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Question 30 1 pts Rank the following in order of strength as a reducing agent. E°...
Rank the following in order of strength as a reducing agent. EM Ag (aq) +e-Ag(s) +0.80...
Rank the following in order of strength as a reducing agent. EM Ag (aq) +e-Ag(s) +0.80 Alaq) + 3e-4Alls) 1.66 Aul(aq) + 3e- 4 Au(s) +1.50 Co2(aq) + 2e- 4 Co(s) -0.28 Cr2(aq) + 2e-4Cr(s) -0.91 Ni2(aq) + 2e-4Nils) -0.25 P2*(aq) + 2e- A Pt(s) +1.19 Sn2(aq) + 2e-4Sn(s) -0.14 Ag [Choose) ΑΙ (Choose) Со [Choose)
Complete each of the following half-reactions with the correct number of electrons and then arrange them...
Complete each of the following half-reactions with the correct number of electrons and then arrange them from strongest oxidizing potential to strongest reducing potential. Strongest Oxidizing Potential Drag the text blocks below into their correct order. 2e Au3+ (aq) + e + Au(s) E° = +1.50 V 5e Sn2+ (aq) + e + Sn(s) E° = -0.14 V 6e Ca2+ (aq) + 2e + Ca(s) E° = -2.87 V wwwwwwwwwwwwwwwwwwwwwwwwwwwwwwwww 4e Co3+ (aq) + 2e + Co2+ (aq) E° =...
Use the tabulated electrode potentials to calculate K for the oxidation of nickel by H+: Ni(s)+2H+(aq)→Ni2+(aq)+H2(g)...
Use the tabulated electrode potentials to calculate K for the oxidation of nickel by H+: Ni(s)+2H+(aq)→Ni2+(aq)+H2(g) Express your answer using two significant figures. Standard reduction half-cell potentials at 25∘C Half-reaction E∘ (V) Half-reaction E∘ (V) Au3+(aq)+3e−→Au(s) 1.50 Fe2+(aq)+2e−→Fe(s) −0.45 Ag+(aq)+e−→Ag(s) 0.80 Cr3+(aq)+e−→Cr2+(aq) −0.50 Fe3+(aq)+3e−→Fe2+(aq) 0.77 Cr3+(aq)+3e−→Cr(s) −0.73 Cu+(aq)+e−→Cu(s) 0.52 Zn2+(aq)+2e−→Zn(s) −0.76 Cu2+(aq)+2e−→Cu(s) 0.34 Mn2+(aq)+2e−→Mn(s) −1.18 2H+(aq)+2e−→H2(g) 0.00 Al3+(aq)+3e−→Al(s) −1.66 Fe3+(aq)+3e−→Fe(s) −0.036 Mg2+(aq)+2e−→Mg(s) −2.37 Pb2+(aq)+2e−→Pb(s) −0.13 Na+(aq)+e−→Na(s) −2.71 Sn2+(aq)+2e−→Sn(s) −0.14 Ca2+(aq)+2e−→Ca(s) −2.76 Ni2+(aq)+2e−→Ni(s) −0.23 Ba2+(aq)+2e−→Ba(s) −2.90 Co2+(aq)+2e−→Co(s) −0.28 K+(aq)+e−→K(s) −2.92 Cd2+(aq)+2e−→Cd(s)...
Consider the following half-reactions and their reduction potentials (volt Au (aq) +3e- Au(s) +1....
Consider the following half-reactions and their reduction potentials (volt Au (aq) +3e- Au(s) +1.50 petad) +2 e' → Pt(s) +1.20 Co2+(aq) + 2 e' → Cols) -0.28 Mn? (aq)+2e Mn/s) -1.18 Which one of the following statements is correct? O A Ptis) can reduce Ht in aqueous solution OB. P (ag) can be reduced by Cols) OC. A (aa) is the weakest oxidizing agent D. Mn? (aq) can oxidize Au (s) OE. Auls) is the strongest reducing agent ous Save...
Use the standard reduction potentials from the following table to choose the weakest reducing agent among...
