Dissolution reactions of gold (Au) in 1M HNO3 and 1M aqua regia (1M HNO3 + 1M HCl) are provided below 1)What is the E°cell and Keq for the dissolution of gold in 1M HNO3 under standard conditions. (calculate) b) Calculate E°cell and Keq for the dissolution of gold in aqua regia under standard conditions.

Dissolution reactions of gold (Au) in 1M HNO3 and 1M aqua regia (1M HNO3 + 1M HCl) are provided below 1)What is the E°cell and Keq for the dissolution of gold in 1M HNO3 under standard conditions. (calculate) b) Calculate E°cell and Keq for the dissolution of gold in aqua regia under standard conditions.

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter21: The Chemistry Of The Main Group Elements

Section: Chapter Questions

Problem 108SCQ

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R = 8.314 mol·K F = 96,485 mot AG = AG° + RT · In(Q) ΔΕΔΕ-).In(O) Half Reaction (Note: All given as reduction) E° (V) 02 (g) + 4 H*(aq) + 4 e¯ → 2 H20 (1) 1.229 2 z" (aq) Z2 (s) + 2 e 3+ (aq) + 3 е 0.426 A (s) 0.292 2 H20 (1) + 2 e G2+ (aq) + 2 e H2 (g) + 2 OH (aq) - 0.828 G (s) - 1.245 > M2+ (aq) + 2 e - 1.893 → M (s) A student constructs a voltaic electrochemical cell with two metal electrodes [metal G and metal A] in their respective aqueous nitrate solutions [G(NO3)2 and A(NO3)3]. Use this information, as well as the reduction potentials in the table above to complete each statement below. Consider the same cell from the above prompt. Calculate AG° in kJ/mol for this galvanic cell. Report your answer with 4 significant figures. You do not need to report units with your answer. If your value is negative, make sure to include a "-" symbol.
Which of the folowing is the correct line notation for the following redox raaction? Fe (aq) + Cu (s)Fe (aq) + Cu* (aq) Cu (e)Fe (e Cu" (aq) | Cu (s) |Fe (eq), Fe+ (aq)| Pt (s) Pre) |Fe®*® (aq. Fe’" (aq | Cu' (safNப (a] Pt (s) Fe (aq), Fe (aq) || Cu (s)Cu (aq) (aq) || Cu (6)|Cu" (aq) cu" (eq|Cu (el | Fe (ag), Fe (aq)| P() Pt (s)Fe (aq), Fe* (aq) || Cu (s)| Cu* (aq) Cu (6) Cu" (eq) ||Fe* (aq), Fe+ (ag) | Pt (9) Cu (s)| Cu (aq) || Fe (aq), Fe (aq)| Pt (s) Pt (s) | Fe* (aq). Fe (aq) || Cu" (ag) |Cu (s)
The following two reactions involve proton transfer. In each reaction, identify the acid and the base. Identify the conjugate base of the acid, and the conjugate acid of the base. Draw Lewis electron dot diagrams for each molecule, and describe the rear- rangement of bonding in the reaction as nonbonding electron pairs become cova- lently shared pairs and vice versa. (a) H¿O(€) + NH (aq) → H;0* (aq) + NH3(aq) (b) CH;CH;OH(aq) + NH7 (aq) → CH;CH;O¯(aq) + NH3(aq)
R = 8.314 mol·K F = 96,485 mol AG° + RT · In(Q) AE° () · In(Q) AG ΔΕ %3D Half Reaction (Note: All given as reduction) E° (V) 02 (g) + 4 H*(aq) + 4 e → 2 H20 (I0) 1.229 Z2 (s) + 2 e - → 2Z (aq) 0.426 (aq) + 3 e A (s) 0.292 2 H20 (1) + 2 e G2+ (aq) + 2 e M2+ (aq) + 2 e Н2 (в) + 2 ОН" (aq) - 0.828 G (s) - 1.245 M (s) - 1.893 Using a U-tube, a student sets up a non-spontaneous electrochemical cell with a battery connected to two carbon electrodes that are submerged in 1 M MZ2 (aq) solution (M is a metal and Z is an anion composed of the newly discovered element Z). Use the reference information given in the table above to answer the following three questions. Question 10 Oxidation will occur at the while reduction will occur at the Possible answers are "anode" and "cathode".
