[Review Topics][References]Use the References to access important values if needed for this question.When the Cu²+ concentration is 1.20 M, the observed cell potential at 298 K for an electrochemical cell with thefollowing reaction is 1.141 v. What is the Cr³+ concentration?3+[Cr³+] = [3+3Cu²+ (aq) + 2Cr(s) → 3Cu(s) + 2Cr³+ (aq)Submit AnswerF3$▶ SARFF4%5TMRetry Entire Group 8 more group attempts remainingCengage Learning Cengage Technical SupportDIIF5O60YG HF6&7UF7JOOPrtScn1F8HomeF9K LEndF10PPreviousPgUpF11NextSave and Exit4xPgDnX8:27 PM12/2/202211F121Ins] [Review Topics][References]Use the References to access important values if needed for this question.When the Cu²+ concentration is 1.20 M, the observed cell potential at 298 K for an electrochemical cell with thefollowing reaction is 1.141 v. What is the Cr³+ concentration?3+[Cr³+] = [3+3Cu²+ (aq) + 2Cr(s) → 3Cu(s) + 2Cr³+ (aq)Submit AnswerF3$▶ SARFF4%5TMRetry Entire Group 8 more group attempts remainingCengage Learning Cengage Technical SupportDIIF5O60YG HF6&7UF7JOOPrtScn1F8HomeF9K LEndF10PPreviousPgUpF11NextSave and Exit4xPgDnX8:27 PM12/2/202211F121Ins]

According to the bartleby guidelines for the multiple questions. I can solve only first one…

When the Cu²+ concentration is 1.20 M, the observed cell potential at 298 K for an electrochemical cell with the following reaction is 1.141 v. What is the Cr³+ concentration? 2+ 3+ 3Cu²+ (aq) + 2Cr(s) → 3Cu(s) + 2Cr³+ (aq) [Cr³+] [Review Topics] [References] Use the References to access important values if needed for this question. Submit Answer M Retry Entire Group 8 more group attempts remaining

When the Cu²+ concentration is 1.20 M, the observed cell potential at 298 K for an electrochemical cell with the following reaction is 1.141 v. What is the Cr³+ concentration? 2+ 3+ 3Cu²+ (aq) + 2Cr(s) → 3Cu(s) + 2Cr³+ (aq) [Cr³+] [Review Topics] [References] Use the References to access important values if needed for this question. Submit Answer M Retry Entire Group 8 more group attempts remaining

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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19
A standard galvanic cell is constructed in which a Co2+ | Co half cell acts as the cathode. Which of the following statements are correct? Hint: Refer to a table of standard reduction potentials. (Choose all that apply.) The cathode reaction is Co2+ + 2e -> Co. Co is oxidized at the cathode. The anode compartment could be Fe³+|Fe²+. As the cell runs, anions will migrate from the Co²+ | Co compartment to the other compartment. In the external circuit, electrons flow from the Co²+ | Co compartment to the other compartment.
A student constructs an electrochemical cell with a half-cell composed of a nickel anode in a 0.10 M Ni2+(aq) solution, and another composed of a silver cathode in a 0.10 M Ag+(aq) solution. The Ecell at 20oC (293K) is measured as +1.03 V. Calculate the experimental standard cell potential, Eocell, for the reaction
Use the standard reduction potentials given below to predict if a reaction will occur when Zn metal is put into a 1 M aqueous Ag solution. Ag+ (aq) + e → Ag(s) E red Zn²+ (aq) + 2e¯ → Zn(s) Ee -0.763 V Fred = 0.799 V If a reaction will occur, write a balanced net ionic equation for the reaction. If no reaction will occur, leave all boxes blank. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) + -> +
When [Pb²+] = 1.10 M, the observed cell potential at 298 K for an electrochemical cell with the reaction shown below is 0.683 V. What is the Cr³+ concentration in this cell? 3Pb²+ (aq) + 2Cr(s) [Cr³+] = → 3Pb(s) + 2Cr³+ (aq) mol/L
4. Electrochemical cell potentials can be used to determine equilibrium constants that would be otherwise difficult to determine because concentrations are small. What is K for the following balanced reaction, if E = +0.0218 V? 3Zn+² (aq) + Cr(s) 3Zn(s) + 2Cr³+ (aq) →
Calculate the cell potential, E, for the given reactions at 25.00 "C using the ion concentrations provided. Then, determine if th cells are spontaneous or nonspontaneous as written. Refer to the table of standard reduction potentials (E). Pt(s) + Fe²(aq) = P² (aq) + Fe(s) [Fe²*1 = 0.0064 M E= incorrect -4761 E= Cu(s) + 2 Ag* (aq) = Cu² (aq) + 2 Ag(s) |Cu²+1 = 0.027 M Ag1=0.027 M E [P1²*1 = 0.067 M Co² (aq) + Ti (aq) — Co¹ (aq) + Ti² '(aq) Co²1 = 0.055 M Co= 0.030 M ITP 1 = 0.0070 M T² = 0.0107 M mam V The cell is not spontaneous spontaneous. The cell is spontaneous not spontaneous. incorrect The cell is spontaneous not spontaneoux.
Calculate the cell potential for the reaction as written at 25.00 °C, given that [Cr²+] = 0.768 M and [Fe2+] = 0.0170 M. Use the standard reduction potentials in this table. Cr(s) + Fe²+(aq) Cr² (aq) + Fe(s) E = x10 TOOLS V
A student constructs an electrochemical cell with a half-cell composed of a nickel anode in a 0.10 M Ni2+(aq) solution, and another composed of a silver cathode in a 0.10 M Ag+(aq) solution. The Ecell at 20.0oC is measured as +1.03 V. Calculate the experimental equilibrium constant, K, for the reaction Your answer should have 3 sig figs.
Use standard reduction potentials to calculate the equilibrium constant for the reaction: Pb2+ (aq) + Sn(s) → Pb(s) + Sn'(aq) Pb + (aq) + 2e → Pbs) Erd - -0.126 V Sn+ (ag) + 2e → Sn(s) E° red = -0.140 V Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant at 298 K: AG° for this reaction would be
When [Pb2+] = 1.18 M, the observed cell potential at 298 K for an electrochemical cell with the reaction shown below is 0.687 V. What is the Cr3+ concentration in this cell?3Pb2+(aq) + 2Cr(s) 3Pb(s) + 2Cr3+(aq)[Cr3+] = mol/L
Calculate the cell potential for the reaction as written at 25.00 °C, given that [Cr2+]=0.876 M and [Ni2+]=0.0130 M Cr(s)+Ni2+(aq)↽−−⇀ Cr2+(aq)+Ni(s)