A voltaic cell consists of Cu?*/Cu and Cd²*/Cd half-cells. Eachcompartment has a volume of 0.500 L with the following initialconcentrations: [Cu2*] = 1.250 M; [Cd2*] = 0.250 M at 25°C. What isthe [Cu2*] when the voltage has dropped to 0.727 V? (E° for Cu²*/Cu= 0.340 V and Eº for Cd2*/Cd = -0.400 V.)%D%3D

Given data,Initial [Cu2+]=1.250MInitial [Cd2+]=0.250MVolume of each…

A voltaic cell consists of Cu2*/Cu and Cd²*/Cd half-cells. Each compartment has a volume of 0.500 L with the following initial concentrations: [Cu²*] = 1.250 M; [Cd²*] = 0.250 M at 25°C. What is the [Cu2*] when the voltage has dropped to 0.727 V? (Eº for Cu²*/Cu = 0.340 V and E° for Cd2*/Cd = -0.400 V.)

A voltaic cell consists of Cu2/Cu and Cd²/Cd half-cells. Each compartment has a volume of 0.500 L with the following initial concentrations: [Cu²] = 1.250 M; [Cd²] = 0.250 M at 25°C. What is the [Cu2] when the voltage has dropped to 0.727 V? (Eº for Cu²/Cu = 0.340 V and E° for Cd2*/Cd = -0.400 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

A voltaic cell is constructed in which the anode is a Cr|Cr3+ half cell and the cathode is a H2|H+ half cell. The half-cell compartments are connected by a salt bridge.
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 =
Consider the galvanic cell based on the following half-reactions. Ag+ + e → Ag Cd²+ + 2e →→ Cd (a) Determine the overall cell reaction and calculate º chemPad XX² cell 8° = +0.80 V 8⁰ = -0.40 V V AGO K Help Greek (b) Calculate AGº (in kJ) and K for the cell reaction at 25°C. kJ (in V). (Use the lowest possible whole number coefficients. Omit states-of-matter from your answer.) cell (c) Calculate cell (in V) at 25°C when [Ag+ ] = V 1.0×10-4 M and [Cd²+] = 1.0×10-² M.
Consider a galvanic cell with the anode containing a Zn metal electrode and a 0.10M Zn(NO3)2 solution and the other half-cell containing a Sn metal electrode and a 0.10M Sn(NO3)2 solution. If the measured Ecell value is +650mV and the Zn2+/Zn reduction potential is assumed to be -790mV, what is the Sn2+/Sn reduction potential?
Consider the following electrochemical cell at a pH of 8.00:Cu(s)|Cu2+(aq, 0.0125 M) || VO2+( aq, 0.00125 M), VO2+( 0.0250 M)b. Calculate E0cell for this system.
A voltaic cell using Pb²⁺/Pb and Ni²⁺/Ni half-cells is set up at standard conditions, and each compartment has a volume of 355 mL. What is the cell potential, in V, after it has delivered 0.150 A for 51.0 hours at 25 °C? (E° for Pb²⁺/Pb = -0.130 V and E° for Ni²⁺/Ni = -0.250 V.)
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 consists of an Al/Al3+ half-cell and a Fe2+/Fe3+ half-cell. The standard reduction potential for Al3+ is −1.66V and for Fe3+ is 0.77 V. Calculate Ecell at 25 ºC when the concentration of [Al3+] = 9.51 x 10-4 M , [Fe3+]= 6.24 x 10-3 M, and [Fe2+]= 5.74 x 10-5 M
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. +
5. What is voltage of the following cell? Sn(s) | Sn(NO3)2 (0.100 M) || AgNO3(0.020 M) | Ag(s)
When [Hg2+] = 1.37 M, the observed cell potential at 298 K for an electrochemical cell with the reaction shown below is 3.321 V. What is the Mg2+ concentration in this cell? Hg2+(aq) + Mg(s) Hg(t) + Mg2+(aq) [Mg2+] = mol/L Submit