Determine the K, for Cug(PO)>(s) Part A An electrochemical cell is set up in the following configuration: 1. The anode compartment consists of a Copper electrode and a solution containing copper ions from a saturated solution of Cuy(POJ(s). Where: Cu(PO2(0)> 3 Cu?*(aq) + 2 PO (aq) 2. The cathode compartment consists of a Copper electrode and a solution containing 1.00 M Cu"(aq) The measured cell potential for this electrochemical cell is 0.272 V. Use this information to determine the value of K for Cuy(PO,(0). Express your answer for K to two significant figures Submit Reavest Anwer

Determine the K, for Cug(PO)>(s) Part A An electrochemical cell is set up in the following configuration: 1. The anode compartment consists of a Copper electrode and a solution containing copper ions from a saturated solution of Cuy(POJ(s). Where: Cu(PO2(0)> 3 Cu?*(aq) + 2 PO (aq) 2. The cathode compartment consists of a Copper electrode and a solution containing 1.00 M Cu"(aq) The measured cell potential for this electrochemical cell is 0.272 V. Use this information to determine the value of K for Cuy(PO,(0). Express your answer for K to two significant figures Submit Reavest Anwer

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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A certain metal è forms a soluble sulfate salt ₂(so). Suppose the left half cell of a galvanic cell apparatus is filled with a 5.00 M solution of M₂(SO4)3 and the right half cell with a 250. 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 35.0 °C. Which electrode will be positive? O left Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. O right What voltage will the voltmeter show? Assume its positive lead is connected to the positive electrode. 0 x10 X
A voltaic electrochemical cell is constructed using the following reaction. The half-cell components are separated by a salt bridge. Br2(1) + Mn(s) 2Br"(aq) + Mn2+(aq) Write the reactions that take place at the anode and at the cathode, the direction in which the electrons migrate in the external circuit, and the direction the anions in the salt bridge migrate. Use smallest possible integer coefficients. If a box is not needed, leave it blank. Enter the reaction that takes place at the anode. Include state symbols: Enter the reaction that takes place at the cathode. Include state symbols: In the external circuit, electrons migrate the Mn electrode the Br2 electrode. Anions migrate the salt bridge the Br2 compartment.
Part A If a voltaic cell is created between a Am"/Am electrode and a Fe*/Fe electrode, what species is being oxidized? O Am"(ag) O Fe(s) O Fe"(ag) O Am(s)
Standard Electrode Potentials at 25 °C Reduction Half-Reaction O Cu (aq) O H,Ozlaq) O Br O 10₂ (aq) Fyl) +20 H₂O₂(aq) + 2 H(aq) +2e" PbOg(s) +4 H(aq) +50, (aq) + 2 e Mn0 (aq) +4 H(aq) + 3 e MnO, (aq) +8H(aq) + 5 e Au³(aq) + 3 e PbOy(s) +4 H(aq) + 2e¯ C+20 00, (aq) +14 H(aq) + 6 e 00+ 4H*(aq) + 4 MnO₂ (s) +4 H(aq) +2e¯ 10₂(aq) + 6H(aq) +5e Big(0+20 VO₂ (aq) + 2 H(aq) + e¯ NO₂ (aq) + 4H(aq) + 3 e CO₂(0)+ Ag (ag)+e Fe(aq) + e 0)+2 H(aq) +2 e Mn0, (aq) + e (8) +26 Cu (aq) + e -2 (aq) -2 H₂O(0) Which of the following is the strongest oxidizing agent? -PbSO4(s) + 2 H₂O(0) →→MnO₂ (s) + 2 H₂O(0) Mn²(aq) + 4H₂O(1) - Au(s) ·Pb²+ (aq) + 2 H₂O(0) - 2 Cr (aq) 2 Cr³+ (aq) + 7 H₂O(1) → 2 H₂O( -2(aq) -Cu(s) Mn²+ (aq) + 2 H₂O(0) ₂(aq) + 3 H₂0(0) -2 Br (aq) - Vo²+ (aq) + H₂O( -NO(g) + 2 H₂O(1) — CIO; (aq) -Ag(s) -Fe²+ (aq) -) HyOz(ag) MnO₂ (aq) 1.00 0.96 0.95 0.80 0.77 0.70 0.56 0.54 0.52 E° (V) 2.87 1.78 1.69 1.68 1.51 1.50 1.46 1.36 1.33 1.23 1.21 1.20 1.09
For the galvanic cell: Zn(s) + 2Tl+(aq) 2Tl(s) + Zn2+(aq) Eocell = 0.42 V The standard reduction potential for the half cell Zn2+(aq) + 2e– Zn(s) is Eored = –0.76 V What is the standard reduction potential for Tl+(aq) + e– Tl(s) Eored = ? V a. +0.17 V b. –0.17 V c. –0.34 V d. +0.34 V
Calculate AG for the following cell reaction: Tl(s) | Tl+ (aq) || Ni²+ (aq) | Ni(s) From AG, determine the standard potential for the half-reaction Tl+ (aq) + e → Tl(s) AG; for Tl+ (aq) is -32.4 kJ/mol. 2+ AG; for Ni²+ (aq) is -45.60 kJ/mol. Standard Electrode (Reduction) Potentials in Aqueous Solution at 25°C Cathode (Reduction) Half-Reaction Ni²+ (aq) + 2e Ni(s) AG = J Standard Potential, E° (V) -0.23 Standard reduction potential for the half-reaction = V
A voltaic cell is constructed in which the following cell reaction occurs. The half-cell compartments are connected by a salt bridge. Pb2+(aq) + Mn(s) Pb(s) + Mn2+(aq) The anode reaction is: The cathode reaction is: + + In the external circuit, electrons migrate e the Mn|Mn2+ electrode e the Pb|Pb2+ electrode. In the salt bridge, anions migrate e the Pb|Pb²+ compartment e the Mn|Mn2+ compartment. +
A non-standard state galvanic cell is constructed at 25.00°C as described here. The Fe(s) anode is immersed in a 0.040 M Fe(NO3)2 solution. The Cu(s) cathode is immersed in a 0.0060 M Cu(NO3)2. The circuit is completed with a salt bridge containing 1.0 M KNO3. The standard Fe/Fe2+ reduction potential is –0.44 V. The standard Cu/Cu2+ reduction potential is +0.34 V. Calculate the non-standard-state cell potential for this galvanic cell and determine if the reaction described is spontaneous under these conditions.
