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QUESTION 13 Consider a voltaic cell based on the half-cells: Ag (aq) + e - Ag(s)...
Consider a voltaic cell based on the half-cells: Ag+ (aq) + e - Ag(s) E* =...
Consider a voltaic cell based on the half-cells: Ag+ (aq) + e - Ag(s) E* = +0.80 V Pb2+(aq) + 2 e-Pb(s) E* = -0.13 V Identify the anode and give the cell voltage under standard conditions: = 0.67 V Ag: E cell B. Pb: E cell = 0.67 V OC. Pb: E cell = 0.93 V D. Pb: E cell = -0.67 V E. Ag: E cell = 0.93 V
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...
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...
Consider a voltaic cell where the anode half-reaction is Zn(s) → Zn2+(aq) + 2 e− and...
Consider a voltaic cell where the anode half-reaction is Zn(s) → Zn2+(aq) + 2 e− and the cathode half-reaction is Sn2+(aq) + 2 e– → Sn(s). What is the concentration of Sn2+ if Zn2+ is 2.5 × 10−3 M and the cell emf is 0.660 V? The standard reduction potentials are given below Zn+2(aq) + 2 e− → Zn(s) E∘red == −0.76 V Sn2+(aq) + 2 e– → Sn(s) E∘red −0.136 V
An electrochemical cell consists of one half-cell that contains Ag(s) and Ag+(aq), and one half-cell that...
An electrochemical cell consists of one half-cell that contains Ag(s) and Ag+(aq), and one half-cell that contains Cu(s) and Cu2+(aq). What species are produced at the electrodes under standard conditions? E° = +0.80 V Agt(aq) + e- → Ag(s) Cu2+(aq) + 2 e- → Cu(s) E° = +0.34 V O Ag(s) is formed at the cathode, and Cu(s) is formed at the anode. Ag(s) is formed at the cathode, and Cu2+ (aq) is formed at the anode. Cu(S) is formed...
question 1 - A voltaic cell is constructed from a standard Ag+|Ag half cell (E°red =...
question 1 - A voltaic cell is constructed from a standard Ag+|Ag half cell (E°red = 0.799V) and a standard Hg2+|Hg half cell (E°red = 0.855V). The anode reaction (including states) is: The cathode reaction(including states) is: The spontaneous cell reaction is: The cell voltage is .... question 2 A voltaic cell is constructed from a standard Cr3+|Cr half cell (E°red = -0.740V) and a standard Fe3+|Fe2+ half cell (E°red = 0.771V). The anode reaction (including states) is: The cathode...
A voltaic cell is based on the reduction of Ag^+(aq) to Ag(s) and the oxidation of...
A voltaic cell is based on the reduction of Ag^+(aq) to Ag(s) and the oxidation of Sn(s) to Sn^2+(aq). (a) Write half-reactions for the cell's anode and cathode. Include the phases of all species in the chemical equation. Anode Cathode (b) Write a balanced cell reaction. Include the phases of all species in the chemical equation.
A voltaic cell is constructed from an Ni2+ (aq) -Ni(s) half-cell and an Ag+ (aq)- Ag(s)...
A voltaic cell is constructed from an Ni2+ (aq) -Ni(s) half-cell and an Ag+ (aq)- Ag(s) half-cell. The initial concentration of Ni2+ (aq) in the Ni2+ - Ni half-cell is [Ni2+1 = 1.80x10-2 M. The initial cell voltage is +1.13 V. Part A By using data in Table 20.1 in the textbook, calculate the standard emf of this voltaic cell. V AEQ ? E V Submit Request Answer Part B. Will the concentration of Ni2+ (aq) increase or decrease as...
Use the standard half-cell potentials listed below to calculate the standard cell potential for the following...
Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25�C. (The equation is balanced.) Sn(s) + 2 Ag+(aq) ? Sn2+(aq) + 2 Ag(s) Sn2+(aq) + 2 e- ? Sn(s) E� = -0.14 V Ag+(aq) + e- ? Ag(s) E� = +0.80 V a)-1.08 V b)+1.74 V c)-1.74 V d)+0.94 V e)+1.08 V
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...
Consider a voltaic cell based on the half-cells: Ag+ (aq) + e - Ag(s) E* = +0.80 V Pb2+(aq) + 2 e-Pb(s) E* = -0.13 V Identify the anode and give the cell voltage under standard conditions: = 0.67 V Ag: E cell B. Pb: E cell = 0.67 V OC. Pb: E cell = 0.93 V D. Pb: E cell = -0.67 V E. Ag: E cell = 0.93 V
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...
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...
An electrochemical cell consists of one half-cell that contains Ag(s) and Ag+(aq), and one half-cell that contains Cu(s) and Cu2+(aq). What species are produced at the electrodes under standard conditions? E° = +0.80 V Agt(aq) + e- → Ag(s) Cu2+(aq) + 2 e- → Cu(s) E° = +0.34 V O Ag(s) is formed at the cathode, and Cu(s) is formed at the anode. Ag(s) is formed at the cathode, and Cu2+ (aq) is formed at the anode. Cu(S) is formed...
A voltaic cell is based on the reduction of Ag^+(aq) to Ag(s) and the oxidation of Sn(s) to Sn^2+(aq). (a) Write half-reactions for the cell's anode and cathode. Include the phases of all species in the chemical equation. Anode Cathode (b) Write a balanced cell reaction. Include the phases of all species in the chemical equation.
A voltaic cell is constructed from an Ni2+ (aq) -Ni(s) half-cell and an Ag+ (aq)- Ag(s) half-cell. The initial concentration of Ni2+ (aq) in the Ni2+ - Ni half-cell is [Ni2+1 = 1.80x10-2 M. The initial cell voltage is +1.13 V. Part A By using data in Table 20.1 in the textbook, calculate the standard emf of this voltaic cell. V AEQ ? E V Submit Request Answer Part B. Will the concentration of Ni2+ (aq) increase or decrease as...
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...
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