Consider the following cell reaction: Pb^2+ + Zn rightarrow Pb + Zn^2 + E degree =...
Pb^2+ +2e- __> Pb e=-0.13V Ag+ +1e-__> Ag e=+0.80V Pb(s)| Pb2+ (1M) || Ag+ (1M) | Ag(s) Determine which of the following statements about the cell shown are True or False. The silver half-cell is the cathode. True False The mass of the silver electrode is decreasing. True False Anions move to the silver half-cell. True False Electrons are spontaneously produced in the lead half-cell. True False The cell, as represented by the line notation, is a voltaic cell. True False The standard cell potential,...
A certain electrochemical cell has for its cell reaction: Zn + HgO rightarrow ZnO + Hg Which is the half-reaction occurring at the anode? a) HgO + 2e^- rightarrow Hg + O_2- b) Zn^2+ + 2e^- rightarrow Zn c) Zn rightarrow Zn^2+ + 2e^- d) ZnO + 2e^- rightarrow Zn
EXPERIMENT 1: List the measured potential for Cell 3: Zn|Zn(NO3)2 || Pb(NO3)2|Pb. Based on your observations, do you expect given electrochemical cell to be spontaneous or nonspontaneous? Explain your answer. Pb|Pb(NO3)2||Zn|Zn(NO3)2 EXPERIMENT 1: What would happen to the measured cell potentials if 30 mL solution was used in each half-cell instead of 25 mL? EXPERIMENT 1: Calculate the theoretical standard cell potential for the electrochemical cell that includes the reaction. Mn+Pb2+⟶Mn2++Pb The standard reduction potentials for each half reaction are...
data collected Cu(NO3)2 | Zn(NO3)2 = 0.999 V Pb | 1.0 M Pb(NO3)2 || 1.0 M Zn(NO3)2 | Zn = 0.396 V PART B: REDUCTION POTENTIALS 1. Report the measured cell potential for each galvanic cell and state which electrode corresponds to the cathode and which to the anode. 2. Given E = -0.76 V for the Zn/Zn half-cell, and your measured Ecell, calculate the reduction potential at the Cu and Pb electrodes and write the redox half- 6 reactions...
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...
Consider a voltaic cell where the anode half-reaction is Zn(s) → Zn2+(aq) + 2 e− and the cathode half-reaction is Sn2+(aq) + 2 e– → Sn(s). What is the concentration of Sn2+ if Zn2+ is 2.5 × 10−3 M and the cell emf is 0.660 V? The standard reduction potentials are given below Zn+2(aq) + 2 e− → Zn(s) E∘red == −0.76 V Sn2+(aq) + 2 e– → Sn(s) E∘red −0.136 V
Consider a voltaic cell al 25 degree Celsius in which the reaction is: Zn (s) + 2H+ (aq) → Zn2+ (aq) + H2(g) It is found that the voltage (think Ecell) is +0.560 V when [Zn2+1 -0.85 M and PH2 = = 0.988 atm. What is the pH in the H2-H half-cell?
Find the emf of the cell described by the cell diagram Fe | Fe^2+ (1.500M) || Au^3+ (0.00400M) | Au. A) 1.99 V B) 1.89 V C) 1.94 V D) 1.66 V E) 1.91 V Which one of the following reactions must be carried out in an electrolytic cell rather than in a galvanic cell? A) Zn^2+ (aq) + Ca(s) rightarrow Zn(s) + Ca^2+ (aq) B) Al^3+ (aq) + 3Br^- (aq) rightarrow Al(s) + (3/2)Br_2 (1) C) 2Al(s) + 3Fe^2+...
Given the following standard reduction potentials: H^+ (aq) + 2e^- rightarrow H_2(g) E degree = 0.00 V Fe^3+ (aq) + 2e^- rightarrow Fe(s) E degree = -0.43 V (a) What is the cell potential by combining the above two half-reactions to make a working voltaic cell (same as galvanic cell)? (b) Which species will be oxidized in anode? Write the half-reaction for the anode. (c) Write the overall reaction and balance the chemical equation for this working voltaic cell. (d)...
Determine the standard cell potential (in volts) at 25 degree C for the following reaction. You will need to look up the relevant reduction potentials in your textbook. 3 Cu^2+ _(aq) + 2 Al_(s) rightarrow 2 Al^3+ _(aq) + 3 Cu_(s) TRUE or FALSE: The above reaction is non-spontaneous and would need the input of electricity to move forward as an electrolytic cell. True False