Answered: Consider the following problem:…

Consider the following problem: Consider a cell reaction at 25°C where n=2. Fill in the following table. AG° E° K (15) ( 17) 19 KJ (14) ( 16 ) ( 18 ) 0.035 V ( 19 ) 0.095

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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An aqueous FeF₂ solution is electrolyzed under 1 bar pressure using platinum electrodes. (a) Write the half-reactions predicted to occur at the anode and cathode, based on the standard cell potentials given below. Half-reaction at anode: Half-reaction at cathode: + + Standard Reduction Potentials (Volts) at 25 °C 2 F (aq) F₂(g) +2 e 2.870 O₂(g) + 4 H3O*(aq) + 4 e¯ →→ 6 H₂O(l) 1.229 2 H₂O(1) +2 eH₂(g) + 2 OH(aq) -0.828 Fe²+ (aq) + 2 e Fe(s) + (b) What is the expected decomposition potential? -0.440 +
Enter electrons as e". Use smallest possible integer coefficients for ALL reactions. If a box is not needed, leave it blank. A voltaic cell is constructed in which the following cell reaction occurs. The half-cell compartments are connected by a salt bridge. 3Br2(1) + 2Cr(s) – 6B1°(aq) + 2Cr*(aq) The anode reaction is: + The cathode reaction is: In the external circuit, electrons migrate v the Cr|Cr* electrode the Br|Br2 electrode. In the salt bridge, anions migrate v the Cr|Cr** compartment v the Br|Br2 compartment.
Enter electrons as e-. Use smallest possible integer coefficients for ALL reactions. If a box is not needed, leave it blank. A voltaic cell is constructed in which the following cell reaction occurs. The half-cell compartments are connected by a salt bridge.3Br2(l) + 2Al(s) ----> 6Br-(aq) + 2Al3+(aq)The anode reaction is: + + The cathode reaction is: + + In the external circuit, electrons migrate _(from or to?)__ the Al | Al3+ electrode _(from or to?) the Br- | Br2 electrode.In the salt bridge, anions migrate _(from or to?) the Br- | Br2 compartment _(from or to?) the Al | Al3+ compartment.
A voltaic cell is constructed in which the anode is a Pb | Pb²+ half cell and the cathode is a l| 12 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 In the salt bridge, anions migrate + + Enter electrons as e + the 1₂ electrode the 1₂ compartment [ the Pb | Pb²+ electrode. the Pb | Pb2+ compartment.
10.)
Based on the sign of the standard cell potential, Eel, classify these reactions as spontaneous or nonspontaneous as written. Assume standard conditions. Refer to the list of standard reduction potentials. Spontaneous as written Nonspontaneous as written Answer Bank Pb2*(aq) + H2(g) - Pb(s) + 2 H*(aq) Ni?*(aq) + s? (aq) Ni(s)+S(s) Al3+(aq) + 3 Na(s) → Al(s) + 3 Na*(aq)
The cell notation of a voltaic cell is: Zn(s) | Zn2+(aq; 0.02M) || Zn2+(aq; 1.0 M) | Zn (s) Draw a diagram of the cell and each half-reaction. Label the anode, cathode, and each relevant reaction. What is Eocell at equilibrium? Why? What is the expected Ecell at T = 273K? Given this Ecell, will the Q of this cell increase or decrease to reach equilibrium?
Consider the same diagram of a galvanic cell as in previous question, conventional current anode X X+ (aq) (C) 0.76 V (D) 0.91 V A e flow Salt bridge Y+ (aq) cathode where the half-cells are Ag|AgNO3(aq) and Ni|Ni(NO3)2(aq). Given the following electrode potentials: Ag (aq) + e-> Ag(s); E° = 0.80 V Ni²+ (aq) + 2e --> Ni(s): E = -0.23 V What is the Ecell at 25°C when the electrolyte concentrations are [Ag*] = 1.3 x 10-5 M and [Ni²+] = 0.10 M. (A) 1.15 V (B) 1.30 V
OH A The transformation above can be performed with some combination of the reagents listed below. Give the necessary reagents in the correct order for each transformation, as a string of letters (without spaces or punctuation, such as "EBF"). If there is more than one correct solution, provide just one answer. Br2 D 1) xs NaNH2; 2) H2O G HBr, ROOR Reagent(s): 2 B TsCl, pyridine E conc. H₂SO4, heat H Br t-BuOK C NaOMe F HBr 1 H2, Lindlar's cat.
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…
The following question refers to the following system: 3Ag(s) + NO3 (aq) + 4H*(aq) → 3Ag*(aq) + NO(g) + 2H2O() Ag → Ag*(aq) + e- NO3 (aq) + 4H*(aq) + 3e→ NO(g) + 2H20(1) Anode reaction: E° = -0.7990 V Cathode reaction: ɛ° = 0.9637 V Determine the standard cell potential. a. 0.5876 V b. 2.0921 V с. 3.5254 V d. 0.1647 V е. —1.7627 V
Please give the line notation for each cell. Use a small L Or a capital i for the line separator. Give the Eo (standard cell potential) of the following equations. Assume at standard conditions. Show work, which reaction you reverse and the total voltage answer. Cr3+(aq) + Cl2(g) ⇐> Cr2O72- (aq) + Cl- (aq) Cu2+ (aq) + Mg(s) ⇐> Mg2+(aq) + Cu(s)