Calculate the standard free-energy change for the reaction at 25 °C. Refer to the list of standard reduction potentials. 2 Au3 + (aq) + 3 Cr(s) = 2 Au(s) + 3 Cr* (aq) AG = kJ * TOOLS x10 10:04 PM 4/20/2022 DELL PrtScr Insert Home End Delete F8 F9 F10 F11 F12 F4 F6 F7 %24 & Backs 6. 7 8.

Calculate the standard free-energy change for the reaction at 25 °C. Refer to the list of standard reduction potentials. 2 Au3 + (aq) + 3 Cr(s) = 2 Au(s) + 3 Cr* (aq) AG = kJ * TOOLS x10 10:04 PM 4/20/2022 DELL PrtScr Insert Home End Delete F8 F9 F10 F11 F12 F4 F6 F7 %24 & Backs 6. 7 8.

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...

See similar textbooks

Similar questions

Given the standard electrode reduction potentials, which reaction will occur spontaneously?
Determine E° for the reaction Al(s) + 3 Ag⁺(aq) → 3 Ag(s) + Al³⁺(aq).
Calculate the K and AG for the following reaction at 25 °C: Mg(s) + Pb2+(aq)=Mg2+(aq) + Pb (s) Note: Reference the Standard reduction potentials at 25 °C and Fundamental constants tables for additional information. Part 1 of 2 Round your answer to 3 significant digits. Кс Part 2 of 2 G Round your answer to 4 significant digits. AG° kJ mol
Consider a galvanic cell at T = 298K. F = 96 485C. At the beginning (t0), [Ca2+] = 0.01M, [H+] = 1M, [HfO2+] = 2M. Consider the half-reactions below: Ca2+(aq) + 2e- → Ca(s) E0red = - 2.76 V HfO2+(aq) + 2H+(aq) + 4e- → Hf(s) + H2O(l) E0red = -1.72 V d. Express and calculate Q (at t0) e. Express and calculate K. f. What value do you expect for Ecell at this point? Why? g. Find Ecell (at t0)
2. In the electrolysis of an aqueous Zn(NO3)2 solution, what reactions occur at the anode and at the cathode, assuming standard conditions? O, + 4H + 4e → 2H;O 6° = 1.23 V 2H,0 + 2e → H2 + 20H E° = -0.83V Zn2 + 2e → Zn ɛ° = -0.76 V NO, + 4H + 3e' → NO + 2H20 E° = 0,96 V ANODE: CATHODE:
Consider a galvanic cell at T = 298K. F = 96 485C. At the beginning (t0), [Ca2+] = 0.01M, [H+] = 1M, [HfO2+] = 2M. Consider the half-reactions below: Ca2+(aq) + 2e- → Ca(s) E0red = - 2.76 V HfO2+(aq) + 2H+(aq) + 4e- → Hf(s) + H2O(l) E0red = -1.72 V a. Find the general reaction, E0cell, and identify the cathode and the anode. Indicate the direction of the flow of electrons (from which solid plate to the other solid plate). b. Write the line notation for this cell. c. Find ΔG0. *d. Express and calculate Q (at t0) e. Express and calculate K. f. What value do you expect for Ecell at this point? Why? g. Find Ecell (at t0) After a certain period of time (t1), the H+ concentration is one-fifth of its initial concentration. *h. Do the RICE and find the concentrations of all species at t1 i. Find the pH at t1 in two…
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 4 significant digits. L (s) + 6H,0 (1) +5Zn²™ (aq) → 21IO, (aq)+ 12H" (aq)+ 5Zn (s) |kJ x10
Based on the sign of the standard cell potential, El classify these reactions as spontaneous or nonspontaneous as written. Assume standard conditions. Refer to the list of standard reduction potentials. Spontaneous as written Ni² (aq) + S² (aq) - Ni(s) + S(s) Answer Bank Al (aq) + 3 Na(s) Al(s) + 3 Na+ (aq) Nonspontaneous as written Pb (aq) + H₂(g)- Pb(s) + 2 H+ (aq)
Hello, im a student it counted my answer wrong can you redo the problem plz. thanks
Consider the following reactions: J + K → K + J (spontaneous) J+LL+J (spontaneous) M + KM+K (non-spontaneous) 1. J 2. J 3. K 4. K 5. L 6. L 7. M 8. M List the numbers for the reducing agents in order of increasing strength (weakest RA in blank 1; strongest RA in blank 4). Blank # 1 Blank # 2 Blank # 3 Blank # 4 N N A/
1. For the reaction: Cus) + 2Ag+ (aq) → 2+ Oxidation half-reaction: Cu(s) → Cuaq) + 2e¯ + Reduction half-reaction: 2Agaq) +2e → 2Ag Answer the following questions using Table 5.4.1: Table 5.4.1. Selected Standard Reduction Potentials at 25 °C Adapted from https://opentextb_c.ca/chemistry/chapter/17-3- Half-Reaction F2)+2 e2F¯(aq) O2(g) + 4H+ (aq) + 4e¯ → 2H₂O) Ag+(aq) + e → Ag(s) → Fe 2+ (aq) Fe³+ (aq) + e 12(1) + 2e™ 21 (24) Cu²+ (aq) + 2e Cu(s) - 2H*(aq) + 2e H₂0) + 2e → Zn(s) Zn² (29) Mg2 (aq) + 2 e→→ MgG) Ca²+ (aq) + 2e →→ Ca(s) a. What is the Eº of the anode half-cell? b. What is the E° for the cathode half-cell? c. Calculate the Eᵒcell for the reaction. d. Is the reaction spontaneous? Cu²+ (aq) + 2Ag(s) standard-reduction-potentials/ E° (V) +2.87 +1.23 +0.80 +0.77 +0.54 +0.34 0.00 -0.76 -2.37 -2.87
Referring to the arrangement in the figure below, calculate the spontaneous at 25 °C. Cadmium anode [Cu²+] [ca²+] Cd²+ = SO²- CdSO4 solution CI™ K+ Salt bridge → Cotton plugs Cu²+ (aq) + Cd (s) x10 Cu(s) + Cd²+ (aq) Round your answer to 1 significant digit. Note: Reference the Standard reduction potentials at 25 °C table for additional information. X Cu²+ [Cu²+] [ca²+] Ś Copper cathode SO² CuSO4 solution ratio at which the following reaction is