Using the activity list included in this problem, which element/ion is the most easily oxidized? Part...
a • Which of these half-cells would combine with the SHE to give the largest possible Eºcell value? • Fe3+/Fe, Ni2+/Ni, Cu2+/Cu = = = Zn2+ (aq) + 2e Cr+ (aq) + 3e Fe2+ (aq) + 2 Cd + (aq) + 2e Ni”* (aq) + 2e Sn²+ (aq) + 2e Pb2+ (aq) + 2 Fe+ (aq) + 3 2H(aq) + 2 Sn+ (aq) + 2e Cu²+ (aq) + e Cu²(aq) + 2e Zn(s) Cr(s) Fe(s) Cd(s) Ni(s) Sn(s) Pb(s) Fe(s)...
Using standard reduction potential in aqueous solutions at 25c Table, which substance is most likely to be oxidised by O2 (g) in acidic aqueous solution? Select one: a. Br2 (l) b. Br- (aq) c. Ni2+ (aq) d. Ag (s) e. Cu2+ (aq) Cathode (Reduction) Half-Reaction Standard Potential E° (volts) Li+(aq) + e- -> Li(s) -3.04 K+(aq) + e- -> K(s) -2.92 Ca2+(aq) + 2e- -> Ca(s) -2.76 Na+(aq) + e- -> Na(s) -2.71 Mg2+(aq) + 2e- -> Mg(s) -2.38 Al3+(aq)...
Using the table below: 19. Three combinations of metals are listed below, which combination would produce the largest voltage if they were used to construct an electrochemical cell? Copper (Cu) with zinc (Zn) Lead (Pb) with zinc (Zn) Lead (Pb) with cadmium (Cd) Liu lur the reaction between Zn and Cu2+ ions is 1.1030 V, we can use the known value for the half-cell potential for zinc to determine the half-cell potential for copper: Zn(s) → Zn2+(aq) + 2e +...
Based on the activity series, which one of the reactions below will occur? Most reactive to least reactive Mn> Zn > Cr> Fe > Co > Ni > Sn> Pb > H2 > Cu > Ag > Hg > Pt > Au © Zn (s) + Mnl2 (aq) → Zn2 (aq) + Mn (5) SnCl2 (aq) + Cu (s) — Sn (s) + CuCl2 (aq) O 2AgNO3(aq) + Pb (s) — 2Ag (s) + Pb(NO3)2 (aq) O 3Hg (1) +...
Using the activity series, predict whether the following reactions would be expected to proceed spontaneously. Cu (*) + 2Ag (aq) → Cu²+ (aq) + 2Ag (6) a.) Will proceed spontaneously b.) will not proceed spontaneously Using the activity series, predict whether the following reactions would be expected to proceed spontaneously. Mg (6) + Fe2+ → Mg²+ (aq) + Fe (3) (aq) a.) Will proceed spontaneously b.) will not proceed spontaneously Using the activity series, predict whether the following reactions would...
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)...
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) +...
NO−3(aq)+4H+(aq)+3e−→NO(g)+2H2O(l) E∘=0.96V ClO2(g)+e−→ClO−2(aq) E∘=0.95V Cu2+(aq)+2e−→Cu(s) E∘=0.34V 2H+(aq)+2e−→H2(g) E∘=0.00V Pb2+(aq)+2e−→Pb(s) E∘=−0.13V Fe2+(aq)+2e−→Fe(s) E∘=−0.45V You may want to reference (Pages 898 - 902) Section 19.4 while completing this problem. Part A Use data from the table above to calculate E∘cell for the reaction. Fe(s)+2H+(aq)→Fe2+(aq)+H2(g) Express your answer using two decimal places.
List the electrochemical series you developed from this lab based on the experimental values you obtained. Compare this to a published electrochemical series list, like the one in your eScience lab manual. Is yours different? If so, in what way is it different? Metal | Al (Trial 1) 2.5 g Al (Trial 2) Zn (Trial 1) Filter Paper Mass (9) Filter paper + Cu Mass (g) Cu Mass (g) Avg. Cu Mass (g) 2.3 g 2.9 g 0.6 g 0.4...
A certain half-reaction has a standard reduction potential +0.14 V. An engineer proposes using this half-reaction at the anode of a galvanic cell that must provide at least 0.80 V of electrical power. The cell will operate under standard conditions Note for advanced students: assume the engineer requires this half-reaction to happen at the anode of the cell. Is there a minimum standard reduction potential that the hall reaction used at the cathode of this cell can have? ves, there...