A galvanic cell is set-up in the laboratory with a copper anode and an unidentified cathode. Your teacher asks you to identify the cathode of the solution with the given information. The anode metal is lustrous and grey in color, so you narrow it down to silver and zinc. The voltmeter reading shows that the cell potential is 0.50 V. The copper (II) sulfate solution was indicated to have a concentration of 0.10 M. Reduction Half-Reaction Standard Reduction Potential (V) Ag+(ag) +e-→ Ag(s) +0.80 Cu2+(aq) +2e-→→ Cu(s) +0.34 Zn2+(ag) +2e-→→→ Zn(s) -0.76 1. Identify the reduction half-reaction involved. ○a. Ag+ (aq) +e²- Ag(s) O b. Cu²+ (aq) +2e* → Cu(s) OC. Zn²+ (aq) +2e → Zn(s)

A galvanic cell is set-up in the laboratory with a copper anode and an unidentified cathode. Your teacher asks you to identify the cathode of the solution with the given information. The anode metal is lustrous and grey in color, so you narrow it down to silver and zinc. The voltmeter reading shows that the cell potential is 0.50 V. The copper (II) sulfate solution was indicated to have a concentration of 0.10 M. Reduction Half-Reaction Standard Reduction Potential (V) Ag+(ag) +e-→ Ag(s) +0.80 Cu2+(aq) +2e-→→ Cu(s) +0.34 Zn2+(ag) +2e-→→→ Zn(s) -0.76 1. Identify the reduction half-reaction involved. ○a. Ag+ (aq) +e²- Ag(s) O b. Cu²+ (aq) +2e* → Cu(s) OC. Zn²+ (aq) +2e → Zn(s)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

A certain half-reaction has a standard reduction potential -0 red = = +0.90 V. An engineer proposes using this half-reaction at the cathode of a galvanic cell that must provide at least 0.70 V of electrical power. The cell will operate under standard conditions. Note for advanced students: assume the engineer requires this half-reaction to happen at the cathode of the cell. ロ→ロ 0 Is there a minimum standard reduction potential that the half-reaction used at the anode of this cell can have? yes, there is a minimum. ☐v red If so, check the "yes" box and calculate the minimum. Round your answer to 2 decimal places. If there is no lower limit, check the "no" box. no minimum Ś ? 0 Is there a maximum standard reduction potential that the half-reaction used at the anode of this cell can have? yes, there is a maximum. Ov red If so, check the "yes" box and calculate the maximum. Round your answer to 2 decimal places. If there is no upper limit, check the "no" box. no maximum E E = = X
. At 25 C, the standard hydrogen electrode (SHE) has a half-cell potential that is defined to be 0.00 volts. If the pH is increased at this electrode (keeping everything else the same), at what pH will the half-cell potential be equal to -0.521 volts?
A solution containing vanadium (chemical symbol V) in an unknown oxidation state was electrolyzed with a current of 1.46 A for 23.1 min. It was found that 0.534 g of V was deposited on the cathode. What was the original oxidation state of the vanadium ion? The original oxidation state of the vanadium ion =
The following spontaneous reaction occurs when metallic zinc is dipped into a solution of copper sulfate. Zn (s) +Cu^ 2+ (aq) ----> Zn^ 2+ (aq) +Cu (s) Describe a galvanic cell that could take advantage of this reaction. What are the half-cell reactions? Make a sketch of the cell and label the cathode and anode, the charges on each electrode , the direction of ion flow, and the direction of electron flow .
A galvanic (voltaic) cell consists of an electrode composed of aluminum in a 1.0 M aluminum ion solution and another electrode composed of gold in a 1.0 M gold(III) ion solution, connected by a salt bridge. Calculate the standard potential for this cell at 25 °C. Refer to the list of standard reduction potentials. Excell V
A certain metal M forms a soluble nitrate salt MNO33 . Suppose the left half cell of a galvanic cell apparatus is filled with a 5.00M solution of MNO33 and the right half cell with a 25.0mM solution of the same substance. Electrodes made of M are dipped into both solutions and a voltmeter is connected between them. The temperature of the apparatus is held constant at 35.0°C. What voltage will the voltmeter show? Assume its positive lead is connected to the positive electrode.Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits.
A concentration cell is constructed using two Ni electrodes with Ni2+ concentrations of 1.0 M and 1.00 x 10–4 M in the two half-cells. The reduction potential of Ni2+ is –0.23 V. Calculate the potential of the cell at 25°C.
The silver zinc battery is used in hearing aids. Explain the fundamental redox reactions that occur in this battery and calculate the theoretical cell potential for this system.
3.5. Diagrams A and B show two different sample injection systems for electrophoresis separation. Describe their mode of operation. Assuming that our sample in both diagrams comprises the composition of anions, cations, and neutral molecules, identify them in order of their movement in the capillary. Sample ►Vacuum Buffer Buffer Figure 4: Injection systems. B A (312)
red A certain half-reaction has a standard reduction potential E = +0.16 V. An engineer proposes using this half-reaction at the cathode of a galvanic cell that must provide at least 1.30 V of electrical power. The cell will operate under standard conditions. Note for advanced students: assume the engineer requires this half-reaction to happen at the cathode of the cell. Is there a minimum standard reduction potential that the half-reaction used at the anode of this cell can have? If so, check the "yes" box and calculate the minimum. Round your answer to 2 decimal places. If there is no lower limit, check the "no" box. Is there a maximum standard reduction potential that the half-reaction used at the anode of this cell can have? If so, check the "yes" box and calculate the maximum. Round your answer to 2 decimal places. If there is no upper limit, check the "no" box. By using the information in the ALEKS Data tab, write a balanced equation describing a half reaction that could be used…
A galvanic cell was constructed with a nickel electrode that was dipped into 1.1 M NiSO4 solution and a chromium electrode that was immersed into a solution containing Cr3+ at an unknown concentration. The potential of the cell was measured to be 0.557 V, with the chromium serving as the anode. The standard cell potential for this system was determined to be 0.487 V. What was the concentration of Cr3+ in the solution of unknown concentration?
A solution containing vanadium (chemical symbol V) in an unknown oxidation state was electrolyzed with a current of 1.08 A for 27.8 min. It was found that 0.317 g of V was deposited on the cathode. What was the original oxidation state of the vanadium ion? The original oxidation state of the vanadium ion = i