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4. The following balanced redox reaction occurs in voltaic cell at 25°C H2 (g) + 2Ag+...
the following reaction occurring in an electrochemical cell at 25°C. (The equation is balanced.) fone 2 pts) a. Use the standard half-cell potentials listed below to calculate the standard cell potential (Eºcell) for 3 Sn(s) + 2 Fe* (aq) - 3 Sn2+ (aq) + 2 Fe(s) Sn 2(aq) + 2 e -Sn (s) E = -0.14 V Fe3+ (aq) + 3 e Fe(s) E° = -0.036 V A) -0.176 V B)-0.104 V C) +0.104 V D) +0.176 V b. Write...
A voltaic cell is constructed in which the following cell reaction occurs. The half-cell compartments are connected by a salt bridge. 2Ag+ (aq) + Cu(s) + 2Ag(s) + Cu2+ (aq) The anode reaction is: The cathode reaction is: + In the external circuit, electrons migrate the Ag|Ag+ electrode the Cu Cu2+ electrode. In the salt bridge, anions migrate the CuCu2+ compartment the Ag|Ag compartment.
4. Which of the following statements about the voltaic cell shown below is correct? Zn(s)[Zn** (aq)|| Cu** (aq)|Cu(s) (a) The oxidation half-reaction is clearly Zn(s) ® Zn** (aq) + 2 e. (b) The oxidation half-reaction is clearly Zn() Zn" (aq) +le. (C) The oxidation half-reaction could not be anything other than Cu(s) ® Cu (aq) +2 e. (d) It is obvious that the oxidation half-reaction is Zn(s) ® Cu(s). 5. Which of the following statements about the voltaic cell shown...
Test IV (Electrochemistry) 2018 Fall What is the oxidation number for the Which of the following is true concerning a galvanic cell? (A) Oxidation occurs at the anode and is 1. 8. underlined manganese in Mn04 (A)-8 (8)-2 (C)-1 (D)4 (E) 7 where anions move towards where anions move towards where cations move towards where anions move towards where anions move towards 2. When balancing the below half-reaction in acidic solutionelectrons are added to the (B) Oxidation occurs at the...
Question 4 (1 point) Write the cell diagram for the reaction 2AgCl(s) + H2(g) --> 2Ag(s) + 2H+(aq) + 2C1-(aq) OPt(s) | H2(g)| H+(aq) || CI+(aq)| AgCl(s) | Ag(s) Pt(s) | H2(g)| H+(aq) || CI+(aq) | Ag(s) | Pt(s) O Ag(s) | AgCl(s) || H+(aq), Ci-(aq) | H2(g) | Pt(s) O Ag(s) | AgCl(s) | CI+(aq) || H+(aq)| H2(g) | Pt(s) Pt(s) Cl(aq), H(aq)| H2(g) || AgCl(s) Ag(s)
1.) Given the following notation for an electrochemical cell Pt(s) | H2(g) | H+(aq) || Ag+(aq) | Ag(s), what is the balanced overall (net) cell reaction? A. H2(g) + 2Ag(s) ® H+(aq) + 2Ag+(aq B. H2(g) + 2Ag+(aq) ® 2H+(aq) + 2Ag(s) C. H2(g) + Ag+(aq) ® H+(aq) + Ag(s D. 2H+(aq) + 2Ag(s) ® H2(g) + 2Ag+(aq) E. 2H+(aq) + 2Ag+(aq) ® H2(g) + 2Ag(s) 2.) Calculate E°cell for the following (nonspontaneous) reaction: Cd(s) + 2Fe3+(aq) ® 2Fe2+(aq) + Cd2+(aq) → A. -0.37...
The measured voltage of a cell in which the following reaction occurs is .96V. Calculate the pH of the H+ (aq) solution The measured voltage of a cell in which the following reaction occurs is 0.96 V H20g, l 0 atm) t Ag (aq, 1.0 M) 2H'(aq, pH 2Ag(s) Calculate the pl l of the H'(aq) solution b 5.4 c. 14.9
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?
Consider the following reaction. 2Ag^+(aq) + Zn(s) --> 2Ag(s) +Zn(aq) a) write the individual oxidation and reduction half-reactions, specifying which is the anode and which is the cathode reaction. b) calculate the cell potential for a cell containing 0.10M Ag^+ and 0.25M Zn^2+ at 298K. (E ag= 0.80 V and E zn= -0.76 V)
Calculate the cell potential (Ecell) and Gibbs Free Energy (Delta G) for the reaction (2Ag+ (aq) + Fe (s) -> Fe2+ (aq) + 2Ag (s) ) under these conditions: a 250mL beaker of 1.0mol Fe metal electrode and 0.10 moles of Fe 2+; and a second 250mL beaker of 2.0 moles Ag metal electrode ad 0.50 moles of Ag+. E naught of the cell= 1.21 V.