What will happen when solid Ag is added to a 1.0 M CuBr2 solution? Brą ()...
Solid NaI is slowly added to a solution that is 0.010 M in Cu+ and 0.010 M in Ag+.(a) Which compound will begin to precipitate first?(b) Calculate [Ag+] when CuI just begins to precipitate.(c) What percent of Ag+ remains in solution at this point?
Solid Nal is slowly added to a solution that is 0.0081 M Cu+ and 0.0099 M Ag+. Which compound will begin to precipitate first?Calculate [Ag+] when Cul just begins to precipitate. What percent of Agt remains in solution at this point?
Calculate the cell potential for the reaction below when the concentrations of ions are: [Ag+ ] = 0.010 M and [Cu2+] = 0.750 M, at 25 °C. Cu(s) + 2Ag+ (aq) --> Cu2+(aq) + 2Ag(s) Given the standard reduction potentials: Cu2+(aq) + 2e– → Cu(s) Eϴ = 0.34 V Ag+ (aq) + e– → Ag(s) Eϴ = 0.80 V (A) 0.35 V (B) 0.44 V (C) 0.46 V (D) 0.48 V (E) 0.57 V
Instead of using zinc, a student accidentally used a 1 M solution of silver (Ag). Based on the information in the table below, what would be the theoretical cell voltage, Eocell, when it is used in a galvanic cell with copper? Electrode Eo Ag+ + e- à Ag +0.80 V Cu2+ + 2e- à Cu +0.34 V Pb2+ + 2e- à Pb -0.13 V Zn2+ + 2e- à Zn -0.76 V Al3+ + 3e- à Al -1.66 V
KNO, salt bridge Mg Zn Ag 1.0 M Mg 1.0 M Zn2 1.0 M Cu 1.0 M Ag Reset Info 1.0 M ME LO M 2 1.0 MC 10 MA Reset Set up a cell that has a My electrode in a 1.0 M aqueous Mg? solution on the left side and a Ag electrode in a 1.0 M aqueous A solution on the right side. Add the salt bridge. What is the balanced net ionic equation for this reaction?...
An electrochemical cell consists of one half-cell that contains Ag(s) and Ag+(aq), and one half-cell that contains Cu(s) and Cu2+(aq). What species are produced at the electrodes under standard conditions? E° = +0.80 V Agt(aq) + e- → Ag(s) Cu2+(aq) + 2 e- → Cu(s) E° = +0.34 V O Ag(s) is formed at the cathode, and Cu(s) is formed at the anode. Ag(s) is formed at the cathode, and Cu2+ (aq) is formed at the anode. Cu(S) is formed...
Half-cell Potentials: Half Reaction: E value +0.80 V Agt + e → Ag Fe3+ + € → Fe2+ +0.77 v +0.34 V -0.13 V Cu2+ +2e → Cu Pb2+ + 2e - → Ib Ni2+ + 2e → Ni Cd2+ +2e → Cd -0.25 V -0.40 V Fe2+ + 2e → Fe -0.44 V Zn2+ + 2e → Zn -0.76 V Al3+ +3e → AI - 1.66 V Consider an electrochemical cell constructed from the following half cells, linked by...
How do the concentrations of Ag+ and SO42- change when more solid Ag2SO4 is added to the already saturated solution?
Which solution could oxidize Cu (s)? A) 1.0 M H+ B) 1.0 M Ag+ C) 1.0 M Ni2+ D) 1.0 M Zn2+ ----------------------------------------------------------------------------------------- For the following reaction, at 25 °C (room temperature), what is the entropy change of the universe? H2O(l) → H2O(s) A) ΔSuniv < 0 B) ΔSuniv > 0 C) ΔSuniv = 0
What is the standard emf of a galvanic cell made of a Co electrode in a 1.0 M Co(NO32 solution and a Al electrode in a 1.0 M AI(NO3)3 solution at 25°C? 0 cell Standard Reduction Potentials at 25°C Half-Reaction E(V +2.87 +2.07 +1.82 O,(g) 2H (aq)2e0(g)+HO Co3+(aq) + e-_? Co2+(aq) H,02(aq) + 2H"(aq) + 2e-_ 2H20 Cu2+(aq) + 2e-? Cu(s) AgCIs) + Ag(s) + CI(a) S02-(aq) + 4H'(aq) + 2e S02(g) + 2H20 Cu2+(aq) + e-_ Cu+(aq) Sn (aq)...