Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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- 4 Consider the voltaic cell: Sn(s) | Sn*2(aq) II Fe*3(aq) | Fe*2(aq) a) Write the overall cell reaction. b) Calculate the standard cell potential at 25°C. c) Calculate the change in free-energy of the reaction at 25°C d) What is the maximum work you can obtain from 25.0 g of nickel? e) What is the value of the equilibrium constant of the reaction? f) Which is the stronger oxidizing agent: Sn*2 or Fe*3? Explainarrow_forwardPb(s) Determine which of the following statements about the cell shown are True or False. True The standard cell potential, o, equals 0.93 V. True As the reaction proceeds, the concentration of the silver ions decreases. False Cations move to the lead half-cell. True The mass of the silver electrode is increasing. True The silver half-cell is the cathode. False The cell, as represented by the line notation, is a voltaic cell. True True The lead electrode is the anode. Electrons are spontaneously produced in the silver half-cell. salt bridge Ag(s) Pb+2 So Pb2+2e → Pb(s) AS NO3 E--0.13V Ag + le → Ag(s) E° - +0.80V Pb(s) Pb2+ (1M) || Ag+ (1M) | Ag(s)arrow_forwardA certain metal M forms a soluble sulfate salt MSO4. Suppose the left half cell of a galvanic cell apparatus is filled with a 2.50 M solution of MSO, and the right half cell with a 25.0 mM solution of the same substance. Electrodes made of M are dipped into both solutions and a voltmeter is connected between them. The temperature of the apparatus is held constant at 40.0 °C. left Which electrode will be positive? x10 O right What voltage will the voltmeter show? Assume its positive lead is connected to the positive electrode. necessary, and round it to 2 significant Be sure your answer has a unit symbol, digits.arrow_forward
- Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Mg(s) ∣ Mg2+(aq, 1.74 M) || Cu2+(aq, 0.0053 M) ∣ Cu(s)arrow_forwardA certain metal M forms a soluble sulfate salt M₂SO4. Suppose the left half cell of a galvanic cell apparatus is filled with a 2.00 M solution of M₂ SO4 and the right half cell with a 10.0 mM solution of the same substance. Electrodes made of M are dipped into both solutions and a voltmeter is connected between them. The temperature of the apparatus is held constant at 25.0 °C. left Which electrode will be positive? x10 right X Ś ? What voltage will the voltmeter show? Assume its positive lead is connected to the positive electrode. 0 Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits.arrow_forwardThe chemical reaction that causes iron to corrode in air is given by: 4Fe+3O2→2Fe2O3 in which at 298 K, ΔHorxn = −1684 kJ and ΔSorxn = −543.7 J/K At what temperature Teq do the forward and reverse corrosion reactions occur in equilibrium?arrow_forward
- Consider a voltaic cell in which the reaction is Zn (s) + 2H+ (aq) → Zn2+ (aq) + H2 (g) It is found that the cell voltage is +0.530 V when [Zn2+] = 1.0 M, PH2 = 1.0 atm. What must be the concentration of H+ in the cell? (Use the following information) (Show your work) 2H+ (aq) + 2e- → H2 (g) Eºred = 0.000 V Zn2+ (aq) + 2e- → Zn(s) Eºred = -0.762 Varrow_forwardConsider the following electrochemical cell notation with a cell potential of 1.22 V. Pt(s) ∣ H2(g, 1.0 atm) ∣ H+(aq,1.0M) ∣∣ Au3+(aq,? M) ∣ Au (s)Determine the standard cell potential and if the cell is more spontaneous or less spontaneous at standard conditions.arrow_forwardWhat will be the products of the electrolysis of an 1-M aqueous aluminum chloride (AICI3) solution at 25 °C? (The electrodes themselves are platinum.) (Use the standard electrode potentials table in your online textbook's Appendix to help you answer the question.) No products will be produced. H₂(8) +20H (aq) + Cl₂(g) 4Al(s) + 30₂(g) + 12H*(aq) O 2H₂(g) + 4H₂O(l) + O₂(g) O2Al(s) + 3Cl2(g)arrow_forward
- What is the calculated value of the cell potential at 298 K for an 2+ Cu²+ concentration is 3.83 × 10-4 M and the A1³+ concentration is 1.12 M? Ecell electrochemical cell with the following reaction, when the 2+ 3Cu²+ (aq) + 2Al(s) → 3Cu(s) + 2A1³+ (aq) V The cell reaction as written above spontaneous nonspontaneous for the concentrations given.arrow_forwardThe oxidation of methanol, as described by the equation below, has a ΔG° value of -937.9 kJ/mol. What is the standard cell potential (in V) for a methanol fuel cell? 2 CH3OH (l) + 3 O2 (g) → 2 CO2 (g) + 4 H2O (l)arrow_forwardThe oxidation of methanol, as described by the equation below, has a ΔG° value of -938 kJ/mol. What is the standard cell potential (in V) for a methanol fuel cell? 2 CH3OH (l) + 3 O2 (g) → 2 CO2 (g) + 4 H2O (l)arrow_forward
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