Homework Answers
Your order and balance reactions are
Strong oxidising agent means elements have high reduction potential.
F2 + 2e = F2
Au3+ + 3e = Au
Fe3+ + e = Fe2+
I2 + 2e = 2 I-
Cu2+ + e = Cu+
2 H+ + 2e = H2
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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...
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 12(s) + → 21 (aq) E° = +0.53 V 4e Fe (aq) + → Fez (aq) E° = +0.77 V F2(g) + 2F-(aq) E° = +2.87 V AHOROD WWWWWWWWWWWWWWWWWWWWWWWWWWWWWWY Au3+ (aq) + Au(s) E° = +1.50 V 2H'(aq) + - + H2(g) E°...
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 5e Ag (aq) Ag(s) E=+0.80 V 2e Sn4 (aq) Sn2 (aq) E = +0.13 V Ca2 (aq) Зе Ca(s) E = -2.87 V Cr(s) E -0.74 V Cr3 (aq) 4e -2F (aq) E= +2.87 V F2(g) e » 21-(aq) E = +0.53 V 12(s)...
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° =...
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 caidizing potential to strongest reducing potential Strongest Oxidizing Potential Drag the text blocks below into their correct order. Fes (aq) + + Fe (aq) = +0.77 V 2H(aq) + * H(o) +0.00 V Natal - Nais) E.-2.71 V Co (aq) + -Co" (aq) +1.82 V Br(0) + - 2Br(ad E - +1.07 v Nad) - Nis) E--0.25 V Strongest Reducting Potential
Consider the following species. Cut Ce3+ Ag+ Zn2+ What is the standard potential for the reaction...
Consider the following species. Cut Ce3+ Ag+ Zn2+ What is the standard potential for the reaction of Cut with Zn2+ to produce Cu2+ and Zn? E = 0.28 X v Will Cut be able to reduce Zn2+ to Zn? no (yes or no) What is the standard potential for the reaction of Ce3+ with Ag! to produce Ag? Ex= 0.90 x v Will Cell be able to reduce Ag! to Ag? yes (yer or no) Ered (V) 0.68 0.52 0.40...
Table 20.1 Half Reaction E°(V). F2 (g) + 2e →2F (aq) +2.87 Cl2 (g) + 2e...
Table 20.1 Half Reaction E°(V). F2 (g) + 2e →2F (aq) +2.87 Cl2 (g) + 2e → 2CV (aq) +1.359 Br2 (1) + 2e → 2Br (aq) +1.065 O2 (g) + 4H+ (aq) + 4e → 2H20 (1)+1.23 Agt te → Ag (s) +0.799 Fe3+ (aq) + € → Fe2+ (aq) +0.771 12 (s) + 2e → 21+ (aq) +0.536 Cu2+ + 2e → Cu(s) +0.34 2H+ + 2e → H2 (g) Pb2+ + 2e → Pb (s) -0.126 Ni2+...
A chemist designs a galvanic cell that uses these two half-reactions: standard reduction potential half-reaction +...
A chemist designs a galvanic cell that uses these two half-reactions: standard reduction potential half-reaction + O2(9)+4 H (aq)+4e' 2H20) = 1.23 V red Ered Fe+. (аq) Fe3(aq)+e = +0.771 V Answer the following questions about thiss cell Write a balanced equation for the half-reaction that happens at the cathode Write a balanced equation for the half-reaction that happens at the anode Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous...
Fill in the Blanks Ered (V) 0.68 0.52 0.40 0.34 0.16 0 Half Reaction Ered (V)...
Fill in the Blanks Ered (V) 0.68 0.52 0.40 0.34 0.16 0 Half Reaction Ered (V) Half Reaction F2+2e →2F 2.87 02 + 2H+ 2e →H,O, Ag?+ e → Ag 1.99 Cute → Cu Code → CO2 1.82 O2 + 2H,0 + 4e → 40H H,02 + 2H+ + 2e → 2H,0 1.78 Cu2+ + 2e → Cu Ce+ + → Ce+ 1.70 Cu2+ e → Cu PbO, + 4H* +502 +2e → PbSO4 + 2H,0 1.69 2H*+2e → H2...
2.87 Ered® (V) 0.68 0.52 0.40 0.34 0.16 Half Reaction F,+ 2e →2F Ag* + e...
2.87 Ered® (V) 0.68 0.52 0.40 0.34 0.16 Half Reaction F,+ 2e →2F Ag* + e → Ag Co3 + e + CO2- H2O2 + 2H+ + 2e → 2H,0 Ce4+ + e → Ce+ PbO, + 4H+ + SO42- + 2e → PbSO, + 2H,0 Mno, + 4H+ + 3e → MnO2 + 2H,0 2e + 2H+ + 10, → 103 + H2O Mn0, +8H+ + 5e → Mn2+ + 4H,0 Aul+ + 3e → Au Cl2 + 2e...