Enter electrons as e A voltaic cell is constructed in which the anode is a Fe2+|Fe3+ half cell and the cathode is a F|F, half cell. The half-cell compartments are connected by a salt bridge. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) The anode reaction is: The cathode reaction is: The net cell reaction is: +. In the external circuit, electrons migrate the Fe2+|Fe3+ electrode the F|F, electrode. from to In the salt bridge, anions migrate the F|F, compartment 3- the Fe2+|Fe+ compartment. +. +. 1
Suppose the following reaction happening at 25°C Sn(s) + CuSO4(aq) SNSO4(aq) (reaction in equilibrium) Cu(s) + <----- a) Write the left (Anode) and right (Cathode) reactions. b) Calculate the standard cell potential E°Cell· c) Calculate the equilibrium constant “K" of the reaction using the standard potential data table. TABLE 17.1 Standard Reduction Potentials at 25°C (298 K) for Many Common Half-Reactions Half-Reaction e (V) Half-Reaction e° (V) F + 2e 2F Ag* +e - Ag" Co +e →Cơ H,O, + 2H + 2e 2H,0 Ce +e → Ce* PbO, + 4H + so + 2e PbSO, + 2H,0 MnO, + 4H* + 3e MnO, + 2H,O 2e + 2H + IO, 10, + H,0 MnO, + 8H + Se" → Mn* + 4H,0 Au + 3e -→ Au PbO, + 4H + 2e Pb* + 2H,O Ca, + 2e" → 2CI" Cr0,- + 14H + 6e" → 2Cr“ + 7H,0 O, + 4H + 4e 2H,O MnO, + 4H + 2e Mn + 2H,O 10, + 6H + Se → I, + 3H,0 Br, + 2e 2Br -2H +e VO + H,O 2.87 1.99 O, + 2H,0 + 4c → 40H Cu + 2e Cu Hg,Cl, + 2e -→ 2Hg + 2CI AgCI +e Ag + CI so- + 4H + 2e → H,SO, + H,O Cu* + e - Cu* 2H + 2e H; Fe + 3e Fe Pb* + 2e" -→ Pb Sn Ni* + 2e Ni…
Consider this cell diagram for an electrochemical cell: Pt(s) | H2(g) | H*(aq) || Cu*(aq) | Cu(s) What is the overall balanced reaction for this redox reaction? O 2H (aq) + 2Cu(s) H2(g) + 2Cu (aq). O H2(g) + 2Cu'(aq) → 2H*(aq) + 2Cu(s) O H2(g) + 2Cu(s)H'(aq) + 2Cu'(aq) O H2(g) + Cu (aq) H'(aq) + Cu(s)
5. A more complex example where other atoms are involved. Balance the following reaction in basic solution. r (aq) + MnO4 (aq) MnO, (s)+ BrO;" (aq) TABLE 19.1 Standard Electrode Potentials at 25 °C Reduction Half-Reaction E'(V) F + 20 H,0,(aq) + 2 H(aq)+2 e 2F(aq) 2.87 Stronger oxidizing agent Weaker 2 H,0 - PBSO (s) +2 H,0) -Mn0(s)+ 2 H,0) Mn (aq) 4 H,O) - Auts) 1.78 reducing agent PO,(s) + 4 H"(ag) + S0,2-(aq) + 2 e 1.69 Mno, (aq)+ 4 H'(aq) 3 e Mno, (aa) + 8 H (aq)+5 e Au (aq)+3e PbO,(s)+ 4 H(aa) + 2 e Cl,(g) + 2 e" 1.68 1.51 1.50 1.46 - P (ag) + 2 HO - 2a(aq) 1.36 1.33 Cr0, (aq) + 14 H'(ag) + 6 e 0+ 4 H (aq) + 4 e MnO(s)+4 H'(aq) +2 e 10, (aq) 6 H'(aq) + 5e Br+2e vo, (aq) + 2 H'(aq) + e NO, (aq) + 4 H°(aq) + 3e CIO+e 2 C"(aq) + 7 H,On - 2 H,O1) 1.23 Mn (aq) + 2 HyOV) 121 ulae) + 3 H,0() 2 Br (ag) - vo"(aq) +H,00 - NO + 2 H,O0 - CIO, (aa) - Agis) 1.20 1.09 1.00 0.96 0.95 Ag"(aa) + e 0.80 Fe (aq) + O+2 H'(aq)+2e - Fe*(aq) 0.77 - H,O,(ag) 0.70 Mn0, Taa) + e Mn0 (aa) 0.56 8) + 2 e…