Connect for Chemistry
13th Edition
ISBN: 9781260161854
Author: Raymond Chang, Jason Overby
Publisher: Mcgraw-hill Higher Education (us)
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Chapter 18, Problem 18.13QP
Predict whether Fe3+ can oxidize I− to I2 under standard-state conditions.
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Chapter 18 Solutions
Connect for Chemistry
Ch. 18.1 - Balance the following equation for the reaction in...Ch. 18.1 - Determine the number of electrons transferred in...Ch. 18.1 - For the following reaction in acidic solution,...Ch. 18.2 - Write the cell diagram for the following redox...Ch. 18.2 - Write the balanced redox reaction corresponding to...Ch. 18.3 - Can Sn reduce Zn2+(aq) under standard-state...Ch. 18.3 - What is the standard emf of a galvanic cell made...Ch. 18.3 - Prob. 1RCFCh. 18.3 - Prob. 2RCFCh. 18.4 - Prob. 4PE
Ch. 18.4 - Prob. 5PECh. 18.4 - Calculate the equilibrium constant for the...Ch. 18.4 - Prob. 2RCFCh. 18.4 - Prob. 3RCFCh. 18.5 - Prob. 6PECh. 18.5 - Prob. 7PECh. 18.5 - Consider the following cell diagram:...Ch. 18.5 - Calculate the cell voltage at 25C of a...Ch. 18.6 - How many Leclanch cells are contained in a 9-volt...Ch. 18.7 - Prob. 1RCFCh. 18.8 - An aqueous solution of Mg(NO3)2 is electrolyzed....Ch. 18.8 - A constant current is passed through an...Ch. 18.8 - What is the minimum voltage needed for the...Ch. 18.8 - Prob. 2RCFCh. 18.8 - In the electrolysis of molten CaCl2, a current of...Ch. 18 - Balance the following redox equations by the...Ch. 18 - Balance the following redox equations by the...Ch. 18 - Define the following terms: anode, cathode, cell...Ch. 18 - Describe the basic features of a galvanic cell....Ch. 18 - What is the function of a salt bridge? What kind...Ch. 18 - What is a cell diagram? Write the cell diagram for...Ch. 18 - What is the difference between the half-reactions...Ch. 18 - Prob. 18.8QPCh. 18 - Use the information in Table 2.1, and calculate...Ch. 18 - Discuss the spontaneity of an electrochemical...Ch. 18 - Calculate the standard emf of a cell that uses the...Ch. 18 - Calculate the standard emf of a cell that uses...Ch. 18 - Predict whether Fe3+ can oxidize I to I2 under...Ch. 18 - Which of the following reagents can oxidize H2O to...Ch. 18 - Consider the following half-reactions:...Ch. 18 - Predict whether the following reactions would...Ch. 18 - Which species in each pair is a better oxidizing...Ch. 18 - Which species in each pair is a better reducing...Ch. 18 - Consider the electrochemical reaction Sn2+ + X Sn...Ch. 18 - The Ecell for the following cell is 1.54 V at 25C:...Ch. 18 - Write the equations relating G and K to the...Ch. 18 - Prob. 18.22QPCh. 18 - Prob. 18.23QPCh. 18 - The equilibrium constant for the reaction...Ch. 18 - Use the standard reduction potentials to find the...Ch. 18 - Calculate G and Kc for the following reactions at...Ch. 18 - Under standard-state conditions, what spontaneous...Ch. 18 - Given that E = 0.52 V for the reduction...Ch. 18 - Prob. 18.29QPCh. 18 - Write the Nernst equation for the following...Ch. 18 - What is the potential of a cell made up of Zn/Zn2+...Ch. 18 - Calculate E, E, and G for the following cell...Ch. 18 - Calculate the standard potential of the cell...Ch. 18 - Referring to the arrangement in Figure 18.1,...Ch. 18 - Calculate the emf of the following concentration...Ch. 18 - Explain the differences between a primary galvanic...Ch. 18 - Discuss the advantages and disadvantages of fuel...Ch. 18 - The hydrogen-oxygen fuel cell is described in...Ch. 18 - Calculate the standard emf of the propane fuel...Ch. 18 - Prob. 