A galvanic cell is powered by the following redox reaction:2+2 Zn(aq) + N₂H4(aq) + 4OH¯(aq) 2 Zn(s) + N₂(g) + 4H₂O(1)Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab.Write a balanced equation forthe half-reaction that takesplace at the cathode.Write a balanced equation forthe half-reaction that takesplace at the anode.Calculate the cell voltageunder standard conditions.Round your answer to 2decimal places.000EVX00Ś

Answer:Galvanic cell is a type of electrochemical cell that converts chemical energy into electrical…

A galvanic cell is powered by the following redox reaction: 2+ 2 Zn²+ (aq) + N₂H₁(aq) + 4OH¯(aq) → 2 Zn(s) + N₂(g) + 4 H₂O(l) Answer the following questions about this cell. If you need any electrochemical data, Write a balanced equation for the half-reaction that takes place at the cathode. Write a balanced equation for the half-reaction that takes place at the anode. Calculate the cell voltage under standard conditions. Round your answer to 2 decimal places. 0 E = Ov

A galvanic cell is powered by the following redox reaction: 2+ 2 Zn²+ (aq) + N₂H₁(aq) + 4OH¯(aq) → 2 Zn(s) + N₂(g) + 4 H₂O(l) Answer the following questions about this cell. If you need any electrochemical data, Write a balanced equation for the half-reaction that takes place at the cathode. Write a balanced equation for the half-reaction that takes place at the anode. Calculate the cell voltage under standard conditions. Round your answer to 2 decimal places. 0 E = Ov

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 galvanic cell is powered by the following redox reaction: 2+ 2 HNO₂(aq) + 2H(aq) + Zn(s) 2 NO(g) + 2 H₂O(1) + Zn²+ (aq) Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab. Write a balanced equation for the half-reaction that takes place at the cathode. Write a balanced equation for the half-reaction that takes place at the anode. Calculate the cell voltage under standard conditions. Round your answer to 2 decimal places. 0 0 E Ov ローロ e X
A chemist designs a galvanic cell that uses these two half-reactions: Cl₂(g)+2e + 2 103(aq) + 12 H (aq) +10e 1₂(s) + 6H₂O(1) Write a balanced equation for the half-reaction that O happens at the cathode. Answer the following questions about this cell. 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? half-reaction If you said it was possible to calculate the cell voltage, do so and enter your answer here. Round your, answer to 3. significant digits. 0 Yes 2 CI (ag) O No Ov standard reduction potential Eº = +1.359 V 'red E = +1.195 V red 0-0 0x10 Ś
Please don't provide handwritten solution
An aqueous copper (II) chloride solution is electrolyzed for a period of 156 minutes. Using a current of 9.00 A. If inert electrodes are used in the process, how many grams of copper were removed from the solution?
A galvanic cell is powered by the following redox reaction: Cl(9) + H2(g) + 2OH (aq) → 2Cl (aq) + 2 H,O(1) Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab. Write a balanced equation for the half-reaction that takes place at the cathode. Write a balanced equation for the half-reaction that takes place at the anode. Calculate the cell voltage under standard conditions. E = Ov Round your answer to 2 decimal places. la
When a lead acid car battery is recharged by the alternator, it acts essentially as an electrolytic cell in which solid lead(II) sulfate (PBSO4) is reduced to lead at the cathode and oxidized to solid lead(II) oxide (PbO) at the anode. Suppose a current of 46.0 A is fed into a car battery for 24.0 seconds. Calculate the mass of lead deposited on the cathode of the battery. Round your answer to 3 significant digits. Also, be sure your answer contains a unit symbol.
An electrochemical cell is constructed by dipping a zinc rod in a solution of Zn(NO3)2(aq), dipping a cobalt rod in a solution of CoCl2(aq), and connecting them with a wire and a salt bridge. In the cell that is constructed, the metallic zinc is being oxidized. d. The standard cell potential for this electrochemical cell is 0.482 V and two moles of electrons are exchanged per mole of reaction. What is equilibrium constant, K, for the redox reaction described by this electrochemical cell at 298 K?
A gold (III) chloride solution was electrolyzed using a current of 13.5 amperes for four hours. How many grams of gold (atomic mass = 197 g/mol) was plated out in this electrochemical process?The electrochemical process at the cathode is:Au+3(aq) + 3 e → Au
Write a balanced chemical equation (including states of matter) for an electrochemical cell that has a copper cathode immersed in a solution of Cu2+ ions, and a lead anode immersed in a solution of Pb2+ ions.
Write the balanced chemical equation for the spontaneous redox reaction. Include states of matter. Calculate the standard cell potential. If the initial concentrations of Zn2+ and of OH– are 1.0 × 10–7 and 2.0 × 10–7, respectively, calculate the cell potential after the Zn2+ concentration has increased by a factor of 100. At this point, what percentage of the initial voltage remains?
Write the balanced equation for the overall reaction that occurs in the cell.Calculate E ̊ for the overall reaction. A 150. mL sample of CH 3OH (aq) is put into the electrochemical cell. The cell produces an average current of 0.0100 amp for 250. seconds, at which point the CH3OH (aq) has been totally consumed. Calculate the charge, in coulombs, that passed through the cell.
A galvanic cell is powered by the following redox reaction: + 2+ HNO₂(aq) + H+ (aq) + Cu¹ (aq) → NO(g) + H₂O(1) + Cu²+ (aq) Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab. Write a balanced equation for the half-reaction that takes place at the cathode. Write a balanced equation for the half-reaction that takes place at the anode. Calculate the cell voltage under standard conditions. Round your answer to 2 decimal places. 0 E = V 0-0 e X 00