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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...
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...
Parts a-j of this question refer to the following cell at 298 K. Complete the diagram...
Parts a-j of this question refer to the following cell at 298 K. Complete the diagram of the following voltaic cell: Zinc and iron electrodes, aqueous zinc nitrate, aqueous iron (III) nitrate, potassium nitrate salt bridge. Fe3+ (aq) + 3e- → Fe (s) E°= -0.040 V Ag+(aq) + e- → Ag(s) E°= 0.795 V a. Identify the electrodes as Anode or Cathode. Write the correct metal for each assuming the reactions are spontaneous b. Show the direction of the electron...
2) On the standard galvanic cell schematic shown below, add labels for: (2 pts) A) Anode...
2) On the standard galvanic cell schematic shown below, add labels for: (2 pts) A) Anode B) Cathode C) Salt Bridge D) Show the direction of electron flow through the wire Equations and Constants: AG --FE E-Eº - (RT/nF)InQ R-8.3145 J/mol K F-96485 J/V mole (7 pts) 3) For the galvanic cell represented by Zn(s)Zn²+ (aq)|| Ag (aq)| Ag(s) Voltmeter A) Write the anode half reaction Zn(s) JAg(s) B) Write the cathode half reaction C) Write the net reduction-oxidation reaction...
A voltaic cell is set up with a beaker on the left containing 1.0 M AgNO...
A voltaic cell is set up with a beaker on the left containing 1.0 M AgNO 3 and a silver electrode, and a beaker on the right containing 1.0 M Cr(NO 3) 3 and a chromium electrode. Given the following standard reduction potentials, answer the 3 questions below: Eº Ag+(aq) + 1e → Ag(s) +0.80 V Cr3+(aq) + 3e → Cr(s) -0.73V Part a. Write out the half-cell reaction that occurs at the anode of the voltaic cell. Part...
please comment if need more info. no need to show work just correct answers. Consider the...
please comment if need more info. no need to show work just
correct answers.
Consider the following reaction at 298K. 2 Fe3+ (aq) + 2 1 (aq) — 2 Fe2+ (aq) +12 (5) Which of the following statements are correct? Choose all that apply Eºcell <0 The reaction is reactant-favored. On= 6 mol electrons delta Gº<0 DK > 1 Consider the following reaction at 298K. I, (s) + Zn (s) — — 21+ (aq) + Zn2+ (aq) Which of the...
please do both please please please QUESTION 15 When an aqueous solution of KBr is electrolyzed,...
please do both please please please
QUESTION 15 When an aqueous solution of KBr is electrolyzed, what forms at the electrodes? A. Cathode: Br2 anode: H2 B. Cathode: Br2: anode: K C. Cathode: H2; anode: O2 D. Cathode: H2; anode: Br2 E. Cathode: K: anode: Br2 QUESTION 13 Consider a voltaic cell based on the half-cells: Ag+(aq) + e - Ag(s) E° - +0.80 V *(aq) + 2 e - Co(s) Eº = -0.28 V Identify the anode and give...
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...
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...
A voltaic cell employs the following redox reaction: Cu(s) + 2 Ag + (aq) → Cu...
A voltaic cell employs the following redox reaction: Cu(s) + 2 Ag + (aq) → Cu 2+ (aq) + 2 Ag(s) The Eº cell for the reaction is +0.46 V. The initial (nonstandard) conditions are: [Ag +] = 0.025M ; [Cu 2+] = 2.0 M Part a. Write the half-reaction that occurs at the anode. Part b. Write the half-reaction that occurs at the cathode. Part c. How many electrons are transferred in this reaction? Part d. What is...
A voltaic cell employs the following redox reaction: Cu(s) + 2 Ag + (aq) → Cu...
A voltaic cell employs the following redox reaction: Cu(s) + 2 Ag + (aq) → Cu 2+ (aq) + 2 Ag(s) The Eº cell for the reaction is +0.46 V. The initial (nonstandard) conditions are: [Ag +] = 2.0 M ; [Cu 2+] = 0.025 M Part a. Write the half-reaction that occurs at the anode. Part b. Write the half-reaction that occurs at the cathode. Part c. How many electrons are transferred in this reaction? Part d. What is...
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...
2) On the standard galvanic cell schematic shown below, add labels for: (2 pts) A) Anode B) Cathode C) Salt Bridge D) Show the direction of electron flow through the wire Equations and Constants: AG --FE E-Eº - (RT/nF)InQ R-8.3145 J/mol K F-96485 J/V mole (7 pts) 3) For the galvanic cell represented by Zn(s)Zn²+ (aq)|| Ag (aq)| Ag(s) Voltmeter A) Write the anode half reaction Zn(s) JAg(s) B) Write the cathode half reaction C) Write the net reduction-oxidation reaction...
please comment if need more info. no need to show work just
correct answers.
Consider the following reaction at 298K. 2 Fe3+ (aq) + 2 1 (aq) — 2 Fe2+ (aq) +12 (5) Which of the following statements are correct? Choose all that apply Eºcell <0 The reaction is reactant-favored. On= 6 mol electrons delta Gº<0 DK > 1 Consider the following reaction at 298K. I, (s) + Zn (s) — — 21+ (aq) + Zn2+ (aq) Which of the...
please do both please please please
QUESTION 15 When an aqueous solution of KBr is electrolyzed, what forms at the electrodes? A. Cathode: Br2 anode: H2 B. Cathode: Br2: anode: K C. Cathode: H2; anode: O2 D. Cathode: H2; anode: Br2 E. Cathode: K: anode: Br2 QUESTION 13 Consider a voltaic cell based on the half-cells: Ag+(aq) + e - Ag(s) E° - +0.80 V *(aq) + 2 e - Co(s) Eº = -0.28 V Identify the anode and give...
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...
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...
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