Chemistry Atoms First2e
2nd Edition
ISBN: 9781947172647
Author: OpenStax
Publisher: OpenStax College
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Textbook Question
Chapter 16, Problem 36E
Using the information thus far in this chapter, explain why battery-powered electronics perform poorly in low temperatures.
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Topic: Photochemistry and Photophysics of Supramolecules
Chapter 16 Solutions
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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- When two solutions, one of 0.1 M KCl (I) and the other of 0.1 M MCl (II), are brought into contact by a membrane. The cation M cannot cross the membrane. At equilibrium, x moles of K+ will have passed from solution (I) to (II). To maintain the neutrality of the two solutions, x moles of Cl- will also have to pass from I to II. Explain this equality: (0.1 - x)/x = (0.1 + x)/(0.1 - x)arrow_forwardCalculate the variation in the potential of the Pt/MnO4-, Mn2+ pair with pH, indicating the value of the standard potential. Data: E0 = 1.12.arrow_forwardGiven the cell: Pt l H2(g) l dis X:KCl (sat) l Hg2Cl2(s) l Hg l Pt. Calculate the emf of the cell as a function of pH.arrow_forward
- The decimolar calomel electrode has a potential of 0.3335 V at 25°C compared to the standard hydrogen electrode. If the standard reduction potential of Hg22+ is 0.7973 V and the solubility product of Hg2Cl2 is 1.2x 10-18, find the activity of the chlorine ion at this electrode.Data: R = 8.314 J K-1 mol-1, F = 96485 C mol-1, T = 298.15 K.arrow_forward2. Add the following group of numbers using the correct number of significant figures for the answer. Show work to earn full credit such as rounding off the answer to the correct number of significant figures. Replace the question marks with the calculated answers or write the calculated answers near the question marks. 10916.345 37.40832 5.4043 3.94 + 0.0426 ? (7 significant figures)arrow_forwardThe emf at 25°C of the cell: Pt l H2(g) l dis X:KCl (sat) l Hg2Cl2(s) l Hg l Pt was 612 mV. When solution X was replaced by normal phosphate buffer solution with a pH of 6.86, the emf was 741 mV. Calculate the pH of solution X.arrow_forward
- Indicate how to calculate the potential E of the reaction Hg2Cl2(s) + 2e ⇄ 2Hg + 2Cl- as a function of the concentration of Cl- ions. Data: the solubility product of Hg2Cl2.arrow_forwardHow can Beer’s Law be used to determine the concentration in a selected food sample. Provide an in-depth discussion and examples of this.arrow_forwardb) H3C- H3C Me CH 3 I HN Me H+arrow_forward
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