u. 1 an anode? N 3. Write the half-reaction at each electrode if cells containing following...
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Experiment 23 Electrochemical Cells Postlaboratory Questions Lell potentials are state functions so the cell potential for Zn (s)[Zn- (aq) Fe (aq me added to the cell potential for Fe+ (aq) Fe (s) Cu²+ (aq)Cu (s) should equal the cell potential of Zn (s)IZn2+ (aq)||Cu2+ (aq) Cu (s). a. Does this hold using the theoretical cell potentials? b. Does this hold using the experimentally determined cell potentials? c. Why might the two differ? 2....
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A galvanic cell is prepared using the following two half-cells: (i) MnO4 (0.273 M), Mn2+ (0.167 M), and H+ (1.0 M), and (ii) Fe2+ (0.247 M) and Fe3+ (0.389 M). The standard reduction potentials for the two half cells are: Mnoa + 8H+ + 5e – Mn2+ + 4H20 E° = 1.507 V Fe3+ + e- Fe2+ E° = 0.770 V a) Calculate the voltage for this galvanic cell. b) Write the balanced equation for...
Write the half-reactions as they occur at each electrode and the net cell reaction for this electrochemical cell containing indium and cadmium: ln(s)|ln^3+ (aq)||Cd^2+ (aq)|Cd(s) anode: Ln rightarrow Ln^3+ + 3e^- cathode: Cd^2+ + 2e^- rightarrow Cd net cell reaction: 2ln + 3ed^2+ rightarrow 3ed + 2ln^3+
Write the half-reactions as they occur at each electrode and the net cell reaction for this electrochemical cell containing indium and cadmiunm anode: In (aa)+3eInls) cathode: Cd (aq)+2e cals) net cell reaction:21n (aq+3Cdls)2lnls)+3cd (aq)
Please combine the Mn electrode half reaction with the Ag
electrode half reaction and write the complete redox reaction using
date from table 8.1. Indicate which is the oxidizing and which is
the reducing agent.
b. Calculate the EMF when the reaction quotient (Q) =
]Mn2+]/[Ag+]^2 = 10^-5
Reducing agent Half-reaction E0 (volts) -2.93 2.87 Ca Na Mg Mn Zn Fe Ni Pb Ca Ca2++2e Na → Na++e- -2.36 Mn Mn++2e Zn Zn2++2e Fe → Fe2++ 2e- NiNi2++2e- -0.76 -0.47...
19 20 Question 16 Half-cell Potentials: Half Reaction: E' value + 0.80 V +0.77 V Agte → AS Fe3+ + + Fe2+ Cu2+ 2e → Cu Pb2+ + 2e → Pb +0.34 V -0.13 V Ni2+ + 2e → NI -0.25 V - 0.40 V Cd2+ +2e → ca Fe2+ + 2e → Fe Zn2+ + 2e → Zn -0.44 V - 0.76 V A13+ +3 → AI - 1.66 V Consider an electrochemical cell constructed from the following half...
For each of the following galvanic cells (1) write out the conventional (overall) cell reaction and the two half reactions of which it is composed, (2) calculate the actual E for each cell a. Pt Br (aq) (0.75 M), Br2 (aq) (0.1 M)||Ci' (0.6 M) Cl2(Q) (0.2 atm), Pt b. Ag AgCl(), Cl- (0.5 M) || MinO4 (0.02 M), Mn2+ (0.15 M), H* (0.1 M) | Pt c. Cd Ca(NH3)42+ (0.04 M), NH3 (aq) (0.1 M) || Fe3+ (0.6 M),...
(1) Identify each of the following half-reactions as either an oxidation half-reaction or a reduction half-reaction. Half-reaction Identification Fe2+(aq)--> Fe3+(aq) + e- Br2(l) + 2e- --> 2Br-(aq) (2) Write a balanced equation for the overall redox reaction. (Use smallest possible integer coefficients.)
Write the half-reactions as they occur at each electrode and the net cell reaction for this electrochemical cell containing copper and silver: Cu(s)|Cu2 (aq)||Ag (aq)|Ag(s) Anode? Cathode? Net cell reaction?
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ratory Assignment Experiment 15 chemistry (Galvanic Cells) Name Rox couples 2 - -> 2Br le ......... Fe +2 2e ....-> Sn 3e > Cr +1.07 +0.77 -0.14 -1.0V der the cell consisting of the Fe* (IM) Fe**and and Bry(lamy B (IM) redox couples. ile the reduction half-reaction and the corresponding standard reduction potential and indicate which electrode does this occur at. Write the oxidation half reaction and the corresponding oxidation potential indicate which electrode does this occur at. Write...