a You have a concentration cell with Cu electrodes and [Cu2+] = 1.00 M (right side) and 0.0085 M (left side). Calculate the potential for this cell at 25°C. Ecell = 0.061 Correct Since the concentration cell is given, E°cell = 0. 0.0591 8.5 x 10-3 E = 0- - log( =0.061V 1.00 b You have a concentration cell with Cu electrodes and [Cu2+] Cu2+ ion reacts with NH3 to form Cu(NH3)4* = 1.00 M (right side) and 0.0085 M (left side). The 2+ by the following equation: Cu2+(aq) + 4NH3(aq) → Cu(NH3)42+(aq) K = 1.0x1013 Calculate the new cell potential after enough NH3 is added to the left cell compartment such that at equilibrium [NH3] = 1.3 M. Ecell = V

a You have a concentration cell with Cu electrodes and [Cu2+] = 1.00 M (right side) and 0.0085 M (left side). Calculate the potential for this cell at 25°C. Ecell = 0.061 Correct Since the concentration cell is given, E°cell = 0. 0.0591 8.5 x 10-3 E = 0- - log( =0.061V 1.00 b You have a concentration cell with Cu electrodes and [Cu2+] Cu2+ ion reacts with NH3 to form Cu(NH3)4* = 1.00 M (right side) and 0.0085 M (left side). The 2+ by the following equation: Cu2+(aq) + 4NH3(aq) → Cu(NH3)42+(aq) K = 1.0x1013 Calculate the new cell potential after enough NH3 is added to the left cell compartment such that at equilibrium [NH3] = 1.3 M. Ecell = 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

[References) What are the reaction quotient (Q) and the calculated value of the cell potential (Ecell) at 298 K for an electrochemical cell with the following reaction, when the Hg2+ concentration is 7.35x104 M and the Mg²* concentration is 1.25 M? Hg"(aq) + Mg(s) Hg(l) + Mg²+(aq) E°cell = 3.225 V Q= Ecel =|
Thank you!
The free energy change for the following reaction at 25 °C, when [Ag*] = 1.20 M and [Cu2+] = 8.38x10-3 M, is -101 kJ: 2Ag*(1.20 M) + Cu(s)2Ag(s) + Cu2+(8.38x10-3 M) AG = -101 kJ What is the cell potential for the reaction as written under these conditions? Answer: V Would this reaction be spontaneous in the forward or the reverse direction v forward reverse
Please show all steps thank you.
Salt bridge U A concentration cell similar to the one shown is composed of two Cu electrodes and solutions of different Cu²+ concentrations. The left compartment contains 0.272 M Cu²+, and the right compartment contains 1.25 M Cu²+ . Calculate the cell potential for this reaction at 298 K. volts In this copper concentration cell, the compartment on the left is the + and the compartment on the right is the +
image #7
Calculate the Ecell value at 298 K for the cell based on the reaction: Cu(s)+2Ag*(aq) Cu?+(aq) + 2Ag(s) where [Ag*] = 0.00150 M and [Cu2+] = 7.50x10-4 M. The standard reduction potentials are shown below: Ag"(aq) +e - Ag(s) E° = 0.7996 V Cu+ (aq)+ 2e → Cu(s) E° = 0.3419 V
Question 3 D Voltage Source Zn 로 salt bridge ZnSO4 Question 4 If the cell pictured above is driven as an electrolytic cell: The electrons would flow (Select ] The following statement is true: [Select] Cu The standard (assuming 1 M concentrations) cell potential is [Select ] If the salt bridge contains KCI, then [Select] CuSO4 In order to decrease (make it a smaller number) the potential necessary for electrolysis, [Select] If the current is set to a constant of 3.82 A for 5.00 min, then (Select] of metal would deposit on the cathode.
Calculate E, E, and AG for the following cell reaction: 3Zn(s) + 2Cr*(aq) 3Zn²* (ag) + 2Cr (s) where Cr*= 0.040 M and Zn*]=0.0095 M. Round each of your answers to 2 significant digits. -[c*]- Note: Reference the Standard reduction potentials at 25 °C table for additional information. J Note: The Faraday constant is 9.649 x 10* V•mol Part: 0 / 3 Part 1 of 3 Save For Skip Part Check O 2022 McGraw Hill LLC. All Rights Reserved. Terms of f a 73*F Clear Cbp 12 IO1 40 1454 esc & 7 96 %24 4. %23 3. R T Y tab D caps lock mit 1 V. In elf B. SI
Q4 A: What is the E for the Fe3+/Fe2+ half-cell if [Fe3+] = 0.001 M and [Fe2+] is 0.1 M at 25 °C? if you know Fe reduction potential = + 0.771 V *
Can someone please help with this question
Question 15 of 23 Submit For the electrochemical cell 2 Al(s) + 3 Mn²*(aq) – 2 Als*(aq) + 3 Mn(s) (E° = 0.48 V, [AI**] = 1.0 M), what is the value of E when [ Mn2*] = 0.013 M? Assume T is 298 K | v 1 2 3 C 7 9. +/- x 10 0 LO 00