Chemistry Atoms First2e
2nd Edition
ISBN: 9781947172647
Author: OpenStax
Publisher: OpenStax College
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Textbook Question
Chapter 16, Problem 35E
Use the Nernst equation to explain the drop in voltage observed for some batteries as they discharge.
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Chemistry Atoms First2e
Ch. 16 - Identify each half-reaction below as either...Ch. 16 - Identify each half-reaction below as either...Ch. 16 - Assuming each pair of half-reactions below takes...Ch. 16 - Balance the equations below assuming they occur in...Ch. 16 - Identify the oxidant and reductant of each...Ch. 16 - Balance the equations below assuming they occur in...Ch. 16 - Identify the oxidant and reductant of each...Ch. 16 - Why dont hydroxide ions appear in equations for...Ch. 16 - Why dont hydrogen ions appear in equations for...Ch. 16 - Why must the charge balance in oxidation-reduction...
Ch. 16 - Write cell schematics for the following cell...Ch. 16 - Assuming the schematics below represent galvanic...Ch. 16 - Write a balanced equation for the cell reaction of...Ch. 16 - Balance each reaction below, and write a cell...Ch. 16 - Identify the oxidant and reductant in each...Ch. 16 - From the information provided, use cell notation...Ch. 16 - Why is a salt bridge necessary in galvanic cell...Ch. 16 - An active (metal) electrode was found to gain mass...Ch. 16 - An active (metal) electrode was found to lose mass...Ch. 16 - The masses of three electrodes (A, B, and C), each...Ch. 16 - Calculate the standard cell potential for each...Ch. 16 - Calculate the standard cell potential for each...Ch. 16 - Write the balanced cell reaction for the cell...Ch. 16 - Determine the cell reaction and standard cell...Ch. 16 - Determine the cell reaction and standard cell...Ch. 16 - Write the balanced cell reaction for the cell...Ch. 16 - For each pair of standard cell potential and...Ch. 16 - For each pair of standard free energy change and...Ch. 16 - Determine the standard cell potential and the cell...Ch. 16 - Determine ∆G and ∆G for each of the reactions...Ch. 16 - Use the data in Appendix L to calculate...Ch. 16 - Consider a battery made from one half-cell that...Ch. 16 - Consider a battery with the overall reaction:...Ch. 16 - Why do batteries go dead, but fuel cells do not?Ch. 16 - Use the Nernst equation to explain the drop in...Ch. 16 - Using the information thus far in this chapter,...Ch. 16 - Which member of each pair of metals is more likely...Ch. 16 - Consider the following metals: Ag, Au, Mg, Ni, and...Ch. 16 - Aluminum (EoA13+/A1=-2.07V) is easily oxidized...Ch. 16 - If a sample of iron and a sample of zinc come into...Ch. 16 - Suppose you have three different metals. A, B, and...Ch. 16 - Why would a sacrificial anode made of lithium...Ch. 16 - If a 2.5 A current flows through a circuit for 35...Ch. 16 - For the scenario in the previous question, how...Ch. 16 - Write the half-reactions and cell reaction...Ch. 16 - What mass of each product is produced in each of...Ch. 16 - How long would it take to reduce 1 mole of each of...Ch. 16 - A Current of 2.345 A passes through the Shown in...Ch. 16 - An irregularly shaped metal part made from a...
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- The mass of three different metal electrodes, each from a different galvanic cell, were determined before and after the current generated by the oxidation-reduction reaction in each cell was allowed to flow for a few minutes. The first metal electrode, given the label A, was found to have increased in mass; the second metal electrode, given the label B, did not change in mass; and the third metal electrode, given the label C, was found to have lost mass. Make an educated guess as to which electrodes were active and which were inert electrodes, and which were anode(s) and which were the cathode(s).arrow_forwardFor each reaction listed, determine its standard cell potential at 25 C and whether the reaction is spontaneous at standard conditions. (a) Mn(s)+Ni2+(aq)Mn2+(aq)+Ni(s) (b) 3Cu2+(aq)+2Al(s)2Al3+(aq)+3Cu(s) (c) Na(s)+LiNO3(aq)NaNO3(aq)+Li(s) (d) Ca(NO3)2(aq)+Ba(s)Ba(NO3)2(aq)+Ca(s)arrow_forwardAn electrolysis experiment is performed to determine the value of the Faraday constant (number of coulombs per mole of electrons). In this experiment, 28.8 g of gold is plated out from a AuCN solution by running an electrolytic cell for two hours with a current of 2.00 A. What is the experimental value obtained for the Faraday Constant?arrow_forward
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