Dariana Using the Nernst equation to calculate nonstandard cell voltage A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: Sn" (aq) + Ba (s)→ Sn (s) + Ba-™ (aq) 2+ Suppose the cell is prepared with 2.40 M Sn in one half-cell and 0.623 M Ba' 2+ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. alo

Dariana Using the Nernst equation to calculate nonstandard cell voltage A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: Sn" (aq) + Ba (s)→ Sn (s) + Ba-™ (aq) 2+ Suppose the cell is prepared with 2.40 M Sn in one half-cell and 0.623 M Ba' 2+ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. alo

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

1 Using the Nernst equation to calculate nonstandard cell voltage A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 210, (aq) + 12H* (aq) + 5Co (s) 1₂ (s) + 6H₂0 (1) + 5 Co²+ (aq) Suppose the cell is prepared with 6.91 MIO3 and 2.94 M H in one half-cell and 5.58 M Co²* in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. 0 D.D X 5
A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 3+ 2 Cr³+ (aq) +3Ca (s) → 2Cr (s) + 3Ca²+ (aq) 3+ 2+ Suppose the cell is prepared with 4.58 M Cr³+ in one half-cell and 2.50 M Ca²+ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. 0 x10 X μ 010
What is the cell potential (E) for a galvanic cell formed from the following two half-reactions? Assume that the cell temperature is 38°C and the operating pressure is 0.04 atm. Cd2*(aq) + 2 e- → Cd(s); [Cd2*] = 0.50 M E° = -0.403 V Mg2*(aq) + 2 e- → Mg(s); [Mg*] = 2.75 M E° = -2.37 V A) 1.90 V B) 1.95 V 1.99 V D) 2.20 V
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.
A galvanic cell using Mg / Mg*" and Cu / Cu" half-cells operates under standard-state conditions at 25 °C, and each compartment has a volume of 227 mL. The cell delivers 0.31 A for 32.1 h. (a) How many grams of Cu are deposited? g Cu
|| Using the Nernst equation to calculate nonstandard cell voltage A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 0 2+ 2+ Cu (aq) + Zn (s) → Cu (s) + Zn²+ (aq) 2+ 2+ Suppose the cell is prepared with 1.39 M Cu in one half-cell and 2.14 M Zn in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. 0 x10 ロ・ロ X μ
Please answer the follow up question
the Nernst equation to calculate nonstandard cell voltage A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 2+ Sn²+ (aq) + Ba(s) → Sn (s) + Ba²+ (aq) 2+ 2+ in one half-cell and 3.14 M Ba Suppose the cell is prepared with 2.84 M Sn Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. 0 ロ・ロ μ 00 09 Ś ? in the other.
Calculate the cell voltage under these conditions. Round your answer to 3 significant digits.
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
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential CrO2−4 (aq)+4H2O(l)+3e−→ CrOH3(s)+5OH−(aq) =E0red−0.13V Cl2(g)+2e−→ 2Cl−(aq) =E0red+1.359V Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. Do you have enough information to calculate the cell voltage under standard conditions? If you said it was possible to calculate the cell voltage, do so and enter your answer here. Be sure your answer has the correct number of significant digits. V
Sketch a galvanic cell ( immersed in 1M solution) with the cell notation Cr(s)/Cr 3+ (aq) // Cu2+/Cu (s) Please indicate the anode and cathode, the flow of electrons, the reaction in the anode and cathode, overall reaction, and the voltage of the cell- is it spontaneous