12. Using two half reactions that have NEGATIVE standard reduction potentials results results in a battery...
12. Using two half reactions that have NEGATIVE standard reduction potentials results results in a battery that... Reduction Half-Reaction F2(g) + 2e →2F(aq) S2082 (aq) + 2e- → 25042 (aq) O2(g) + 4H+ (aq) + 4e → 2H2O(1) Br2(1) + 2e + 2Br (aq) Agt(aq) + e → Ag(s) Fe3+ (aq) + e- → Fe2+ (aq) 126) + 2e → 21 (aq) Cu2+ (aq) + 2e → Cu(s) Sn4+ (aq) + 2e → Sn2+ (aq) S(s) + 2H+ (aq) +...
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 12(s) + → 21 (aq) E° = +0.53 V 4e Fe (aq) + → Fez (aq) E° = +0.77 V F2(g) + 2F-(aq) E° = +2.87 V AHOROD WWWWWWWWWWWWWWWWWWWWWWWWWWWWWWY Au3+ (aq) + Au(s) E° = +1.50 V 2H'(aq) + - + H2(g) E°...
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 5e Ag (aq) Ag(s) E=+0.80 V 2e Sn4 (aq) Sn2 (aq) E = +0.13 V Ca2 (aq) Зе Ca(s) E = -2.87 V Cr(s) E -0.74 V Cr3 (aq) 4e -2F (aq) E= +2.87 V F2(g) e » 21-(aq) E = +0.53 V 12(s)...
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° =...
Complete each of the following half-reactions with the correct number of electrons and then arrange them from strongest caidizing potential to strongest reducing potential Strongest Oxidizing Potential Drag the text blocks below into their correct order. Fes (aq) + + Fe (aq) = +0.77 V 2H(aq) + * H(o) +0.00 V Natal - Nais) E.-2.71 V Co (aq) + -Co" (aq) +1.82 V Br(0) + - 2Br(ad E - +1.07 v Nad) - Nis) E--0.25 V Strongest Reducting Potential
Consider the following species. Cut Ce3+ Ag+ Zn2+ What is the standard potential for the reaction of Cut with Zn2+ to produce Cu2+ and Zn? E = 0.28 X v Will Cut be able to reduce Zn2+ to Zn? no (yes or no) What is the standard potential for the reaction of Ce3+ with Ag! to produce Ag? Ex= 0.90 x v Will Cell be able to reduce Ag! to Ag? yes (yer or no) Ered (V) 0.68 0.52 0.40...
Table 20.1 Half Reaction E°(V). F2 (g) + 2e →2F (aq) +2.87 Cl2 (g) + 2e → 2CV (aq) +1.359 Br2 (1) + 2e → 2Br (aq) +1.065 O2 (g) + 4H+ (aq) + 4e → 2H20 (1)+1.23 Agt te → Ag (s) +0.799 Fe3+ (aq) + € → Fe2+ (aq) +0.771 12 (s) + 2e → 21+ (aq) +0.536 Cu2+ + 2e → Cu(s) +0.34 2H+ + 2e → H2 (g) Pb2+ + 2e → Pb (s) -0.126 Ni2+...
A chemist designs a galvanic cell that uses these two half-reactions: standard reduction potential half-reaction + O2(9)+4 H (aq)+4e' 2H20) = 1.23 V red Ered Fe+. (аq) Fe3(aq)+e = +0.771 V Answer the following questions about thiss cell Write a balanced equation for the half-reaction that happens at the cathode Write a balanced equation for the half-reaction that happens at the anode Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous...
Fill in the Blanks Ered (V) 0.68 0.52 0.40 0.34 0.16 0 Half Reaction Ered (V) Half Reaction F2+2e →2F 2.87 02 + 2H+ 2e →H,O, Ag?+ e → Ag 1.99 Cute → Cu Code → CO2 1.82 O2 + 2H,0 + 4e → 40H H,02 + 2H+ + 2e → 2H,0 1.78 Cu2+ + 2e → Cu Ce+ + → Ce+ 1.70 Cu2+ e → Cu PbO, + 4H* +502 +2e → PbSO4 + 2H,0 1.69 2H*+2e → H2...
2.87 Ered® (V) 0.68 0.52 0.40 0.34 0.16 Half Reaction F,+ 2e →2F Ag* + e → Ag Co3 + e + CO2- H2O2 + 2H+ + 2e → 2H,0 Ce4+ + e → Ce+ PbO, + 4H+ + SO42- + 2e → PbSO, + 2H,0 Mno, + 4H+ + 3e → MnO2 + 2H,0 2e + 2H+ + 10, → 103 + H2O Mn0, +8H+ + 5e → Mn2+ + 4H,0 Aul+ + 3e → Au Cl2 + 2e...
12. Using two half reactions that have NEGATIVE standard reduction potentials results results in a battery that... Reduction Half-Reaction F2(g) + 2e →2F(aq) S2082 (aq) + 2e- → 25042 (aq) O2(g) + 4H+ (aq) + 4e → 2H2O(1) Br2(1) + 2e + 2Br (aq) Agt(aq) + e → Ag(s) Fe3+ (aq) + e- → Fe2+ (aq) 126) + 2e → 21 (aq) Cu2+ (aq) + 2e → Cu(s) Sn4+ (aq) + 2e → Sn2+ (aq) S(s) + 2H+ (aq) +...
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