A voltaic cell has the following initial state: Cr (s) | Cr (aq, 2.0 M)|| C* (aq, 9.0 M) | Cr (s) Each half-cell has a volume of 1.00 L. Calculate the number of hours the cell can run at 26 A before reaching equilibrium. Enter your answer to 1 decimal place. Reduction E° (V) half-reaction

A voltaic cell has the following initial state: Cr (s) | Cr (aq, 2.0 M)|| C* (aq, 9.0 M) | Cr (s) Each half-cell has a volume of 1.00 L. Calculate the number of hours the cell can run at 26 A before reaching equilibrium. Enter your answer to 1 decimal place. Reduction E° (V) half-reaction

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...

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A voltaic cell has the following initial state: Cr (s) | Cr3 (aq, 2.0 M) || Cr* (aq, 9.0 M) | Cr (s) Each half-cell has a volume of 1.00 L. Calculate the number of hours the cell can run at 26 A before reaching equilibrium. Enter your answer to 1 decimal place. Reduction half-reaction E (V) Au (aq)+e + Au(s) 1.69 + Ag(s) + Cu(s) Ag (aq) + e 0.80 Cu (aq) +e 0.52 Cu (aq) + 2e + Cu(s) 0.32 Ph2+ (aq)+2e + Pb(s) -0.13 + Sn(s) -0.14 (aq)+ 2e Ni2+ (aq) + 2e Co+(aq) + 2e Sn2+ + Ni(s) -0.23 + Co(s) -0.28 In+ (aq) + 3e + In(s) -0.34 Ca (aq) + 2e + Cd(s) -0.40 Fe (aq) + 2e + Fe(s) -0.45 Cr (aq) + 3e + Cr(s) -0.73 Zn2+ (aq) + 2e + Zn(s) -0.76
A voltaic electrochemical cell is constructed using the following reaction. The half-cell components are separated by a salt bridge. Br2(1) + Mn(s) 2Br"(aq) + Mn2+(aq) Write the reactions that take place at the anode and at the cathode, the direction in which the electrons migrate in the external circuit, and the direction the anions in the salt bridge migrate. Use smallest possible integer coefficients. If a box is not needed, leave it blank. Enter the reaction that takes place at the anode. Include state symbols: Enter the reaction that takes place at the cathode. Include state symbols: In the external circuit, electrons migrate the Mn electrode the Br2 electrode. Anions migrate the salt bridge the Br2 compartment.
Consider the voltaic cell: Mg Mg2+ (1.0 M)||H* (1.0 M)|H₂ (1 atm)|Pt(s) Which of the following changes will cause a decrease in the cell voltage? increase the pressure of H₂ at 2.0 atm decrease the mass of the Mg electrode O decrease the concentration of Mg2+ ion lower the pH of the catholyte
Consider a voltaic cell in which the reaction is Zn (s) + 2H+ (aq) → Zn2+ (aq) + H2 (g) It is found that the cell voltage is +0.530 V when [Zn2+] = 1.0 M, PH2 = 1.0 atm. What must be the concentration of H+ in the cell? (Use the following information) (Show your work) 2H+ (aq) + 2e- → H2 (g) Eºred = 0.000 V Zn2+ (aq) + 2e- → Zn(s) Eºred = -0.762 V
Consider the voltaic cell with a standard potential of 0.25V: Ni | Ni2+ (1.0 M) | H+ (1.0 M) | H2 (1 atm) | Pt what is the value of the equilibrium constant for the reaction at 298 K?
The cell notation of a voltaic cell is: Zn(s) | Zn2+(aq; 0.02M) || Zn2+(aq; 1.0 M) | Zn (s) Draw a diagram of the cell and each half-reaction. Label the anode, cathode, and each relevant reaction. What is Eocell at equilibrium? Why? What is the expected Ecell at T = 273K? Given this Ecell, will the Q of this cell increase or decrease to reach equilibrium?
Consider the following voltaic cellat 25°C: Al(s) | Al3*(0.20 M, aq) || Al3+(0.75 M, aq) | Al(s) If the standard reduction potential for the Al3+(aq) /Al(s) redox couple is -1.66 V, what is the overall cell reaction and the cell potential of the voltaic cell shown above? (Reference the cell as written above.) The overall cell reaction is Al3+(0.75 M, aq) AIS*(0.20 M, ag) and E°cell = +0.0113 V. There is no overall cell reaction and E°cell = 0.00 V. The overall cell reaction is Al3+(0.20 M, aq) Als*(0.75 M, aq) and E°cell = +0.0113 V. The overall cell reaction is Al3+(0.20 M, aq) →A13+(0.75 M, ag) and E°cell| = -0.0113 V. The overall cell reaction is Al3*(0.75 M, aq) →AI3*(0.20 M, aq) and E°cell = -0.0113 V. None of these
A voltaic cell is constructed in which the anode is a Al|Al3+ half cell and the cathode is a H2|H+ half cell. The half-cell compartments are connected by a salt bridge. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) The anode reaction is: + + The cathode reaction is: + + The net cell reaction is: + + In the external circuit, electrons migrate the H2|H+ electrode the Al|Al3+ electrode.In the salt bridge, anions migrate the Al|Al3+ compartment the H2|H+ compartment. Submit Answer Retry Entire Group 1 more group attempt remaining
Consider the following half-reactions and their standard reduction potentials then give the standard line (cell) notation for a voltaic cell built on these half reactions. Mn2*(aq) + 2 e Mn(s) E° = -1.18 V Fe(aq) +3 e Fe(s) E° = -0.036 V A. Fe(s) | Fe3t(aq, 1.0 M) || Mn (s) | Mn 2*(aq. 1.0 M) B. Mn (s) | Mn 2*(aq, 1.0 M) | | Fe(s) | Fe(aq. 1.0 M) C. Fe(s) | Fe3t(aq. 1.0 M) || Mn2*(aq, 1.0 M) | Mn(s) D. Mn (s) | Mn 2*(aq. 1.0 M) || Fe(aq, 1.0 M) | Fe(s)
-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 anode is a Sn|Sn²+ half cell and the cathode is a Cu+| Cu²+ half cell. The half-cell compartments are connected by a salt bridge. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) I The anode reaction is: + The cathode reaction is: + The net cell reaction is: + In the external circuit, electrons migrate electrode the Cu+I Cu²+ electrode. In the salt bridge, anions migrate the Sn|Sn²+ compartment. + + + the Sn|Sn²+ the Cu+I Cu2+ compartment
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. +