Chemistry: Atoms First
3rd Edition
ISBN: 9781259638138
Author: Julia Burdge, Jason Overby Professor
Publisher: McGraw-Hill Education
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Chapter 18, Problem 18.59QP
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Chemistry: Atoms First
Ch. 18.1 - Permanganate ion and iodide ion react in basic...Ch. 18.1 - Use the half-reaction method to balance the...Ch. 18.1 - Use the half-reaction method to balance the...Ch. 18.1 - Prob. 18.1.1SRCh. 18.1 - MnO4 and C2O42 react in basic solution to form...Ch. 18.3 - A galvanic cell consists of an Mg electrode in a...Ch. 18.3 - Determine the overall cell reaction and Ecell (at...Ch. 18.3 - A galvanic cell with Ecell = 0.30 V can be...Ch. 18 - Balance the following redox equations by the...Ch. 18 - Balance the following redox equations by the...
Ch. 18 - In the first scene of the animation, when a zinc...Ch. 18 - What causes the change in the potential of the...Ch. 18 - Why does the color of the blue solution in the...Ch. 18 - Prob. 18.4VCCh. 18 - Define the following terms: anode, cathode, cell...Ch. 18 - Prob. 18.4QPCh. 18 - Prob. 18.5QPCh. 18 - What is a cell diagram? Write the cell diagram for...Ch. 18 - What is the difference between the half-reactions...Ch. 18 - Discuss the spontaneity of an electrochemical...Ch. 18 - Prob. 18.9QPCh. 18 - Prob. 18.10QPCh. 18 - Calculate the standard emf of a cell that uses...Ch. 18 - Prob. 18.12QPCh. 18 - Prob. 18.13QPCh. 18 - Consider the following half-reactions....Ch. 18 - Predict whether NO3 ions will oxidize Mn2+ to MnO4...Ch. 18 - Prob. 18.16QPCh. 18 - Prob. 18.17QPCh. 18 - Prob. 18.18QPCh. 18 - Prob. 18.19QPCh. 18 - Use the information m Table 2.1, and calculate the...Ch. 18 - Prob. 18.21QPCh. 18 - Prob. 18.22QPCh. 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 - Prob. 18.26QPCh. 18 - Balance (in acidic medium) the equation for the...Ch. 18 - Prob. 18.28QPCh. 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 - What is the emf of a cell consisting of a Pb2+/Pb...Ch. 18 - Prob. 18.35QPCh. 18 - Calculate the emf of the following concentration...Ch. 18 - What is a battery? Describe several types of...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 - What is the difference between a galvanic cell...Ch. 18 - Prob. 18.43QPCh. 18 - Calculate the number of grams of copper metal that...Ch. 18 - Prob. 18.45QPCh. 18 - Consider the electrolysis of molten barium...Ch. 18 - Prob. 18.47QPCh. 18 - Prob. 18.48QPCh. 18 - Prob. 18.49QPCh. 18 - How many faradays of electricity are required to...Ch. 18 - Calculate the amounts of Cu and Br2 produced in...Ch. 18 - Prob. 18.52QPCh. 18 - Prob. 18.53QPCh. 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 - Prob. 18.60QPCh. 18 - Prob. 18.61QPCh. 18 - Prob. 18.62QPCh. 18 - Tarnished silver contains Ag2S. The tarnish can be...Ch. 18 - Prob. 18.64QPCh. 18 - For each of the following redox reactions, (i)...Ch. 18 - Prob. 18.66QPCh. 18 - Prob. 18.67QPCh. 18 - Prob. 18.68QPCh. 18 - Prob. 18.69QPCh. 18 - Prob. 18.70QPCh. 18 - Prob. 18.71QPCh. 18 - Prob. 18.72QPCh. 18 - Prob. 18.73QPCh. 18 - Prob. 18.74QPCh. 18 - A galvanic cell consists of a silver electrode in...Ch. 18 - Explain why chlorine gas can be prepared by...Ch. 18 - Prob. 18.77QPCh. 18 - Prob. 18.78QPCh. 18 - Prob. 18.79QPCh. 18 - Prob. 18.80QPCh. 18 - Prob. 18.81QPCh. 18 - Prob. 18.82QPCh. 18 - An acidified solution was electrolyzed using...Ch. 18 - Prob. 18.84QPCh. 18 - Consider the oxidation of ammonia....Ch. 18 - Prob. 18.86QPCh. 18 - Prob. 18.87QPCh. 18 - Prob. 18.88QPCh. 18 - Prob. 18.89QPCh. 18 - Prob. 18.90QPCh. 18 - Prob. 18.91QPCh. 18 - Prob. 18.92QPCh. 18 - An aqueous solution of a platinum salt is...Ch. 18 - Prob. 18.94QPCh. 18 - Prob. 18.95QPCh. 18 - Prob. 18.96QPCh. 18 - Prob. 18.97QPCh. 18 - A silver rod and a SHE are dipped into a saturated...Ch. 18 - Prob. 18.99QPCh. 18 - Prob. 18.100QPCh. 18 - The magnitudes (but not the signs) of the standard...Ch. 18 - Prob. 18.102QPCh. 18 - Given the standard reduction potential for Au3+ in...Ch. 18 - Prob. 18.104QPCh. 18 - Prob. 18.105QPCh. 18 - Prob. 