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8) What is the standard cell potential for the following reaction? (use data in the back...
Test Yourself Section. Controlled-Potential Electrolysis What cathode potential is required to reduce 99.99% of 0.10 M...
Test Yourself Section.
Controlled-Potential Electrolysis What cathode potential is required to reduce 99.99% of 0.10 M Cu to Cu(s)? Is it pos- sible to remove this Cu without reducing 0.10 M Sn in the same solution? Cu2 +2e Cu(s) EXAMPLE 2+ (17-7) E = 0.339 V (17-8) E= -0.141 V Sn2 2et Sn(s) Solution If 99.99% of Cu were reduced, the concentration of remaining Cu 1.0 X 10 5 M, and the required cathode potential would be would be 0.059...
A voltaic cell is constructed in which the following cellreaction occurs. The half-cell compartments are...
A voltaic cell is constructed in which the following cell reaction occurs. The half-cell compartments are connected by a salt bridge.question 1 - Sn2+(aq)+ Co(s) ----------> Sn(s)+ Co2+(aq)The anode reaction (including states) is:The cathode reaction (including states) is:In the external circuit, electrons migrate _____fromto the Co|Co2+ electrode _____fromto the Sn|Sn2+ electrode.In the salt bridge, anions migrate _____fromto the Sn|Sn2+ compartment _____fromto the Co|Co2+ compartment.question 2 -A voltaic cell is constructed in which the anode is a Cd|Cd2+ half cell and the cathode is a Cu+|Cu2+ half cell. The half-cell...
QUESTION 8 Refer to the data you obtained in the simulation for the concentration cells. Select...
QUESTION 8 Refer to the data you obtained in the simulation for the concentration cells. Select the correct statements that describe the concentration cell with half cells containing 0.01 M Cu2+ and 0.10 M Cu2+ respectively The voltage is 29.6 mV The voltage is 59.2 mV The solution containing 0.1 M Cu2+ is at the cathode The solution containing 1.0 M Cu2+ is at the cathode The solution containing 0.1 M Cu2+ is at the anode The solution containing 0.01...
Question 9 What is the cell notation for a voltaic cell that incorporates the following redox...
Question 9 What is the cell notation for a voltaic cell that incorporates the following redox reaction? Cu2+ (aq) + Sn (s) Sn2+ (aq) + Cu(s) O a. Sn (s) | Sn2+ (aq) || Cu (8) | Cu2+ (aq) O b. Sn (s) | Sn2+ (aq) || Cu2+ (aq) | Cu (8) OC. Cu(s) | Cu2+ (aq) || Sn (s) | Sn2+ (aq) Od. Cu2+ (aq)|Cu () || Sn2+ (aq) | Sn (8) O e. Cu (s) | Cu2+ (aq)...
Use the half-reactions below to produce a voltaic cell with the given standard cell potential. Standard...
Use the half-reactions below to produce a voltaic cell with the given standard cell potential. Standard Cell Potential Co- (aq) + e-Cot (aq) E = +1.82 V 1.53 V 2H(aq) + 2e-H2(g) E = +0.00 V Pb2+ (aq) + 2e-Pb(s) E = -0.13 V Fe (aq) + e-Fel+ (aq) E = +0.77 V Ag (aq) + e-Ag(s) E = +0.80 V Sn* (aq) + 2e Sne (aq) 20.13 V Cu- (aq) + e- Cu(aq) E = +0.15 V Zn²+ (aq)...
The cell potential of the following electrochemical cell depends on the pH of the solution in...
The cell potential of the following electrochemical cell depends on the pH of the solution in the anode half-cell: Pt(s)|H2(g,1atm)|H+(aq,?M)||Cu2+(aq,1.0M)|Cu(s). What is the pH of the solution if Ecell is 360 mV ?
Consider the reaction corresponding to a voltaic cell and its standard cell potential. cell Zn(s) +...
Consider the reaction corresponding to a voltaic cell and its standard cell potential. cell Zn(s) + Cu2+ (aq) + Cu(s) + Zn2+ (aq) E = 1.1032 V As What is the cell potential for a cell with a 2.573 M solution of Zn²+ (aq) and 0.1055 M solution of Cu²+ (aq) at 432.4 K?
Consider the reaction corresponding to a voltaic cell and its standard cell potential. Zn(s) + Cu2+...
