Consider a voltaic cell at 25°C consisting of a Co(s) electrode immersed in a 1.0 M Co(NO3)2 solution and an Al electrode immersed in a 1.0 M AI(NO3)3 solution, linked by a KCI bridge. Refer to the half-reactions and standard potentials below. Al3+ + 3e Al -1.67 V Co2+2e Co -0.28 V 1. Which is the reduction half reaction and potential? [Select) A A13++ 3e Al -1.67 V +1.67 V B. Al Al3+ + 3e™ C. Co²+ + 2e Co -0.28 V D. Co Co2+ + 2e* +0.28 V II. Which is the oxidation half reaction and potential? Select] A A133e Al -1.67 V B. Al Al 13e +1.67 V C. Co2¹ +2e → Co -0.28 V D. Co Co2 +2e +0.28 V III. Which is the net cell reaction and potential? | Select J A 3A13+ 2Co3AI 2Co2 -1.39 V -1.39 V B. 2A13+ 3Co2A1+ 3Co2¹ C. 2A1+ 3C02¹2A13¹+ 3Co +1.39 V D. 3Al2C023A1³+ + 2Co +1.39 V IV. What is the cell notation? [Select] A. AllA1³(aq)||Co²2¹ (aqlCo(s) B. Co² ColAl(s)A1³+ (aq) C. Cos) CofaqlA1³(aq)|Al(s) D. Al3AClCo²¹ (₂) V

Consider a voltaic cell at 25°C consisting of a Co(s) electrode immersed in a 1.0 M Co(NO3)2 solution and an Al electrode immersed in a 1.0 M AI(NO3)3 solution, linked by a KCI bridge. Refer to the half-reactions and standard potentials below. Al3+ + 3e Al -1.67 V Co2+2e Co -0.28 V 1. Which is the reduction half reaction and potential? [Select) A A13++ 3e Al -1.67 V +1.67 V B. Al Al3+ + 3e™ C. Co²+ + 2e Co -0.28 V D. Co Co2+ + 2e* +0.28 V II. Which is the oxidation half reaction and potential? Select] A A133e Al -1.67 V B. Al Al 13e +1.67 V C. Co2¹ +2e → Co -0.28 V D. Co Co2 +2e +0.28 V III. Which is the net cell reaction and potential? | Select J A 3A13+ 2Co3AI 2Co2 -1.39 V -1.39 V B. 2A13+ 3Co2A1+ 3Co2¹ C. 2A1+ 3C02¹2A13¹+ 3Co +1.39 V D. 3Al2C023A1³+ + 2Co +1.39 V IV. What is the cell notation? [Select] A. AllA1³(aq)||Co²2¹ (aqlCo(s) B. Co² ColAl(s)A1³+ (aq) C. Cos) CofaqlA1³(aq)|Al(s) D. Al3AClCo²¹ (₂) V

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

Consider the galvanic cell based on the following half-reactions: Mn2+ + 2e → Mn ɛ° -1.18 V Cd2+ + 2e –→ Cd e° : -0.40 V = a. Determine the overall cell reaction and calculate cell · (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) + + E cel b. Calculate AG° and K for the cell reaction at 25°C. AG° kJ K C. Calculate Ecell at 25°C when Ma*] Ca*+ = 1.2 Mn²+ - 0.10 М and x 10-5 М. Ecell =
Given the following electrochemical cell, calculate the potential for the cell in which the concentration of Ag+ is 0.0765 M, the pH of the H* cell is 2.700, and the pressure for H₂ is held constant at 1 atm. The temperature is held constant at 55°C. Ag Agt H+ + Ag+le ←H₂(g) Standard reduction potentials: 2H+ + 2e H₂ Fº = 0 V → Ag E°=0.800 V
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 a galvanic cell made up of Ni and Zn?
A table of standard electrode potentials is necessary for many of the following question(s). Consider the following reaction: If a galvanic cell utilizes this reaction and the initial concentrations are [Hg 2 2+] = 0.10 M, [Sn 2+] = 0.30 M, and [Sn 4+] = 0.20 M, what will be E cell under these conditions? 2+ (aq) + Sn2+ (aq) → Sn4+ (aq) + 2Hg(s) Hg2 a. 0.68 V O b. 0.66 V O c. 0.61 V O d. 0.74 V O e. 0.57 V
If a voltaic cell is created between a Sr2+/Sr electrode and a In3+/In electrode
-3 M solution of Cu(NO3)2. The other half-cell consists of a zinc electrode in One half-cell in a voltaic cell is constructed from a copper wire electrode in a 3.9 x 10 a 0.45 M solution of Zn(NO3)2 . Calculate the cell potential. You may need to use the following data: Zn²+ (aq) + 2 e¯ → Zn(s) E° = -0.763 V Cu²+ (aq) + 2 e¯ → Cu(s) E° = +0.337 V Potential = V
A voltaic cell is constructed in which the following cell reaction occurs. The half-cell compartments are connected by a salt bridge. Pb2+(aq) + Mn(s) Pb(s) + Mn2+(aq) The anode reaction is: The cathode reaction is: + + In the external circuit, electrons migrate e the Mn|Mn2+ electrode e the Pb|Pb2+ electrode. In the salt bridge, anions migrate e the Pb|Pb²+ compartment e the Mn|Mn2+ compartment. +
3. The oxidation of methanol, as described by the equation below, has a AG value of -937.9 kJ/mol. What is the standard cell potential for a methanol fuel cell? 2CH3OH +30₂ → 2CO₂ + 4H₂O
One half-cell in a voltaic cell is constructed from a copper wire electrode in a 2.7 x 10-8 M solution of Cu(NO3)2. The other half-cell consists of a zinc electrode in a 0.65 M solution of Zn(NO3)2. Calculate the cell potential. You may need to use the following data: Zn2+ (aq) + 2 e + Zn(s) E = -0.763 V Cu?+ (aq) + 2 e + Cu(s) E = +0.337 V Potential = V
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
Use the tabulated half-cell potentials to calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C. 2 Al(s) + 3 Mg²+(aq) → 2 Al3+(aq) + 3 Mg(s) 4.6E+31 9.0E-73 1.0E+24 1.1E+72 1.1E-72