18.106QPCh. 18 - Prob. 18.107QPCh. 18 - Prob. 18.108QPCh. 18 - Prob. 18.109QPCh. 18 - Prob. 18.110QPCh. 18 - Prob. 18.111QPCh. 18 - In recent years there has been much interest in...Ch. 18 - Prob. 18.113QPCh. 18 - Prob. 18.114QPCh. 18 - Prob. 18.115QPCh. 18 - Prob. 18.116QPCh. 18 - Prob. 18.117QPCh. 18 - A galvanic cell using Mg/Mg2+ and Cu/Cu2+...Ch. 18 - Prob. 18.119QPCh. 18 - Prob. 18.120QPCh. 18 - Lead storage batteries arc rated by ampere-hours,...Ch. 18 - Use Equations 14.10 and 18.3 to calculate the emf...Ch. 18 - Prob. 18.123QPCh. 18 - A 9.00 102 mL amount of 0.200 M MgI2 solution was...Ch. 18 - Prob. 18.125QPCh. 18 - Which of the components of dental amalgam...Ch. 18 - Calculate the equilibrium constant for the...Ch. 18 - Prob. 18.128QPCh. 18 - Prob. 18.129QPCh. 18 - Prob. 18.130QPCh. 18 - Prob. 18.131QP
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- An electrode is prepared from liquid mercury in contact with a saturated solution of mercury(I) chloride, Hg2Cl, containing 1.00 M Cl . The cell potential of the voltaic cell constructed by connecting this electrode as the cathode to the standard hydrogen half-cell as the anode is 0.268 V. What is the solubility product of mercury(I) chloride?arrow_forwardAn aqueous solution of an unknown salt of vanadium is electrolyzed by a current of 2.50 amps for 1.90 hours. The electroplating is carried out with an efficiency of 95.0%, resulting in a deposit of 2.850 g of vanadium. a How many faradays are required to deposit the vanadium? b What is the charge on the vanadium ions (based on your calculations)?arrow_forwardAn electrode is prepared by dipping a silver strip into a solution saturated with silver thiocyanate, AgSCN, and containing 0.10 M SCN . The cell potential of the voltaic cell constructed by connecting this electrode as the cathode to the standard hydrogen half-cell as the anode is 0.45 V. What is the solubility product of silver thiocyanate?arrow_forward
- (a) Write equations for the half-reactions that occur at the cathode and the anode when an aqueous solution of KCl is electrolyzed. Which chemical species is oxidized, and which chemical species is reduced in this reaction? (b) Predict the products formed when an aqueous solution of CsI is electrolyzed.arrow_forwardAn aqueous solution of an unknown salt of gold is electrolyzed by a current of 2.75 amps for 3.39 hours. The electroplating is carried out with an efficiency of 93.0%, resulting in a deposit of 21.221 g of gold. a How many faradays are required to deposit the gold? b What is the charge on the gold ions (based on your calculations)?arrow_forwardIn the electrolysis of a solution containing Ag+(aq), metallic Ag(s) deposits on the cathode. Using a current of 1.12 A for 2.40 hours, what mass of silver forms?arrow_forward
- A galvanic cell is based on the following half-reactions: In this cell, the copper compartment contains a copper electrode and [Cu2+] = 1.00 M, and the vanadium compartment contains a vanadium electrode and V2+ at an unknown concentration. The compartment containing the vanadium (1.00 L of solution) was titrated with 0.0800 M H2EDTA2, resulting in the reaction H2EDTA2(aq)+V2+(aq)VEDTA2(aq)+2H+(aq)K=? The potential of the cell was monitored to determine the stoichiometric point for the process, which occurred at a volume of 500.0 mL H2EDTA2 solution added. At the stoichiometric point, was observed to be 1 .98 V. The solution was buffered at a pH of 10.00. a. Calculate before the titration was carried out. b. Calculate the value of the equilibrium constant, K, for the titration reaction. c. Calculate at the halfway point in the titration.arrow_forwardChlorine, Cl2, is produced commercially by the electrolysis of aqueous sodium chloride. The anode reaction is 2Cl(aq)Cl2(g)+2e How long will it take to produce 2.00 kg of chlorine if the current is 5.00 102 A?arrow_forwardIn the electrolysis of a solution containing Ni2+(aq), metallic Ni(s) deposits on the cathode. Using a current of 0.150 A for 12.2 minutes, what mass of nickel will form?arrow_forward
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