Using the following reactions to make a battery: Zn+2 + 2e- → Zn Eº1/2 = -0.76...
Using the following reactions to make a battery:
Zn+2 + 2e- → Zn Eº1/2 = -0.76 v
Al+3 + 3e- → Al Eº1/2 = -1.66 v
What is the balanced redox reaction? (Type in the coefficients and the charges.Type 0 for the uncharged metals.)
__Al__ + ___Zn___ → __Zn___ + ____Al____
Homework Answers
According to E01/2 values Zn2+ reduces to Zn0 and Al0 oxidizes to Al3+ as follows
Zn2+ + 2e- -----------------> Zn0
Al0 ----------------------------> Al3+
Balance the equations in order to balances the electrons;
(Zn2+ + 2e- -----------------> Zn0) * 3
(Al0 ----------------------------> Al3+) * 2
The overall balanced redox reaction:
2 Al0 + 3 Zn2+ ---------------------> 2 Al3+ + 3 Zn0
Add Answer to:
Using the following reactions to make a battery:
Zn+2 + 2e- → Zn
Eº1/2 = -0.76...
PART A: REDOX REACTIONS 1. For each of the metals, write the redox equations for reactions...
PART A: REDOX REACTIONS 1. For each of the metals, write the redox equations for reactions you observed in a table as shown below. Write NR for “no reaction” where none was observed. 2+ (**e.g., Cu + Zn → Cu + Zn , Ecell = 1.10 V) Cu(NO3)2 Pb(NO3)2 Zn(NO3)2 16 Cu(s) NR NR Pb(s) NR Zn(s) NR 2. Calculate the Eº for every cell, whether or not a reaction was observed, using equation (5) and values for the standard...
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...
6. Al(s) + A1+ (aq) + 3 e Zn + (aq) +2e → Zn() The half-reactions...
6. Al(s) + A1+ (aq) + 3 e Zn + (aq) +2e → Zn() The half-reactions for the oxidation-reduction reaction between Al(s) and Zn2+ (aq) are represented above. Based on the half-reactions, what is the coefficient for Al(s) if the equation for the oxidation-reduction reaction is balanced with the smallest whole-number coefficients? We were unable to transcribe this image
Consider the galvanic cell based on the following half-reactions: Zn2+ + 2e + Zn * =...
Consider the galvanic cell based on the following half-reactions: Zn2+ + 2e + Zn * = -0.76 V Cd²+ + 2e - → Cd &* = -0.40 V a. Determine the overall cell reaction and calculate call (Use the lowest possible coefficients. Use the pull-down boxes to specify states such as (aq) or (s). If a box is not needed, leave it blank.) V cell b. Calculate AG and K for the cell reaction at 25°C. AGE kJ K =...
Consider a galvanic cell based on the following half reactions: E° (V) Zn2+ + 2e →...
Consider a galvanic cell based on the following half reactions: E° (V) Zn2+ + 2e → Zn -0.76 Au?+ + 3e → Au 1.50 If this cell is set up at 25°C with [Zn2] = 1.00 x 10-4M and [Au?') -2.00 10-2M, the expected cell potential is Submit Hide Hints Hint 1 Hint 2 The Nernst equation is based on the balanced cell reaction. Q reflects the mass action expression for the balanced cell reaction and n is the number...
Combine the following two reactions to obtain a balanced overall redox reaction. Zn → Zn2++2e− and...
Combine the following two reactions to obtain a balanced overall redox reaction. Zn → Zn2++2e− and H++e− → H Express your answer as a chemical formula.
1.) For the complete balanced redox reaction below, what is the Eocell? Zn(s) + 2Cu+(aq) ⟶...
1.) For the complete balanced redox reaction below, what is the Eocell? Zn(s) + 2Cu+(aq) ⟶ 2Cu(s) + Zn2+(aq) Zn2+ + 2e- Zn(s) Eo = -0.76 V Cu+ + e- Cu(s) Eo = 0.52 A) -1.28 V B) +1.28 V C) 0.24 V D) -0.24 V E) +2.56 V 2.) For the redox reaction below, what is the Ecell if [Zn2+] = 0.072 M and [Cu+] = 1.27 M? T = 298 K Zn(s) + 2Cu+(aq) ⟶ 2Cu(s) + Zn2+(aq) Half Reactions:...
please I need answers to all these questions! Name 3 HW Electrochemistry Submit before Nov 20,...
please I need answers to all these questions!