Use the standard reduction potentials from the following table to choose the weakest reducing agent among those shown below. Ag+(aq) + - + Ag(s) E° = 0.80 V Cu2+(aq) + 2e → Cu(s) E° = 0.34 V Ni2+(aq) + 2e + Ni(s) E° = -0.26 V Cr3+(aq) + 3e- → Cr(s) E° = -0.74 V Mn2+(aq) + 2e → Mn(s) E° = -1.19 V О Ni(s) Ag(s) Cr(s) Mn(s) Cu(s)
A) Use tabulated electrode potentials to calculate ΔG∘ for the reaction. 2K(s)+2H2O(l)→H2(g)+2OH−(aq)+2K+(aq) B) (Refer to the...
A) Use tabulated electrode potentials to calculate ΔG∘ for the reaction. 2K(s)+2H2O(l)→H2(g)+2OH−(aq)+2K+(aq) B) (Refer to the following standard reduction half-cell potentials at 25∘C: VO2+(aq)+Ni2+(aq)2H+(aq)++2e−e−→ →Ni(s)VO2+(aq) +H2O(l)E∘=−0.23V E∘=0.99V) An electrochemical cell is based on these two half-reactions: Oxidation:Reduction:Ni(s)VO2+(aq,0.024M)+2H+(aq,1.4M)+e−→→Ni2+(aq,1.8M)+2e−VO2+(aq,1.8M)+H2O(l) Calculate the cell potential under these nonstandard concentrations. C) Standard reduction half-cell potentials at 25∘C Half-reaction E∘ (V ) Half-reaction E∘ (V ) Au3+(aq)+3e−→Au(s) 1.50 Fe2+(aq)+2e−→Fe(s) − 0.45 Ag+(aq)+e−→Ag(s) 0.80 Cr3+(aq)+e−→Cr2+(aq) − 0.50 Fe3+(aq)+3e−→Fe2+(aq) 0.77 Cr3+(aq)+3e−→Cr(s) − 0.73 Cu+(aq)+e−→Cu(s) 0.52 Zn2+(aq)+2e−→Zn(s) − 0.76...
Find the best reducing agent from Cu+, Ag+ F2 and Fe3+ #1. In the reduction table...
Find the best reducing agent from Cu+, Ag+ F2 and Fe3+
#1. In the reduction table i can see several repeated values of
Fe3+ one is equal to 0.77v and the second one is equal to -0.036v
so, which one do I choose? Please explain.
#2.If I'm asked to find the best oxidation agent, from the
values already provided (Cu+, Ag+ F2 and Fe3+) which one would it
be? and how would I decide from repeated values, like in #1,...
Consider the following standard reduction potentials in acid solution:
Consider the following standard reduction potentials in acid solution:E^o(V)Al3+ + 3e– ? Al(s) –1.66AgBr(s) + e– ? Ag(s) + Br– +0.07Sn4+ + 2e– ? Sn2+ +0.14Fe3+ + e– ? Fe2+ +0.77The strongest reducing agent among those shown above is
Standard reduction half-cell potentials at 25°C E (V) E (V) 1.50 -0.45 0.80 -0.50 0.77 -0.73...
Standard reduction half-cell potentials at 25°C E (V) E (V) 1.50 -0.45 0.80 -0.50 0.77 -0.73 0.52 -0.76 0.34 -1.18 Half-reaction Aut (aq) + 3e +Au(s) Ag+ (aq) + +Ag(s) Fe3+ (aq) +34 Fo+ (aq) Cut(aq) + Cu(s) Cu²+ (aq) + 2e +Cu(s) 2H+ (aq) - 2e +H2 (6) Fe3+ (aq) + 3e Fe(s) Pb2+ (aq) + 2e →Pb(s) Sn-(aq) + 2e +Sn(s) Ni2+ (aq) + 2e →Ni(s) Co2(aq) +2e + Co(s) ca? (aq) + 2e +Cd(s) 0.00 Half-reaction Fe(aq)...
4. Write a balanced equation from each cell notation, then calculate thee of the cell, is...
4. Write a balanced equation from each cell notation, then calculate thee of the cell, is it spontaneous or nonspontaneous? A. Cr(s) Crot || Cui Cu(s) B. Al(s) Al* | Ce Ce Pt C. Cu (s) Cu? || Al Al (s) Useful information: F= 96485 J/V mol electrons, AG ----F-Ecell AG --RTINK: Ece 0.0592/n*logK; EcellEcett -0.0592/n*logQ Ce (aq) + Ag+ (aq) + e Fet (aq) + Cu" (aq) + Cu (aq) + 2e 2H(aq) + 2 Pb (aq) + 2e...
