please help wirh D E and F
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please help wirh D E and F
AG for the reaction = 13. (50) For the...
number 13 a-i please AG for the reaction - 13. (50) For the reaction in base,...
number 13 a-i please
AG for the reaction - 13. (50) For the reaction in base, H.O.(aq) + CIO.(aq) → CIO, (aq) + O2(g) to gas tank a. Label all parts of the voltaic cell (Parts: direction of electron flow, direction of anion/cation flow, anode, cathode components of solutions, electrodes, salt bridge, meter) Be sure to pay attention to the gaseous component and adjust your labeling accordingly. On the lines under each half-cell, write the balanced half-cell reaction which will...
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...
20iii please and thanks Long Answer 20. A galvanic (voltaic) cell consists of Ag/Ag* and Sn/Sn2...
20iii please and thanks
Long Answer 20. A galvanic (voltaic) cell consists of Ag/Ag* and Sn/Sn2 half cells at standard conditions with a salt bridge containing KCI. Sn2+ (aq) + 2 e-→ Sn (s) Eo =-0.137 V Ag (aq) e > Ag (s)+0.800 V i. ii. Write a balanced equation for the spontaneous redox reaction and determine Ee Sketch this galvanic cell. Label the anode, the cathode, the direction of flow of electrons in the external circuit and the direction...
PLEASE ANSWER ALL 4. The cell potential for the unbalanced chemical reaction: Hg2 2+(aq) + NO3...
PLEASE ANSWER ALL 4. The cell potential for the unbalanced chemical reaction: Hg2 2+(aq) + NO3 - (aq) + H+ (aq) → Hg2+(aq) + HNO2(aq) is measured under standard conditions and found to be + 0.02 V at 25C. a) What substance (not just the element) is oxidized in the cell? b) What substance (not just the element) is reduced in the cell? c) Write the half-reaction that occurs in the anode compartment. d) Write the half-reaction that occurs in...
all parts please cell A voltaic cell employs the following redox reaction: Cu(s) + 2 Ag+...
all parts please
cell A voltaic cell employs the following redox reaction: Cu(s) + 2 Ag+ (aq) Cu 2+ (aq) + 2 Ag(s) The E° 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...
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...
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...
Chem 1212 Lab Report on electrochemistry Electrochemistry When electrons transfer between reaction components in a redox...
Chem 1212 Lab Report on electrochemistry
Electrochemistry When electrons transfer between reaction components in a redox reaction, we can harness the motion of the electrons to create a potential. Electrochemistry revolves around the separation of the two half-reactions in a redox reaction and establishing two different electrodes. This might involve physically separating the half-reactions or including a separator, such as a semi-permeable membrane or plastic dividers. With the reactions separated, the electrons will need to flow through the wire connecting...
Consider the following electrochemical cell. Ag(s) | Ag+(aq) || Cr3+(aq) | Cr(s) Determine the overall reaction...
Consider the following electrochemical cell. Ag(s) | Ag+(aq) || Cr3+(aq) | Cr(s) Determine the overall reaction and its standard cell potential (in V) at 25°C for this reaction. (Include states-of-matter under the given conditions in your answer. Use the lowest possible whole number coefficients.) Overall reaction (please provide)= standard cell potential V= Is the reaction spontaneous at standard conditions?
number 13 a-i please
AG for the reaction - 13. (50) For the reaction in base, H.O.(aq) + CIO.(aq) → CIO, (aq) + O2(g) to gas tank a. Label all parts of the voltaic cell (Parts: direction of electron flow, direction of anion/cation flow, anode, cathode components of solutions, electrodes, salt bridge, meter) Be sure to pay attention to the gaseous component and adjust your labeling accordingly. On the lines under each half-cell, write the balanced half-cell reaction which will...
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...
20iii please and thanks
Long Answer 20. A galvanic (voltaic) cell consists of Ag/Ag* and Sn/Sn2 half cells at standard conditions with a salt bridge containing KCI. Sn2+ (aq) + 2 e-→ Sn (s) Eo =-0.137 V Ag (aq) e > Ag (s)+0.800 V i. ii. Write a balanced equation for the spontaneous redox reaction and determine Ee Sketch this galvanic cell. Label the anode, the cathode, the direction of flow of electrons in the external circuit and the direction...
all parts please
cell A voltaic cell employs the following redox reaction: Cu(s) + 2 Ag+ (aq) Cu 2+ (aq) + 2 Ag(s) The E° 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...
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...
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...
Chem 1212 Lab Report on electrochemistry
Electrochemistry When electrons transfer between reaction components in a redox reaction, we can harness the motion of the electrons to create a potential. Electrochemistry revolves around the separation of the two half-reactions in a redox reaction and establishing two different electrodes. This might involve physically separating the half-reactions or including a separator, such as a semi-permeable membrane or plastic dividers. With the reactions separated, the electrons will need to flow through the wire connecting...
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