Name 3 HW Electrochemistry Submit before Nov 20, 2019 at 12 PM D2L Submission: Submit one file containing all calculations and the original paper Assessments Assign ments HW Electrochemistry 1) Which two of the following half-reactions will combine to give the galvanic cell with the highest cell potential? Reduction Half-Reaction E (V) Metal Al3+ 3e- Al(s) Aluminum -1.66 Mn + 2e Mn(s) - 1.18 Manganese Zn 2e Zinc Zn(s) -0.76 Cr3 Зе-...
While performing Lab 11, Electrochemistry, students connected 1 M solutions of the following metals and used...
While performing Lab 11, Electrochemistry, students connected 1 M solutions of the following metals and used electrodes to monitor the cell potential. Using the table of theoretical values and what you know of the metals to fill in the blanks below. When writing equations: Use spaces only before and after a plus sign. For example, the reaction: Fe2+ + 2e → Fe would be entered as: Fe^2+ + 2e. Fe Galvanic Cell Consisting of: Zn²+ + 2e Zn -0.76 +...
Please show all work! 2. A battery is constructed from these two half reactions. The balanced,...
Please show all work!
2. A battery is constructed from these two half reactions. The balanced, standard reduction equation and E (as V vs. SHE) for each is shown. Ce" E-2.336 E0432 3e- Ce (s) + 2 CO (g) 2H+2e--HC.O (a) (1 pt) What is the balanced overall reaction that occurs? (b) (0.5 pt) What is n, the number of electrons transferred, for this reaction (c) (1 pt) What is E for the battery from these two reactions?
PART A: REDOX REACTIONS 1. For each of the metals, write the redox equations for reactions you observed in a table as shown below. Write NR for “no reaction” where none was observed. 2+ (**e.g., Cu + Zn → Cu + Zn , Ecell = 1.10 V) Cu(NO3)2 Pb(NO3)2 Zn(NO3)2 16 Cu(s) NR NR Pb(s) NR Zn(s) NR 2. Calculate the Eº for every cell, whether or not a reaction was observed, using equation (5) and values for the standard...
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...
6. Al(s) + A1+ (aq) + 3 e Zn + (aq) +2e → Zn() The half-reactions for the oxidation-reduction reaction between Al(s) and Zn2+ (aq) are represented above. Based on the half-reactions, what is the coefficient for Al(s) if the equation for the oxidation-reduction reaction is balanced with the smallest whole-number coefficients? We were unable to transcribe this image
Consider the galvanic cell based on the following half-reactions: Zn2+ + 2e + Zn * = -0.76 V Cd²+ + 2e - → Cd &* = -0.40 V a. Determine the overall cell reaction and calculate call (Use the lowest possible coefficients. Use the pull-down boxes to specify states such as (aq) or (s). If a box is not needed, leave it blank.) V cell b. Calculate AG and K for the cell reaction at 25°C. AGE kJ K =...
Consider a galvanic cell based on the following half reactions: E° (V) Zn2+ + 2e → Zn -0.76 Au?+ + 3e → Au 1.50 If this cell is set up at 25°C with [Zn2] = 1.00 x 10-4M and [Au?') -2.00 10-2M, the expected cell potential is Submit Hide Hints Hint 1 Hint 2 The Nernst equation is based on the balanced cell reaction. Q reflects the mass action expression for the balanced cell reaction and n is the number...
please I need answers to all these questions!
Name 3 HW Electrochemistry Submit before Nov 20, 2019 at 12 PM D2L Submission: Submit one file containing all calculations and the original paper Assessments Assign ments HW Electrochemistry 1) Which two of the following half-reactions will combine to give the galvanic cell with the highest cell potential? Reduction Half-Reaction E (V) Metal Al3+ 3e- Al(s) Aluminum -1.66 Mn + 2e Mn(s) - 1.18 Manganese Zn 2e Zinc Zn(s) -0.76 Cr3 Зе-...
While performing Lab 11, Electrochemistry, students connected 1 M solutions of the following metals and used electrodes to monitor the cell potential. Using the table of theoretical values and what you know of the metals to fill in the blanks below. When writing equations: Use spaces only before and after a plus sign. For example, the reaction: Fe2+ + 2e → Fe would be entered as: Fe^2+ + 2e. Fe Galvanic Cell Consisting of: Zn²+ + 2e Zn -0.76 +...
Please show all work!
2. A battery is constructed from these two half reactions. The balanced, standard reduction equation and E (as V vs. SHE) for each is shown. Ce" E-2.336 E0432 3e- Ce (s) + 2 CO (g) 2H+2e--HC.O (a) (1 pt) What is the balanced overall reaction that occurs? (b) (0.5 pt) What is n, the number of electrons transferred, for this reaction (c) (1 pt) What is E for the battery from these two reactions?
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