A Zn²+ Zn half-cell is connected to a Cu²+ Cu half-cell to make a galvanic cell, in which [Zn²+] = [Cu²+] = 1.00 M. The cell potential at 25°C is measured to be AE corresponds to the overall cell reaction 1.10 V, which "cell Zn(s) + Cu²* (aq) → Zn²* (aq) + Cu(s) Calculate AG for this reaction under the given conditions.

A Zn²+ Zn half-cell is connected to a Cu²+ Cu half-cell to make a galvanic cell, in which [Zn²+] = [Cu²+] = 1.00 M. The cell potential at 25°C is measured to be AE corresponds to the overall cell reaction 1.10 V, which "cell Zn(s) + Cu²* (aq) → Zn²* (aq) + Cu(s) Calculate AG for this reaction under the given conditions.

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

Find the voltage of the cell if the right half-cell contains 0.330 M AgNO₃ (aq) and the left half-cell contains 0.115 M Cu(NO₃)₂ (aq). Express your answer to three significant figures.
Write the cell notation for an electrochemical cell consisting of an anode where Zn (s) is oxidized to Zn²+ (aq) and a cathode where H* (aq) is reduced to H2₂ (g) at a platinum electrode . Assume all aqueous solutions have a concentration of 1 mol/L and gases have a pressure of 1 bar.
Calculate the cell potential for the galvanic cell in which the given reaction occurs at 25 °C, given that [Sn**] = 0.0666 M, [Fe*1 = 0.0301 M, [Sn*+] = 0.00345 M, and [Fe2+] = 0.01092 M. Standard reduction potentials can be found in this table. Sn²*(aq) + 2 Fe* (aq) = Sn*(aq) + 2 Fe²+*(aq) E = V
A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 3Cu (aq) + 2A1 (s) 3Cu (s)+2A1* (aq) 2+ 3+ Suppose the cell is prepared with 2.15 M Cu“ in one half-cell and 7.31 M Al" in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. AL Rights
For the galvanic cell 2Ag+ + Cr → 2Ag + Cr2+, which equation allows you to correctly calculate the standard cell potential?
4. A galvanic cell consisting of a magnesium electrode and a standard hydrogen electrode is constructed. The cell generates a voltage, Ecell, of 2.099 V. The standard reduction potential for the two half-cell reactions are as follows: Mg²+ (aq) + 2e → Mg (s) 2H+ (aq) + 2e → H₂ (g) -2.38 V OV (i) Determine the standard cell potential, Eºcell. (ii) Assuming a Mg²+ (aq) concentration of 1 mol dm³ and a H₂ (g) pressure of 1 atm, calculate the theoretical pH of the cell. You may use concentrations/partial pressures in place of activities.
A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: Cu?* (aq)+Zn (s) → Cu (s) +Zn²* (aq) Suppose the cell is prepared with 3.40 M Cu´" in one half-cell and 5.47 M Zn2+ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. x10
[Fe3+]= 2.0×10−3 M; [Mg2+]= 3.15 M Express your answer in units of volts.
Write the cell notation for an electrochemical cell consisting of an anode where H, (g) is oxidized to Ht (aq) at a platinum electrode and a cathode where Ag* (aq) is reduced to Ag (s) . Assume all aqueous solutions have a concentration of 1 mol/L and gases have a pressure of 1 bar.
What is the cell potential (E0) for a galvanic cell formed from the following two half-reactions? Assume that the cell temperature is 45°C and the operating pressure is 0.06 atm. Fe2+(aq) + 2 e− ↔ Fe(s) ; [Fe2+] = 2.25 M E0 = −0.44 V Ag+(aq) + e− ↔ Ag(s) ; [Ag+] = 1.55 × 10−4 M E0 = 0.7994 V
A voltaic cell is being constructed from an Al/A|^ 3+ electrode and a Sn/Sn^ 2+ electrodeWhen constructed properly and the circuit is closed, the tin electrode is observed to gain mass and the overall cell potential to be 1.52V. Which of the following chemical reactions takes place at the cathode? Al3+(aq) + 3e- → Al(s) Sn(s) → Sn2+(aq) + 2e- Sn2+(aq) + 2e- → Sn(s) Al(s) → Al3+(aq) + 3e- Based on the overall reaction taking place across the voltaic cell, how many moles of electrons are involved? When electrons are flowing in the cell, which electrode gains mass? True or false: If an aluminum electrode is set to be part of a voltaic cell that also involves a standard hydrogen electrode (SHE), the aluminum electrode would be the anode.
In the given electrochemical cell, what is the cathode half-reaction? Zn(s) | Zn2+(aq) || Fe3+(aq), Fe2+(aq) | Pt(s)