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Assignment 8 - Electrochemistry 22. A trophy manufacturer electroplates an iron trophy with gold. POWER SUPPLY...
Assignment 8 - Electrochemistry 1. Consider the reaction: 2Felip) +2170g) →2Feldg) +12(aq) Is the reaction spontaneous?...
Assignment 8 - Electrochemistry 1. Consider the reaction: 2Felip) +2170g) →2Feldg) +12(aq) Is the reaction spontaneous? Explain. (2 marks) (3 marks) 2. Balance the following half-reaction: CO2- C(OH), (basic) (3 marks) 3. Balance the following redox reaction: CIO, +Al+CI+A1 (acidic) 4. Consider the following reaction: Cr20,2- +6Br” +14H2Cr +3Bry + 7H,0 In a redox titration, 15.58 mL of 0.125 M Cr,0,2- was needed to completely oxidize the Br" in a 25.00 mL sample of NaBr. Calculate the (Br") in the...
Draw a labelled diagram of the apparatus that includes the anode, the cathode, the electrolyte, t...
Draw a labelled diagram of the apparatus that includes the anode, the cathode, the electrolyte, the direction of ion flow and the direction of electron flow provided by the power source. 28. Answer (4 Marks) Cu 29. Write and identify the half-reactions and net reaction. Answer (3 Marks) Cathode Half-Reaction Anode Half-Reaction Net Reaction 30. Calculate the theoretical potential difference of this cell. Answer (2 Mark) Chemistry so Unit C Module 6 S Besides deposition of Cu(s), what other empirical...
At the turn of the 20th century, electric automobiles were more popular than gasoline-fueled cars. Thomas...
At the turn of the 20th century, electric automobiles were more popular than gasoline-fueled cars. Thomas Edison, the prolific American inventor, was interested in electric automobiles and developed an iron-nickel (Fe-Ni) battery to power them. He claimed that, due to their higher energy density, his batteries were superior to the lead-acid batteries then being used in automobiles. Today, the Edison battery is available in various voltages up to 48 V. It is used in London subway locomotives, in New York...
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-...
ELECTROCHEMISTRY PRE-LAB ASSIGNMENT: Use the data given below to do similar calculations as you w...
Pre Lab : Electrochemistry
ELECTROCHEMISTRY PRE-LAB ASSIGNMENT: Use the data given below to do similar calculations as you will be performing in today's lab Part A: Verification of the Nernst equation The electrochemical cell to be used can be represented using conventional cell notation as: Ag(s) l Agcl(s) HCII M)|Ce(aq),Ce (a) Pts) [Ce4+]-0. | 0 M [Ce3+]-0. I 0 M Room temperature 21.6°C voltage(m V Solution mL of Ce+ solution mL of Ces solution 25.0 25.0 25.0 25.0 25.0 24.0...
i need help with all of these questions Chem 103A Electrochemistry 5. A voltaic cell is...
i need help with all of these questions
Chem 103A Electrochemistry 5. A voltaic cell is to be constructed using the Ag/Ag half cell and the Pb/Pb half-cell. Measurement shows that the silver electrode is positive. a) Write balanced half-reactions and the overall spontancous reaction, without using a table of half-cell potentials. b) Diagram the cell, labeling electrodes as anode and cathode, labeling the salt bridge, showing what ions are in solution, and showing the direction of electron flow in...
Name SHOW ALL WORK. NO CREDIT UNLESS ALL WORK IS SHOWN. ROUNDING/SIG FIG ERRORS WILL BE...
Name SHOW ALL WORK. NO CREDIT UNLESS ALL WORK IS SHOWN. ROUNDING/SIG FIG ERRORS WILL BE PENALIZED. 1. Parts a-j of this question refer to the following cell at 298 K. Complete the diagram of the following voltaic cell: Silver and iron electrodes, aqueous Silver nitrate, aqueous iron (UI) nitrate, potassium nitrate salt bridge. Fe3+ (aq) + 3e → Fe (s) Ag (aq) + e - Ag(s) E° -0.040 V Eº= 0.795 V a. Identify the electrodes as Anode or...
Name SHOW ALL WORK. NO CREDIT UNLESS ALL WORK IS SHOWN. ROUNDING/SIG FIG ERRORS WILL BE...
Name SHOW ALL WORK. NO CREDIT UNLESS ALL WORK IS SHOWN. ROUNDING/SIG FIG ERRORS WILL BE PENALIZED. 1. Parts a-j of this question refer to the following cell at 298 K. Complete the diagram of the following voltaic cell: Silver and iron electrodes, aqueous Silver nitrate, aqueous iron (UI) nitrate, potassium nitrate salt bridge. Fe3+ (aq) + 3e → Fe (s) Ag (aq) + e - Ag(s) E° -0.040 V Eº= 0.795 V a. Identify the electrodes as Anode or...
I need the answers for page 2 and three do not pay attention to the first...
I
need the answers for page 2 and three do not pay attention to the
first page!
EXPERIMENT 10: DETERMINATION OF THE ELECTROCHEMICAL SERIES QUESTIONS Which metal was not oxidized by any of the other half-cells? 1. Using Table 1, what are two metal half-cells that would oxidize the metal from question #1? 2 3. Which metal was oxidized by all of the other half-cells? 4. Using Table 1, what are two metal half-cells that the metal from question #3...
