CHEM: ATOM FIRST V. 1 W/ACCESS >C<
18th Edition
ISBN: 9781307286205
Author: Burdge
Publisher: Mcgraw-Hill/Create
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Chapter 18, Problem 18.107QP
Interpretation Introduction
Interpretation:
The decomposition of hydrogen peroxide at
Concept Introduction:
The standard electrode potential
The relation between Gibbs free energy and cell potential: The amount of energy in a system that can be converted into useful energy is defined as free energy in
Free energy and the cell potential is related by the given equation.
Where,
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CHEM: ATOM FIRST V. 1 W/ACCESS >C<
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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- The standard potential, E, for the reaction of Zn(s) and Cl2(g) is +2.12 V. What is the standard free energy change, rG, for the reaction?arrow_forwardCalcium metal can be obtained by the direct electrolysis of molten CaCl2, at a voltage of 3.2 V. (a) How many joules of electrical energy are required to obtain 12.0 1b of calcium? (b) What is the cost of the electrical energy obtained in (a) if electrical energy is sold at the rate of nine cents per kilowatt hour?arrow_forwardActually, the carbon in CO2(g) is thermodynamically unstable with respect to the carbon in calcium carbonate(limestone). Verify this by determining the standardGibbs free energy change for the reaction of lime,CaO(s), with CO2(g) to make CaCO3(s).arrow_forward
- Calculate the standard cell potential of the cell corresponding to the oxidation of oxalic acid, H2C2O4, by permanganate ion. MnO4. 5H2C2O4(aq)+2MnO4(aq)+6H+(aq)10CO2(g)+2Mn2+(aq)+8H2O(l) See Appendix C for free energies of formation: Gf for H2C2O4(aq) is 698 kJ.arrow_forwardHydrazine, N2H4, can be used as the reducing agent in a fuel cell. N2H4(aq) + O2(aq) N2(g) + 2 H2O () (a) If rG for the reaction is 598 kJ, calculate the valueof E expected for the reaction. (b) Suppose the equation is written with all coefficients doubled. Determine rG and E for this new reaction.arrow_forwardCalculate G for the following reactions and state whether each reaction is spontaneous under standard conditions at 298 K. (a) 2Na(s) + H2SO4() Na2SO4(s) + H2(g) (b) Cu(s) + H2SO4() CuSO4(s) + H2(g)arrow_forward
- Given the following standard free energies at 25°C for the following reactions: N2O5(g)2NO(g)+32O2(g)G=59.2kJNO(g)+12O2(g)NO2(g)G=35.6kJ Calculate G° at 25°C for the following reaction: 2NO2(g)+12O2(g)N2O5(g)arrow_forwardCalculate G at 355 K for each of the reactions in Question 17. State whether the reactions are spontaneous.arrow_forwardConsider the following cell reaction at 25C. 2Cr(s)+3Fe2+(aq)2Cr3+(aq)+3Fe(s) Calculate the standard cell potential of this cell from the standard electrode potentials, and from this obtain G for the cell reaction. Use data in Appendix C to calculate H; note that Cr(H2O)63+(aq) equals Cr3+(aq). Use these values of H and G to obtain S for the cell reaction.arrow_forward
- For each of the reactions, calculate E from the table of standard potentials, and state whether the reaction is spontaneous as written or spontaneous in the reverse direction under standard conditions. (a) Zn(s)+Fe2+(aq)Zn2+(aq)+Fe(s) (b) AgCl(s)+Fe2+(aq)Ag(s)+Fe3+(aq)+Cl(aq) (c) Br2(l)+2Cl(aq)Cl2(g)+2Br(aq)arrow_forwardThe 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_forward
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