18.41QPCh. 18 - Galvanized iron is steel sheet that has been...Ch. 18 - Tarnished silver contains Ag2S. The tarnish can be...Ch. 18 - Prob. 18.44QPCh. 18 - What is the difference between a galvanic cell...Ch. 18 - Describe the electrolysis of an aqueous solution...Ch. 18 - The half-reaction at an electrode is...Ch. 18 - Consider the electrolysis of molten barium...Ch. 18 - Prob. 18.49QPCh. 18 - If the cost of electricity to produce magnesium by...Ch. 18 - One of the half-reactions for the electrolysis of...Ch. 18 - How many moles of electrons are required to...Ch. 18 - Calculate the amounts of Cu and Br2 produced in...Ch. 18 - In the electrolysis of an aqueous AgNO3 solution,...Ch. 18 - A steady current was passed through molten CoSO4...Ch. 18 - A constant electric current flows for 3.75 h...Ch. 18 - What is the hourly production rate of chlorine gas...Ch. 18 - Chromium plating is applied by electrolysis to...Ch. 18 - The passage of a current of 0.750 A for 25.0 min...Ch. 18 - A quantity of 0.300 g of copper was deposited from...Ch. 18 - In a certain electrolysis experiment, 1.44 g of Ag...Ch. 18 - One of the half-reactions for the electrolysis of...Ch. 18 - A steady current of 10.0 A is passed through three...Ch. 18 - Industrially, copper metal can be purified...Ch. 18 - A Daniell cell consists of a zinc electrode in...Ch. 18 - A concentration cell is constructed having Cu...Ch. 18 - For each of the following redox reactions, (i)...Ch. 18 - The oxidation of 25.0 mL of a solution containing...Ch. 18 - The SO2 present in air is mainly responsible for...Ch. 18 - Prob. 18.70QPCh. 18 - Prob. 18.71QPCh. 18 - Oxalic acid (H2C2O4) is present in many plants and...Ch. 18 - Prob. 18.73QPCh. 18 - Prob. 18.74QPCh. 18 - From the following information, calculate the...Ch. 18 - Consider a galvanic cell composed of the SHE and a...Ch. 18 - A galvanic cell consists of a silver electrode in...Ch. 18 - Prob. 18.78QPCh. 18 - Calculate the emf of the following concentration...Ch. 18 - Prob. 18.80QPCh. 18 - Suppose you are asked to verify experimentally the...Ch. 18 - Prob. 18.82QPCh. 18 - An aqueous KI solution to which a few drops of...Ch. 18 - A piece of magnesium metal weighing 1.56 g is...Ch. 18 - Prob. 18.85QPCh. 18 - An acidified solution was electrolyzed using...Ch. 18 - In a certain electrolysis experiment involving...Ch. 18 - Consider the oxidation of ammonia:...Ch. 18 - When an aqueous solution containing gold(III) salt...Ch. 18 - In an electrolysis experiment, a student passes...Ch. 18 - People living in cold-climate countries where...Ch. 18 - Given that...Ch. 18 - A galvanic cell with Ecell = 0.30 V can be...Ch. 18 - Shown here is a galvanic cell connected to an...Ch. 18 - Fluorine (F2) is obtained by the electrolysis of...Ch. 18 - A 300-mL solution of NaCl was electrolyzed for...Ch. 18 - Industrially, copper is purified by electrolysis....Ch. 18 - An aqueous solution of a platinum salt is...Ch. 18 - Consider a galvanic cell consisting of a magnesium...Ch. 18 - A current of 6.00 A passes through an electrolytic...Ch. 18 - Prob. 18.101QPCh. 18 - Explain why most useful galvanic cells give...Ch. 18 - The table here shows the standard reduction...Ch. 18 - Consider a concentration cell made of the...Ch. 18 - A silver rod and a SHE are dipped into a saturated...Ch. 18 - Zinc is an amphoteric metal; that is, it reacts...Ch. 18 - Use the data in Table 18.1 to determine whether or...Ch. 18 - The magnitudes (but not the signs) of the standard...Ch. 18 - A galvanic cell is constructed as follows. One...Ch. 18 - Given the standard reduction potential for Au3+ in...Ch. 18 - Prob. 18.111QPCh. 18 - When 25.0 mL of a solution containing both Fe2+...Ch. 18 - Consider the Daniell cell in Figure 18.1. When...Ch. 18 - Use the data in Table 18.1 to show that the...Ch. 18 - Consider two electrolytic cells A and B. Cell A...Ch. 18 - A galvanic cell consists of a Mg electrode in a 1...Ch. 18 - The concentration of sulfuric acid in the...Ch. 18 - Consider a Daniell cell operating under...Ch. 18 - An electrolysis cell was constructed similar to...Ch. 18 - Prob. 18.120QPCh. 18 - Prob. 18.121QPCh. 18 - Prob. 18.122QPCh. 18 - A piece of magnesium ribbon and a copper wire are...Ch. 18 - The zinc-air battery shows much promise for...Ch. 18 - Calculate E for the reactions of mercury with (a)...Ch. 18 - Because all alkali metals react with water, it is...Ch. 18 - A galvanic cell using Mg/Mg2+ and Cu/Cu2+...Ch. 18 - Given the following standard reduction potentials,...Ch. 18 - Compare the pros and cons of a fuel cell, such as...Ch. 18 - Lead storage batteries are rated by ampere hours,...Ch. 18 - Use Equations (17.10) and (18.3) to calculate the...Ch. 18 - A construction company is installing an iron...Ch. 18 - A 9.00 102-mL 0.200 M MgI2 was electrolyzed. As a...Ch. 18 - Based on the following standard reduction...Ch. 18 - Calculate the equilibrium constant for the...Ch. 18 - The nitrite ion (NO2) in soil is oxidized to...Ch. 18 - The diagram here shows an electrolytic cell...Ch. 18 - Fluorine is a highly reactive gas that attacks...Ch. 18 - Show a sketch of a galvanic concentration cell....Ch. 18 - The emf of galvanic cells varies with temperature...Ch. 18 - A concentration cell ceases to operate when the...Ch. 18 - It has been suggested that a car can be powered...Ch. 18 - Estimate how long it would take to electroplate a...Ch. 18 - The potential for a cell based on the standard...
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- Calculate the pH of 0.015 M HCl.arrow_forwardCalculate the pH of 0.450 M KOH.arrow_forwardWhich does NOT describe a mole? A. a unit used to count particles directly, B. Avogadro’s number of molecules of a compound, C. the number of atoms in exactly 12 g of pure C-12, D. the SI unit for the amount of a substancearrow_forward
- 5 What would the complete ionic reaction be if aqueous solutions of potassium sulfate and barium acetate were mixed? ed of Select one: O a 2 K SO4 + Ba2 +2 C₂H3O21 K+SO4 + Ba2+ + 2 C2H3O21 K+SO42 + Ba2 +2 C2H3O2 BaSO4 +2 K+ + 2 C2H3O estion Ob. O c. Od. 2 K SO4 +Ba2 +2 C₂H₂O₂ BaSO4 + K+ + 2 C2H3O BaSO4 + K + 2 C2H301 →Ba² +SO42 +2 KC2H3O s pagearrow_forward(28 pts.) 7. Propose a synthesis for each of the following transformations. You must include the reagents and product(s) for each step to receive full credit. The number of steps is provided. (OC 4) 4 steps 4 steps OH b.arrow_forwardLTS Solid: AT=Te-Ti Trial 1 Trial 2 Trial 3 Average ΔΗ Mass water, g 24.096 23.976 23.975 Moles of solid, mol 0.01763 001767 0101781 Temp. change, °C 2.9°C 11700 2.0°C Heat of reaction, J -292.37J -170.473 -193.26J AH, kJ/mole 16.58K 9.647 kJ 10.85 kr 16.58K59.64701 KJ mol 12.35k Minimum AS, J/mol K 41.582 mol-k Remember: q = mCsAT (m = mass of water, Cs=4.184J/g°C) & qsin =-qrxn & Show your calculations for: AH in J and then in kJ/mole for Trial 1: qa (24.0969)(4.1845/g) (-2.9°C)=-292.37J qsin = qrxn = 292.35 292.37J AH in J = 292.375 0.2923kJ 0.01763m01 =1.65×107 AH in kJ/mol = = 16.58K 0.01763mol mol qrx Minimum AS in J/mol K (Hint: use the average initial temperature of the three trials, con Kelvin.) AS=AHIT (1.65×10(9.64×103) + (1.0 Jimaiarrow_forward
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