EXPERIMENT: 26 ELECTROCHEMISTRY: GALVANIC AND ELECTROLYTIC CELLS Materials Required : 50 mL beake...
Help please
EXPERIMENT: 26 ELECTROCHEMISTRY: GALVANIC AND ELECTROLYTIC CELLS Materials Required : 50 mL beakers (2) test tubes sandpaper glass U-tube cotton voltmeter 9.0 V battery connecting wires with alligator clips (2) thermometer iron nail paper clips (2) copper wire magnesium ribbon magnesium sulfate (MgSO) copper sulfate pentahydrate (CuSO, 5H,O) sodium chloride (NaCI) saturated sodium chloride (NaCI)solution phenolphthalein indicator SAFETY PRECAUTIONS: EYE PROTECTION MUST BE WORN AT ALL TIMES IN LABORATORY. Purpose of Experiment: Oxidation-reduction reactions will be performed and...
Assignment 8 - Electrochemistry 1. Consider the reaction: 2Felip) +2170g) →2Feldg) +12(aq) Is the reaction spontaneous? Explain. (2 marks) (3 marks) 2. Balance the following half-reaction: CO2- C(OH), (basic) (3 marks) 3. Balance the following redox reaction: CIO, +Al+CI+A1 (acidic) 4. Consider the following reaction: Cr20,2- +6Br” +14H2Cr +3Bry + 7H,0 In a redox titration, 15.58 mL of 0.125 M Cr,0,2- was needed to completely oxidize the Br" in a 25.00 mL sample of NaBr. Calculate the (Br") in the...
Draw a labelled diagram of the apparatus that includes the anode, the cathode, the electrolyte, the direction of ion flow and the direction of electron flow provided by the power source. 28. Answer (4 Marks) Cu 29. Write and identify the half-reactions and net reaction. Answer (3 Marks) Cathode Half-Reaction Anode Half-Reaction Net Reaction 30. Calculate the theoretical potential difference of this cell. Answer (2 Mark) Chemistry so Unit C Module 6 S Besides deposition of Cu(s), what other empirical...
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-...
Pre Lab : Electrochemistry
ELECTROCHEMISTRY PRE-LAB ASSIGNMENT: Use the data given below to do similar calculations as you will be performing in today's lab Part A: Verification of the Nernst equation The electrochemical cell to be used can be represented using conventional cell notation as: Ag(s) l Agcl(s) HCII M)|Ce(aq),Ce (a) Pts) [Ce4+]-0. | 0 M [Ce3+]-0. I 0 M Room temperature 21.6°C voltage(m V Solution mL of Ce+ solution mL of Ces solution 25.0 25.0 25.0 25.0 25.0 24.0...
i need help with all of these questions
Chem 103A Electrochemistry 5. A voltaic cell is to be constructed using the Ag/Ag half cell and the Pb/Pb half-cell. Measurement shows that the silver electrode is positive. a) Write balanced half-reactions and the overall spontancous reaction, without using a table of half-cell potentials. b) Diagram the cell, labeling electrodes as anode and cathode, labeling the salt bridge, showing what ions are in solution, and showing the direction of electron flow in...
Name SHOW ALL WORK. NO CREDIT UNLESS ALL WORK IS SHOWN. ROUNDING/SIG FIG ERRORS WILL BE PENALIZED. 1. Parts a-j of this question refer to the following cell at 298 K. Complete the diagram of the following voltaic cell: Silver and iron electrodes, aqueous Silver nitrate, aqueous iron (UI) nitrate, potassium nitrate salt bridge. Fe3+ (aq) + 3e → Fe (s) Ag (aq) + e - Ag(s) E° -0.040 V Eº= 0.795 V a. Identify the electrodes as Anode or...
Name SHOW ALL WORK. NO CREDIT UNLESS ALL WORK IS SHOWN. ROUNDING/SIG FIG ERRORS WILL BE PENALIZED. 1. Parts a-j of this question refer to the following cell at 298 K. Complete the diagram of the following voltaic cell: Silver and iron electrodes, aqueous Silver nitrate, aqueous iron (UI) nitrate, potassium nitrate salt bridge. Fe3+ (aq) + 3e → Fe (s) Ag (aq) + e - Ag(s) E° -0.040 V Eº= 0.795 V a. Identify the electrodes as Anode or...
I
need the answers for page 2 and three do not pay attention to the
first page!
EXPERIMENT 10: DETERMINATION OF THE ELECTROCHEMICAL SERIES QUESTIONS Which metal was not oxidized by any of the other half-cells? 1. Using Table 1, what are two metal half-cells that would oxidize the metal from question #1? 2 3. Which metal was oxidized by all of the other half-cells? 4. Using Table 1, what are two metal half-cells that the metal from question #3...
Help please
EXPERIMENT: 26 ELECTROCHEMISTRY: GALVANIC AND ELECTROLYTIC CELLS Materials Required : 50 mL beakers (2) test tubes sandpaper glass U-tube cotton voltmeter 9.0 V battery connecting wires with alligator clips (2) thermometer iron nail paper clips (2) copper wire magnesium ribbon magnesium sulfate (MgSO) copper sulfate pentahydrate (CuSO, 5H,O) sodium chloride (NaCI) saturated sodium chloride (NaCI)solution phenolphthalein indicator SAFETY PRECAUTIONS: EYE PROTECTION MUST BE WORN AT ALL TIMES IN LABORATORY. Purpose of Experiment: Oxidation-reduction reactions will be performed and...
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