AG = AG° + RT · In(Q) ΔΕ ΔΕ-). In(Q) Half Reaction (Note: All given as reduction) E° (V) 02 (g) + 4 H*(aq) + 4 e¯ → 2 H20 (I) 1.229 |Z2 (s) + 2 e 2z (aq) 0.426 3+ |A°™ (aq) + 3 e A (s) 0.292 2 H20 (1) + 2 e H2 (g) + 2 OH¯ (aq) - 0.828 > 2+ G (aq) + 2 e¯ → G (s) - 1.245 M2+ (aq) + 2 e → M (s) - 1.893 A student constructs a voltaic electrochemical cell with two metal electrodes [metal G and metal A] in their respective aqueous nitrate solutions [G(NO3)2 and A(NO3)3]. Use this information, as well as the reduction potentials in the table above to complete each statement below. The metal electrode A is... o not changing in mass. o increasing in mass. o decreasing in mass. Question 4 The metal solution A(NO3)3 is... o increasing in concentration. o not changing in concentration. o decreasing in concentration.
Be sure to answer all parts. Consider the following balanced redox reaction (do not include state of matter in your answers): 2CrO₂ (aq) + 2H₂O()+6C10 (aq) → 2CrO42 (aq) + 3Cl₂(g) + 40H (aq) (a) Which species is being oxidized? (b) Which species is being reduced? (c) Which species is the oxidizing agent? (d) Which species is the reducing agent? (e) From which species to which does electron transfer occur? Electrons transfer from to
14.58 Complete and balance the following oxidation-reduction reactions, assuming they occur in acidic solution. (a) C20; (aq)+MnO,(aq)' CO(g)+Mn²*(aq) (b) CIO3(aq)+CI¯(aq) Cl2(aq) (c) S20;(aq)+I½(a) so; (ag)+I¬(aq)
Write the equilibrium constant expression, K, for the following reaction taking place in dilute aqueous solution. HNO2(aq) + H,O(1)=H30*(aq) + NO2 (aq)
Write the balanced molecular chemical equation for the reaction in aqueous solution for cesium carbonate and magnesium nitrate. If no reaction occurs, write NR. CS2CO3 + Mg(NO3)2 →2 CSNO3 + M9CO3 04 02+03+ 4+ 3 6. 7 8. 6. 0. 口3||□4 Os 19 10 (s) (1) (g) (aq) Mg Mn N NR Cs 69°F O pe here to search 4- 2.
Complete and balance the following equations for reac- tions taking place in acidic solution. (a) VO;(aq)+ SO2 (g) (b) Br2(€) + SO2(g) (c) CrO?¯(aq) + Np** (aq) – (d) HCOOH(aq) + MnO, (aq) → CO2(g) + Mn²* (aq) (e) Hg,HPO4(s) + Au(s) + Cl¯(aq) → VO²*(aq) + SOž (aq) - → Br (aq) + Sof (aq) 4+ Cr** (aq) + NpOž* (aq) 2+ - Hg(€) + H2PO, (aq) + AuCl (aq)
2+ (a) MnO + VO²+ → Mn²+ + V(OH)4+ (b) I₂ + H₂S(g) → I¯¯ +S(s) 2+ (c) Cr₂O7²- + U4+ → Cr³+ + UO₂²+ (d) Cl + MnO₂ (s) → Cl₂(g) + Mn²+ (e) IO3 + I→ 1₂(aq) (f) IO3 + I + Cl¯ → IC₂ (g) HPO3²- + MnO4+OH → PO³+ MnO2- Write balanced redox equations for the following reactions. Show the full balancing process and supply H+ and/or H2O as needed to obtain balance. Item g is balanced in basic medium while the rest are in acidic medium. Identify the oxidizing agent and the reducing agent on the left side of each equation in the previous problem.
Assume the pe of the surface water of a lake is controlled by the O2/H2O half-reaction. What would the concentration of ferrous iron (Fe2") be in the system if it has a pH of 8 and it is in equilibrium with the atmosphere (Po2 = 0.21 atm)? Assume the temperature is 25 °C. log K pe O2(g) + 4H* + 4e" = 2H,0 83.1 20.78 FEOOH(s) + 3H* + e = Fe2* + 2H2O 13.5 13.50