Tutored Practice Problem 20.2.4 COUNTS TOWARDS GRADE Use cell potential to calculate an equilibrium constant. Calculate the cell potential and the equilibrium constant for the following reaction at 298 K: Co2(aq) + Pb(s) Co(s) + Pb²+ (aq) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant: Check & Submit Answer Close Problem Show Approach
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- ELECTROCHEMISTRY: Copper was electroplated from a Cu2SO, solution onto an electrode with an active surface area of 3.11 cm2. Determine the thickness (mm) of the deposit if the current is kept constant at 4.45 A for 1.2715 hours. (density of Cu = 8.96 g/cm3, MW of Cu = 63.55 g/mol). (Input values only with 2 decimal places. Do not include the unit.)||| O ELECTROCHEMISTRY Calculating standard reaction free energy from standard... KJ Explanation Check X Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy AG for the following redox reaction. Round your answer to 2 significant digits. 2Zn (s) + N₂ (g) + 4H₂O(1)→ 2Zn²+ (aq) + N₂H₁ (aq) + 40H (aq) S 2. M Smart... ? h Hulu ... Home MacBook Air Netflix G CH3(c... 1/5 C Ⓒ2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | A A@Two Copper strips were used to determine the effect of electrolysis time and immersed in 3.080g of Cu (NO3)2dissolved in 25mL of DI water. The weight of one copper strip act as an anode is taken before the reaction and after the reaction to calculate the change in mass due to different applied current. The current is applied for 5mins for every reptation. Current (A) 0.5 1.0 1.5 2.0 Initial mass of strip (mg) 2941 3390 2.893 2.738 Final mass of strip (mg) 2893 3297 2.738 2.573 Mass change Dm (mg) 48 93 155 165 The theoretical mass of copper deposited on supplying different current: Michael Faraday equation: Q = I x t = nFN Calculate the theoretical mass that should be obtained at each applied current and Compares the theoretical mass (mg) of copper and the actual mass deposited (obtained from the electrolysis, ∆m) by calculating the %error at different times. Briefly discuss the observed results. Is there any trend observed?
- (a) In the electrolysis of aqueous NaCl, how many liters of Cl2(g) (at STP) are generated by a current of 91.2 A for a period of 60.1 min? The unbalanced chemical reaction representing this electrolysis is shown below.NaCl(aq) + H2O(l) Cl2(g) + H2(g) + NaOH(aq)__________ liters of Cl2(g) is generated by this electrolysis.(b) How many moles of NaOH(aq) are formed in the solution in this process? _______moles of NaOH(aq) are formed.日く A apclassroom.collegeboard.org A UPDATES AVAILABLE 29m ago Do you want to install the updates now? CollegeBoard AP'Classroom Unit 9 Progress Check: MCQ 13 14 15 16 23 24 « 0.47 V NO3 K+ Pb. Cu Submit 1.0 M Pb(NO3)2- -1.0 M Cu(NO3)2 The galvanic cell illustrated above was constructed using a salt bridge containing KNO3. A second cell is constructed from identical half-cells but uses NaNO, for the salt bridge. Which of the following best explains whether the initial potential of the second cell will be different from the initial potential of the first cell? A The initial potential of the second cell will be lower than the initial potential of the first cell because Na has a lower molar mass than K has. B The initial potential of the second cell will be higher than the initial potential of the first cell because Na is less electronegative than K is. The initial potential of the second cell will be the same as the first cell because the ions from the salt bridge are not oxidized or…A 50.00 ml. sample of phenol cleaning solution was analyzed by reaction of phenol with Brg 0 The Bry ) was produced by anodic oxidation of Br by application of a 88.934 mA constant current for 10o.36 minutes. Express your answer in mng phenol/ml. sample. Report your answer to 3 sig figs OH OH Br + 3H + 3Br Br 3Br, + Br
- Part A What mass of Cu(s) is electroplated by running 19.0 A of current through a Cu+ (aq) solution for 4.00 h? Express your answer to three significant figures and Include the appropriate units. > View Avallable Hint(s) Value Units SubmitLearning Goal: To learn how to use the Nernst equation. The standard reduction potentials listed in any reference table are only valid at the common reference temperature of 25 °C and standard conditions of 1 M for solutions and 1 atm for gases. To calculate the cell potential at nonstandard conditions, one uses the Nernst equation, E=E 2.303 RT 1 nF -log10 Q where E is the potential in volts. Eo is the standard potential at 25°C in volts. R 8.314 J/(K-mol) is the gas constant, T is the temperature in kelvins. 12 is the number of moles of electrons transferred, F = 96, 500 C/(mol e-) is the Faraday constant, and is the reaction quotient. At the common reference temperture of 298 K. substituting each constant into the equation the result is E = E- Vlog 10 Q 0.0592 V 71Use the References to access important values if needed for this question. When the Pb2+ concentration is 1.37 M, the observed cell potentlal at 298K for an electrochemlcal cell with the following reaction Is 0.678V. What is the Cr+ concentration? 3P62+(aq) + 20r(s)- 3Pb(s) + 2Cr3+ (aq) Answer: M. Submit Answer Retry Entire Group 6 more group attempts remalning11:21 Mon May 3 Done < AA A session.masteringchemistry.comSEE MORE QUESTIONSRecommended textbooks for youChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage LearningOrganic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind…ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEYChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage LearningOrganic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind…ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY