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9.) (8 pts.) Use the following /2 cell information to answer the question below: Cu(s) |...
uestion 27 of 30 Map The concentrations of NaCl and KI are at 0.170 M and...
uestion 27 of 30 Map The concentrations of NaCl and KI are at 0.170 M and 0.120 M,respectively, in the following electrochemical cell: Cu(s)I Cul(s) I r(aq) II Cr(aq) | AgC(s) IAg(s A) Using the following half-reactions, calculate cell voltage: Cults) + e. Culs) +1- E"--0.185 V Number B) Now, calculate the cell voltage using the following half-reactions. Cul are 1.810-10 and 1.0102, respectively. solubility products (Ksp) for AgCI and Ag++ e- Ag(s) E"-0.7993 V Number O Previous ) Give...
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...
3. A student connects a Cd?"(0.20 M)|Cd(s) half-cell to a Cu?"(1 M) Cu(s) electrode. When the...
3. A student connects a Cd?"(0.20 M)|Cd(s) half-cell to a Cu?"(1 M) Cu(s) electrode. When the red lead is attached to the Cu electrode, the cell potential read by the voltmeter, E is +0.77 V. a. What is the reduction half-reaction at the cathode (red lead)? b. What is the oxidation half-reaction at the anode (black lead)? c. What is the overall cell reaction? d. Write the expression for the thermodynamic reaction quotient, Q, and calculate its value for this...
The cell potential of a redox reaction occurring in an electrochemical cell under any set of...
The cell potential of a redox reaction occurring in an
electrochemical cell under any set of temperature and concentration
conditions can be determined from the standard cell potential of
the cell using the Nernst equation where E is the cell
potential of the cell, E° is the standard cell potential
of the cell, R is the gas constant, T is the
temperature in kelvin, n is the moles of electrons
transferred in the reaction, and Q is the reaction
quotient....
cell A voltaic cell employs the following redox reaction: Cu(s) + 2 Ag+ (aq) – Cu...
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 +] = 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 the cell potential,...
1) Calculate the cell potential, E°cell, for the following electrochemical reaction. Cu(s) + I2(g) → Cu+2(aq)...
1) Calculate the cell potential, E°cell, for the following electrochemical reaction. Cu(s) + I2(g) → Cu+2(aq) + 2I-1(aq) E = ? a.-0.87 V b.-0.19 V c.0.19 V d.0.87 V 2) Calculate the equilibrium constant (Keq) for the following reaction at 25 °C? (Faraday's Constant = 96,500 J / V · mol) & (R = 8.314 J / mol · K) 2Fe+3(aq) + Sn+2(aq) → 2Fe+2(aq) + Sn+4(aq) K = ? a. 4.04 x 107 b. 3.44 x 1018 c. 4.48...
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...
Consider the reaction corresponding to a voltaic cell and its standard cell potential. Zn(s) + Cu?+...
Consider the reaction corresponding to a voltaic cell and its standard cell potential. Zn(s) + Cu?+ (aq) Cu(s) + Zn²+ (aq) E cell 1.1032 V What is the cell potential for a cell with a 2.344 M solution of Zn?' (aq) and 0.1701 M solution of Cu?+ (aq) at 441.2 K?
Galvanic Cell reaction I am a little confused on what the following questions are asking. For...
Galvanic Cell reaction I am a little confused on what the following questions are asking. For some background: A galvanic cell using 0.200M KBr and 0.100 AgNO3 creates Ag(s) I AgBr(s) I Br - (aq, 0.0500M) II Ag+ (aq, 0.100M) I Ag(s) average cell voltage: 0.530 V what is the overall cell reaction? Show how you calculated the standard cell potential (using the average cell voltage) Show how you calculated the solubility product of AgBr(s) using your experimentally determined standard...
uestion 27 of 30 Map The concentrations of NaCl and KI are at 0.170 M and 0.120 M,respectively, in the following electrochemical cell: Cu(s)I Cul(s) I r(aq) II Cr(aq) | AgC(s) IAg(s A) Using the following half-reactions, calculate cell voltage: Cults) + e. Culs) +1- E"--0.185 V Number B) Now, calculate the cell voltage using the following half-reactions. Cul are 1.810-10 and 1.0102, respectively. solubility products (Ksp) for AgCI and Ag++ e- Ag(s) E"-0.7993 V Number O Previous ) Give...
3. A student connects a Cd?"(0.20 M)|Cd(s) half-cell to a Cu?"(1 M) Cu(s) electrode. When the red lead is attached to the Cu electrode, the cell potential read by the voltmeter, E is +0.77 V. a. What is the reduction half-reaction at the cathode (red lead)? b. What is the oxidation half-reaction at the anode (black lead)? c. What is the overall cell reaction? d. Write the expression for the thermodynamic reaction quotient, Q, and calculate its value for this...
The cell potential of a redox reaction occurring in an
electrochemical cell under any set of temperature and concentration
conditions can be determined from the standard cell potential of
the cell using the Nernst equation where E is the cell
potential of the cell, E° is the standard cell potential
of the cell, R is the gas constant, T is the
temperature in kelvin, n is the moles of electrons
transferred in the reaction, and Q is the reaction
quotient....
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 +] = 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 the cell potential,...
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...
Consider the reaction corresponding to a voltaic cell and its standard cell potential. Zn(s) + Cu?+ (aq) Cu(s) + Zn²+ (aq) E cell 1.1032 V What is the cell potential for a cell with a 2.344 M solution of Zn?' (aq) and 0.1701 M solution of Cu?+ (aq) at 441.2 K?
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