Rank the following in order of strength as a reducing agent. EM Ag (aq) +e-Ag(s) +0.80 Alaq) + 3e-4Alls) 1.66 Aul(aq) + 3e- 4 Au(s) +1.50 Co2(aq) + 2e- 4 Co(s) -0.28 Cr2(aq) + 2e-4Cr(s) -0.91 Ni2(aq) + 2e-4Nils) -0.25 P2*(aq) + 2e- A Pt(s) +1.19 Sn2(aq) + 2e-4Sn(s) -0.14 Ag [Choose) ΑΙ (Choose) Со [Choose)
Complete each of the following half-reactions with the correct number of electrons and then arrange them from strongest oxidizing potential to strongest reducing potential. Strongest Oxidizing Potential Drag the text blocks below into their correct order. 2e Au3+ (aq) + e + Au(s) E° = +1.50 V 5e Sn2+ (aq) + e + Sn(s) E° = -0.14 V 6e Ca2+ (aq) + 2e + Ca(s) E° = -2.87 V wwwwwwwwwwwwwwwwwwwwwwwwwwwwwwwww 4e Co3+ (aq) + 2e + Co2+ (aq) E° =...
Consider the following half-reactions and their reduction potentials (volt Au (aq) +3e- Au(s) +1.50 petad) +2 e' → Pt(s) +1.20 Co2+(aq) + 2 e' → Cols) -0.28 Mn? (aq)+2e Mn/s) -1.18 Which one of the following statements is correct? O A Ptis) can reduce Ht in aqueous solution OB. P (ag) can be reduced by Cols) OC. A (aa) is the weakest oxidizing agent D. Mn? (aq) can oxidize Au (s) OE. Auls) is the strongest reducing agent ous Save...
Use the standard reduction potentials from the following table to choose the weakest reducing agent among those shown below. Ag+(aq) + - + Ag(s) E° = 0.80 V Cu2+(aq) + 2e → Cu(s) E° = 0.34 V Ni2+(aq) + 2e + Ni(s) E° = -0.26 V Cr3+(aq) + 3e- → Cr(s) E° = -0.74 V Mn2+(aq) + 2e → Mn(s) E° = -1.19 V О Ni(s) Ag(s) Cr(s) Mn(s) Cu(s)
Find the best reducing agent from Cu+, Ag+ F2 and Fe3+
#1. In the reduction table i can see several repeated values of
Fe3+ one is equal to 0.77v and the second one is equal to -0.036v
so, which one do I choose? Please explain.
#2.If I'm asked to find the best oxidation agent, from the
values already provided (Cu+, Ag+ F2 and Fe3+) which one would it
be? and how would I decide from repeated values, like in #1,...
Standard reduction half-cell potentials at 25°C E (V) E (V) 1.50 -0.45 0.80 -0.50 0.77 -0.73 0.52 -0.76 0.34 -1.18 Half-reaction Aut (aq) + 3e +Au(s) Ag+ (aq) + +Ag(s) Fe3+ (aq) +34 Fo+ (aq) Cut(aq) + Cu(s) Cu²+ (aq) + 2e +Cu(s) 2H+ (aq) - 2e +H2 (6) Fe3+ (aq) + 3e Fe(s) Pb2+ (aq) + 2e →Pb(s) Sn-(aq) + 2e +Sn(s) Ni2+ (aq) + 2e →Ni(s) Co2(aq) +2e + Co(s) ca? (aq) + 2e +Cd(s) 0.00 Half-reaction Fe(aq)...
4. Write a balanced equation from each cell notation, then calculate thee of the cell, is it spontaneous or nonspontaneous? A. Cr(s) Crot || Cui Cu(s) B. Al(s) Al* | Ce Ce Pt C. Cu (s) Cu? || Al Al (s) Useful information: F= 96485 J/V mol electrons, AG ----F-Ecell AG --RTINK: Ece 0.0592/n*logK; EcellEcett -0.0592/n*logQ Ce (aq) + Ag+ (aq) + e Fet (aq) + Cu" (aq) + Cu (aq) + 2e 2H(aq) + 2 Pb (aq) + 2e...
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