Consider the reaction corresponding to a voltaic cell and its standard cell potential. Zn(s) + Cu2+ (aq) Cu(s) + Zn2+ (aq) ЕО cell = 1.1032 V What is the cell potential for a cell with a 2.440 M solution of Zn2+ (aq) and 0.1636 M solution of Cu²+ (aq) at 439.5 K?
3) A voltaic cell employs the following redox reaction: Sn2+ (aq) + Mn (s) →Sn (s)...
3) A voltaic cell employs the following redox reaction: Sn2+ (aq) + Mn (s) →Sn (s) + Mn2+ (aq) a) Make a sketch of the cell. Label the cathode, anode, Sn2+, Mn, Sn, Mn?, and salt bridge. Indicate the direction of electron flow and the direction of ion flow from the salt bridge. b) Use line notation to represent the cell. c) What is the cell potential at 25°C when [Sn?] is 0.002 M and [Mn2+] is 0.050 M?
An electrochemical cell based on the following reaction has astandard cell voltage (Eocell) of 0.48 V...
An electrochemical cell based on the following reaction has astandard cell voltage (Eocell) of 0.48 V Sn (s) + Cu2+ (aq) ---> Sn2+ (aq) + Cu (s) What is the standard reduction potential of tin? Sn2+ (aq) +2e- ---> Sn(s) a. -0.14 V b. 0.14 V c. -0.82 V d. 0.82 V e. none of the above
Test Yourself Section.
Controlled-Potential Electrolysis What cathode potential is required to reduce 99.99% of 0.10 M Cu to Cu(s)? Is it pos- sible to remove this Cu without reducing 0.10 M Sn in the same solution? Cu2 +2e Cu(s) EXAMPLE 2+ (17-7) E = 0.339 V (17-8) E= -0.141 V Sn2 2et Sn(s) Solution If 99.99% of Cu were reduced, the concentration of remaining Cu 1.0 X 10 5 M, and the required cathode potential would be would be 0.059...
Question 9 What is the cell notation for a voltaic cell that incorporates the following redox reaction? Cu2+ (aq) + Sn (s) Sn2+ (aq) + Cu(s) O a. Sn (s) | Sn2+ (aq) || Cu (8) | Cu2+ (aq) O b. Sn (s) | Sn2+ (aq) || Cu2+ (aq) | Cu (8) OC. Cu(s) | Cu2+ (aq) || Sn (s) | Sn2+ (aq) Od. Cu2+ (aq)|Cu () || Sn2+ (aq) | Sn (8) O e. Cu (s) | Cu2+ (aq)...
Use the half-reactions below to produce a voltaic cell with the given standard cell potential. Standard Cell Potential Co- (aq) + e-Cot (aq) E = +1.82 V 1.53 V 2H(aq) + 2e-H2(g) E = +0.00 V Pb2+ (aq) + 2e-Pb(s) E = -0.13 V Fe (aq) + e-Fel+ (aq) E = +0.77 V Ag (aq) + e-Ag(s) E = +0.80 V Sn* (aq) + 2e Sne (aq) 20.13 V Cu- (aq) + e- Cu(aq) E = +0.15 V Zn²+ (aq)...
Consider the reaction corresponding to a voltaic cell and its standard cell potential. cell Zn(s) + Cu2+ (aq) + Cu(s) + Zn2+ (aq) E = 1.1032 V As What is the cell potential for a cell with a 2.573 M solution of Zn²+ (aq) and 0.1055 M solution of Cu²+ (aq) at 432.4 K?
Consider the reaction corresponding to a voltaic cell and its standard cell potential. Zn(s) + Cu2+ (aq) Cu(s) + Zn2+ (aq) ЕО cell = 1.1032 V What is the cell potential for a cell with a 2.440 M solution of Zn2+ (aq) and 0.1636 M solution of Cu²+ (aq) at 439.5 K?
3) A voltaic cell employs the following redox reaction: Sn2+ (aq) + Mn (s) →Sn (s) + Mn2+ (aq) a) Make a sketch of the cell. Label the cathode, anode, Sn2+, Mn, Sn, Mn?, and salt bridge. Indicate the direction of electron flow and the direction of ion flow from the salt bridge. b) Use line notation to represent the cell. c) What is the cell potential at 25°C when [Sn?] is 0.002 M and [Mn2+] is 0.050 M?
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