Describe an electrochemical cell that would have the following net equation, by answering the following questions,...

Question

Question

Add a comment Improve this question Transcribed image text

Answer 1

Answer #1

041 (S) (av) (C) Redution) 16 Oudatien oxi dation hall celu Redution half cell! otz Ni av (s) (Av) (S) Figureinct there in we

Add a comment

Answer 2

Similar Homework Help Questions

Describe an electrochemical cell that would have the following net equation, by answering the following questions,...

Describe an electrochemical cell that would have the following net equation, by answering the following questions, Fe(s) + Ni2+ (aq) → Ni(s) + Fe2(aq) a) Write the reduction and oxidation half-equations for the cell. b) Sketch the electrochemical cell. Identify the components of the cell as in Figure 1.. c) Calculate the expected net voltage for this cell.
Table provided below for context Please answer all parts that you can. 1. Which electrochemical cell...

Table provided below for context Please answer all parts that you can. 1. Which electrochemical cell had the greatest voltage? Identify the anode and the cathode for this pair, the measured cell potential, and the calculated Eºcell- 2. Which electrochemical cell had the smallest voltage? Identify the anode and the cathode for this pair, the measured cell potential, and the calculated Eºcell- 3. If the oxidation and reduction half-reactions are separated in a battery, this means the oxidizing agent is...
the following reaction occurring in an electrochemical cell at 25°C. (The equation is balanced.) fone 2...

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...

Calculate e cell for the electrochemical cell below, Pb(s) |Pb2+(aq, 1.0 M) || Fe2+(aq, 1.0 M)...

Calculate e cell for the electrochemical cell below, Pb(s) |Pb2+(aq, 1.0 M) || Fe2+(aq, 1.0 M) | Fe(s) given the following reduction half-reactions. Pb2+(aq) + 2 e– ® Pb(s) E° = –0.126 V Fe2+(aq) + e– ® Fe(s) E° = –0.44 V
I need help with questione 1-12 and discussion question 1 and 2. The previous pictures help...

I need help with questione 1-12 and discussion question 1 and 2. The previous pictures help determine the chart. Please Show Work thank you so much An oxidation half-reaction is characterized by electrons appearing on the product side. The oxidation of aluminum for instance would be represented thusly: Al(s) → Al3+ + 3e- (1) An reduction half-reaction is characterized by electrons appearing on the reactant side. The reduction of ferrous iron for instance would be represented thusly: Fe2+ + 2e...
O ADVANCED MATERIAL Analyzing a galvanic cell A galvanic cell is powered by the following redox...

O ADVANCED MATERIAL Analyzing a galvanic cell A galvanic cell is powered by the following redox reaction: 3 Fe+(aq) + Cr(OH),(s) + 5OH(aq) – 3 Fe2(aq) + Cro (aq) + 4H20( Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab. Write a balanced equation for the half-reaction that takes place at the cathode. Write a balanced equation for the half reaction that takes place at the...

(a) Iron is above copper on the activity series. Based on that fact, write the net...

(a) Iron is above copper on the activity series. Based on that fact, write the net ionic reaction expected for a spontaneous reaction involving Fe(s), Cu(s), Fe2+(aq) and Cu2+(aq). (b) If an electrochemical cell were made with the components described above, what would be the metal the cathodic half-cell? (c) If an electrochemical cell were made with the components described above, what would be the metal ion in the cathodic half-cell?
Balance the following oxidation-reduction reactions using the half-reaction method. 1. HCOOH (aq) + MnO.. (aq) → CO2 (g) + Mn2. Acidie solution Identify the reduction half Identify the oxidation...

Balance the following oxidation-reduction reactions using the half-reaction method. 1. HCOOH (aq) + MnO.. (aq) → CO2 (g) + Mn2. Acidie solution Identify the reduction half Identify the oxidation half Basic solution Identify the reduction half Identify the oxidation half Write a balanced equation for the electrode and overall cell reactions in the following galvanic cell and determine E°. Sketch the cell, labeling the anode and cathode and showing the direction of electron and ion flow. 2. 3. Circle the...
For the following half reactions and the partially complete image for an electrochemical cell: Indicate the...

For the following half reactions and the partially complete image for an electrochemical cell: Indicate the direction of electron flow and then complete the cell diagram. bar Cl₂'g) . 4 . e Ci(m) Pt(s) Cl2(g) CI-(aq) Ni2+(aq) Ni(s) Ered/v 1.358 C12(g) + 2e → 201(aq) Ni2+ lag) + 2 → Ni(s) -0.257 electrochemical cell: am. -Ibar Claig) . > > SI cí (im) Eredly 1.358 ) -0.257

A galvanic cell is powered by the following redox reaction: 3 Fe'*(aq) + MnO(s) + 4...

A galvanic cell is powered by the following redox reaction: 3 Fe'*(aq) + MnO(s) + 4 OH(aq) → 3 Fe2+ (aq) + Mno (aq) + 2 H,00 Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab. Write a balanced equation for the half-reaction that takes place at the cathode. Write a balanced equation for the half-reaction that takes place at the anode. x 5 ? Calculate...

Describe an electrochemical cell that would have the following net equation, by answering the following questions,...

Homework Answers