For the saturated solution of CuC₂O4 in the anode half-cell, and 1.0M Cu in the cathode half-cell, the measured cell potential is 0.139V Table 3. Cell Potentials of Concentration Copper Cell Anode: Copper (Cu) Anode electrolyte concentration, M 1.0 0.10 0.010 0.0010 0.00010 0.000010 0.0000010 Cathode electrolyte concentration, M 1.0 1.0 1.0 1.0 1.0 1.0 1.0 Cathode -Log[Anode] 0 1 2 3 4 5 6 Copper (Cu) Measured Potential, V 0.155 0.185

For the saturated solution of CuC₂O4 in the anode half-cell, and 1.0M Cu in the cathode half-cell, the measured cell potential is 0.139V Table 3. Cell Potentials of Concentration Copper Cell Anode: Copper (Cu) Anode electrolyte concentration, M 1.0 0.10 0.010 0.0010 0.00010 0.000010 0.0000010 Cathode electrolyte concentration, M 1.0 1.0 1.0 1.0 1.0 1.0 1.0 Cathode -Log[Anode] 0 1 2 3 4 5 6 Copper (Cu) Measured Potential, V 0.155 0.185

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 voltaic cell is constructed, based on the Zn/Sn2+ ion reaction. Zn + Sn2+ → Zn2+ + Sn The standard cell potential is 0.626 V. What is the cell potential be when [Zn2+]=1.2 M and [Sn2+]=0.8 M ?
A voltaic cell is constructed with a Ni//Ni2+ half-cell and a Ag/Ag+ half-cell. The nickel electrode is negatively charged. Draw a diagram of the cell, labeling the electrodes with their charges and showing the direction of electron flow in the circuit and of cation and anion flow in the salt bridge.Identify the anode and cathode half-reactions and show the shorthand notation. Calculate the standard potential in volts for the reaction at room temperature
What is the standard cell potential for the reaction below? Enter your answer with two decimal places and no units. Mg(s) + Br2() Mg2+(aq) + 2 Br"aq) The standard reduction potential is -2.37 V for the Mg2+/Mg half-cell and +1.09 V for the Bro/Br half-cell. Enter your answer in decimal format using two decimal places, (value + 2%).
A voltaic cell employs the following redox reaction: 2 Fe3+ Calculate the cell potential at 25 °C under each of the following conditions. (ag) + 3 Mg (s) → 2 Fe (s) + 3 Mg²+ (aq) Part C [Fe+] = 3.10 M ; [Mg²+] = 1.2x10-3 M Ecell Submit Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining
A galvanic (voltaic) cell consists of an electrode composed of nickel in a 1.0 M nickel(II) 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. E° V 'cell * TOOLS х10
If a voltaic cell is created between a Sr2+/Sr electrode and a In3+/In electrode
Write a balanced equation for the half-reaction that happens at the cathode of this cell. Write a balanced equation for the half-reaction that happens at the anode of this cell. Of what substance is E1 made? Of what substance is E2 made? What are the chemical species in solution S1? What are the chemical species in solution S2? 0 0 0 0 0 0
A galvanic (voltaic) cell consists of an electrode composed of cadmium in a 1.0 M cadmium ion solution and a second electrode composed of lead in a 1.0 M lead(II) ion solution, connected by a salt bridge. Calculate the standard potential for this cell at 25 °C. Use this list of standard reduction potentials. E: cell 11 x10 TOOLS V
A voltaic cell is constructed with two silver–silver chloride electrodes, each of which is based on the following half-reaction: AgCl1s2 + e- ¡ Ag1s2 + Cl -1aq2 The two half-cells have 3Cl -4 = 0.0150 M and 3Cl -4= 2.55 M, respectively. What is the standard emf of the cell?
Study each overall cell reaction. Identify and write the half-reaction that occurs in the anode and in the cathode. Calculate the standard cell potential and describe the reaction as spontaneous or non-spontaneous. Cl2(g) + 2Br-(aq) → 2Cl-(aq) + Br2(l)
Calculate Ecell (volts) for the galvanic cell containing the reaction shown below where the concentration of the ion at the anode is 0.400 M and the concentration of the ion at the cathode is 1.86 M.
Calculate Ecell (volts) for the galvanic cell containing the reaction shown below where the concentration of the ion at the anode is 0.700 M and the concentration of the ion at the cathode is 2.01 M.