Na+(aq)+e−→Na(s) −2.71 What is produced at each electrode in the electrolysis of an aqueous solution of both NaBr and AgF? H2(g), Ag(s), Na(s), O2(g), Br(l), F2(g) sort to respective designation below Anode, Cathode, Not produced
a) Consider the following half-reactions: Half-reaction E° (V) F2(g) + 2e- 2F-(aq) 2.870V 2H+(aq) + 2e- H2(g) 0.000V Zn2+(aq) + 2e- Zn(s) -0.763V
13)) a) Consider the following half-reactions: Half-reaction E° (V) F2(g) + 2e- 2F-(aq) 2.870V 2H+(aq) + 2e- H2(g) 0.000V Zn2+(aq) + 2e- Zn(s) -0.763V (1) The weakest oxidizing agent is: enter formula (2) The strongest reducing agent is: (3) The strongest oxidizing agent is: (4) The weakest reducing agent is: (5) Will F-(aq) reduce Zn2+(aq) to Zn(s)? (6) Which species can be reduced by H2(g)? If none, leave box blank. b)) Consider the following half-reactions: Half-reaction E° (V) Ag+(aq) +...
The standard reduction potential for the F2/2F- redox couple is +2.87 V This means that: F2...
The standard reduction potential for the F2/2F- redox couple is +2.87 V This means that: F2 is a good reducing agent F2 is a good oxidizing agent F- is a good reducing agent F- is a good oxidizing agent
Reduction Half Reaction E (V) Ag2MoO4(s) + 2e- ---> 2 Ag(s) + MoO42-(aq) 0.4573 V Ag+(aq)...
Reduction Half Reaction E (V) Ag2MoO4(s) + 2e- ---> 2 Ag(s) + MoO42-(aq) 0.4573 V Ag+(aq) + e- ---> Ag(s) 0.7996 V a.) Calculate the mass in grams of Ag2MoO4(s) that will dissolve in 2.0 L of water. b.) Calcilate the cell potential of: Ag(s) | Ag2MoO4(s) | MoO42-(aq) (0.010 M) || Ag+(aq) (0.010M) | Ag (s)
Using the following reduction potentials: I2(s) + 2e- <---> 2I-(aq) E0 = 0.535 V I2 (aq)...
Using the following reduction potentials: I2(s) + 2e- <---> 2I-(aq) E0 = 0.535 V I2 (aq) +2e- <---> 2I-(aq) E0 = 0.620 V I3-(aq) + 2e- <---> 3I-(aq) E0 = 0.535 V a) Calculate the equilibrium constant for I2(aq) + I-(aq) <---> I3-(aq) b) Calculate the equilibrium constant for I2(s) + I-(aq) <---> I3-(aq) c) Calculate the solubility (g/L) of I2(s) in water.
Reduction half-reaction E∘ (V) Ag+(aq)+e−→Ag(s) 0.80 Cu2+(aq)+2e−→Cu(s) 0.34 Sn4+(aq)+4e−→Sn(s) 0.15 2H+(aq)+2e−→H2(g) 0 Ni2+(aq)+2e−→Ni(s) −0.26 Fe2+(aq)+2e−→Fe(s) −0.45...
Reduction half-reaction E∘ (V) Ag+(aq)+e−→Ag(s) 0.80 Cu2+(aq)+2e−→Cu(s) 0.34 Sn4+(aq)+4e−→Sn(s) 0.15 2H+(aq)+2e−→H2(g) 0 Ni2+(aq)+2e−→Ni(s) −0.26 Fe2+(aq)+2e−→Fe(s) −0.45 Zn2+(aq)+2e−→Zn(s) −0.76 Al3+(aq)+3e−→Al(s) −1.66 Mg2+(aq)+2e−→Mg(s) −2.37 1) Use the table of standard reduction potentials given above to calculate the equilibrium constant at standard temperature (25 ∘C) for the following reaction: Fe(s)+Ni2+(aq)→Fe2+(aq)+Ni(s) 2) Calculate the standard cell potential (E∘) for the reaction X(s)+Y+(aq)→X+(aq)+Y(s) if K = 3.80×10−4. Express your answer to three significant figures and include the appropriate units.
Half-reaction E° (V) Hg2+(aq) + 2e- -----> Hg(l) 0.855V Ni2+(aq) + 2e- -----> Ni(s) -0.250V Zn2+(aq)...
Half-reaction E° (V) Hg2+(aq) + 2e- -----> Hg(l) 0.855V Ni2+(aq) + 2e- -----> Ni(s) -0.250V Zn2+(aq) + 2e- ----->  Zn(s) -0.763V (1) The weakest oxidizing agent is: ___   enter formula (2) The strongest reducing agent is: ___ (3) The strongest oxidizing agent is:___ (4) The weakest reducing agent is: ___ (5) Will Zn(s) reduce Hg2+(aq) to Hg(l)? _____(yes)(no) (6) Which species can be oxidized by Ni2+(aq)? ___ If none, leave box blank.
Selective Oxidation The standard reduction potential for the half-reaction Sn4+ + 2e- --> Sn2+ is +0.15...
Selective Oxidation The standard reduction potential for the half-reaction Sn4+ + 2e- --> Sn2+ is +0.15 V. Consider data from the table of standard reduction potentials for common half-reactions, in your text. For a galvanic cell under standard conditions, which of the following cathodic half reactions would produce, at the anode, a spontaneous oxidation of Sn to Sn2+ but not Sn2+ to Sn4+. (Yes or No) 1. Sn4+ + 2e- --> Sn2+ 2. PbSO4 + 2e- --> Pb + SO42-...
Half-reaction E° (V) Br2(l) + 2e- 2Br-(aq) 1.080V Sn2+(aq) + 2e- Sn(s) -0.140V Al3+(aq) + 3e-...
Half-reaction E° (V) Br2(l) + 2e- 2Br-(aq) 1.080V Sn2+(aq) + 2e- Sn(s) -0.140V Al3+(aq) + 3e- Al(s) -1.660V (1) The weakest oxidizing agent is: enter formula (2) The strongest reducing agent is: (3) The strongest oxidizing agent is: (4) The weakest reducing agent is: (5) Will Al(s) reduce Br2(l) to Br-(aq)? (6) Which species can be oxidized by Sn2+(aq)? If none, leave box blank.
Explain why the sum of the potentials for the half-reactions Sn2+(aq) + 2e− → Sn(s) and...
Explain why the sum of the potentials for the half-reactions Sn2+(aq) + 2e− → Sn(s) and Sn4+(aq) + 2e− → Sn2+(aq) does not equal the potential for the reaction Sn4+(aq) + 4e−→ Sn(s). What is the net cell potential? Compare the values of ΔG° for the sum of the potentials and the actual net cell potential.
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