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10. Given a Galvanic cell Zn(s) I zs. I cu-l cus) the right-hand side of this...
In a galvanic cell, a spontaneous redox reaction occurs. However the reactants are separated such that...
In a galvanic cell, a spontaneous redox reaction occurs. However the reactants are separated such that the transfer of electrons is forced to occur across a wire. The resulting electricity is measured in volts (V) and is the sum of the potentials of the oxidation and reduction half-reactions: E^o cell = E^o red + E^o ox By reversing the reduction half-reactions, you get the corresponding oxidation half-reaction, for which E^o ox has the opposite sign of E^o red You can...
1. We will be building a Cu? and Zn galvanic cell. Write the two half reactions...
1. We will be building a Cu? and Zn galvanic cell. Write the two half reactions (one as a reduction and one as an oxidation based on forming a spontaneous reaction) and write the combined reaction. (Similar to equations 9.3-9.5 but for our system specifically). (3 pts) In the galvanic cell we are building in class, which is the anode and which is the cathode? (2 pts) 2. Calculate Ecel for our voltaic cell. (Use Table 16.1 in your OpenStax...
3. Draw a functional Galvanic cell given the following: Co Co + 2 e and Cu...
3. Draw a functional Galvanic cell given the following: Co Co + 2 e and Cu Cu +2 e. Label the anode, cathode, electrodes, solutions and all parts of the cell. Write and balance the half reactions and overall cell reaction. Calculate Eally ?Gonn and K. Show your work. Write the short hand notation for the cell.
4. Which of the following statements about the voltaic cell shown below is correct? Zn(s)[Zn** (aq)||...
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...
Consider the galvanic cell that uses the reaction 2 Ag^+ (aq) + Cu(s) rightarrow Cu^2+ (aq)...
Consider the galvanic cell that uses the reaction 2 Ag^+ (aq) + Cu(s) rightarrow Cu^2+ (aq) + 2 Ag (s) Clearly sketch the experimental set-up, write down the anode and cathode half-reactions, and give the shorthand notation for the cell.
3. Consider the following redox reaction: Zn Zn (s) +Cu2 (aq) (aq)+ Cu (s) 3.a. (10 p) Indicate the line diagram of...
3. Consider the following redox reaction: Zn Zn (s) +Cu2 (aq) (aq)+ Cu (s) 3.a. (10 p) Indicate the line diagram of the galvanic cell that uses the spontaneous redox reaction shown above. 3.b. (5 p) Write the reduction reaction corresponding to each half-cell. 3.c (5p)Calculate the equilibrium constant of the reaction K using the Nemst equation. Refer to Appendix H in the textbook to find the E values.
Show all steps please :) A galvanic cell is prepared using the following two half-cells: (i)...
Show all steps please :)
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...
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential Zn(s)...
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential Zn(s) red -0.763 V Zn2+ (aq)+2e NO3(aq)+4 H+ (aq)+3e NO(9)+2H20(1) EO red = +0.96 V Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. е х Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is...
A galvanic cell is prepared using the following half-cells: (i) MnO4-(0.283M), Mn2+(0.081M), and H+(1.0 M), and...
A galvanic cell is prepared using the following half-cells: (i) MnO4-(0.283M), Mn2+(0.081M), and H+(1.0 M), and (ii) Sn2+(0.236M) and Sn4+(0.145M). MnO4-+ 8H++ 5e-↔Mn2++ 4H2O Eo= 1.507 V Sn4++ 2e-↔Sn2+Eo= 0.151 V a)Calculate the galvanic cell voltage. b)Write the complete cell description. c)Write the cell reaction indicating clearly the direction of spontaneous reaction. d)Name the electrode (anode or cathode), give the polarity (positive or negative) of the electrode, and state the reaction (oxidation or reduction) occurring in the tin half-cell. Please...
please answer the full question. 2. You measured cell potentials (voltages) for reactions of metals and...
please answer the full question.
2. You measured cell potentials (voltages) for reactions of metals and metal ions. We will use the standard date and practice calculating these. Recall: E-Ecathode - Eanode Remember reduction occurs at the cathode; oxidation occurs at the anode For the anode reactions, your reactant will be on the product side of the standard equation, but don't change any sign. The equation does that for you. Cathode Reaction Agt + e → Ag Ecathode Anode Reaction...
In a galvanic cell, a spontaneous redox reaction occurs. However the reactants are separated such that the transfer of electrons is forced to occur across a wire. The resulting electricity is measured in volts (V) and is the sum of the potentials of the oxidation and reduction half-reactions: E^o cell = E^o red + E^o ox By reversing the reduction half-reactions, you get the corresponding oxidation half-reaction, for which E^o ox has the opposite sign of E^o red You can...
1. We will be building a Cu? and Zn galvanic cell. Write the two half reactions (one as a reduction and one as an oxidation based on forming a spontaneous reaction) and write the combined reaction. (Similar to equations 9.3-9.5 but for our system specifically). (3 pts) In the galvanic cell we are building in class, which is the anode and which is the cathode? (2 pts) 2. Calculate Ecel for our voltaic cell. (Use Table 16.1 in your OpenStax...
3. Draw a functional Galvanic cell given the following: Co Co + 2 e and Cu Cu +2 e. Label the anode, cathode, electrodes, solutions and all parts of the cell. Write and balance the half reactions and overall cell reaction. Calculate Eally ?Gonn and K. Show your work. Write the short hand notation for the cell.
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...
Consider the galvanic cell that uses the reaction 2 Ag^+ (aq) + Cu(s) rightarrow Cu^2+ (aq) + 2 Ag (s) Clearly sketch the experimental set-up, write down the anode and cathode half-reactions, and give the shorthand notation for the cell.
3. Consider the following redox reaction: Zn Zn (s) +Cu2 (aq) (aq)+ Cu (s) 3.a. (10 p) Indicate the line diagram of the galvanic cell that uses the spontaneous redox reaction shown above. 3.b. (5 p) Write the reduction reaction corresponding to each half-cell. 3.c (5p)Calculate the equilibrium constant of the reaction K using the Nemst equation. Refer to Appendix H in the textbook to find the E values.
Show all steps please :)
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...
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential Zn(s) red -0.763 V Zn2+ (aq)+2e NO3(aq)+4 H+ (aq)+3e NO(9)+2H20(1) EO red = +0.96 V Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. е х Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is...
please answer the full question.
2. You measured cell potentials (voltages) for reactions of metals and metal ions. We will use the standard date and practice calculating these. Recall: E-Ecathode - Eanode Remember reduction occurs at the cathode; oxidation occurs at the anode For the anode reactions, your reactant will be on the product side of the standard equation, but don't change any sign. The equation does that for you. Cathode Reaction Agt + e → Ag Ecathode Anode Reaction...
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