Important InformationAtomic Masses (g/mol): H = 1.01, C = 12.01, N = 14.01, O = 16.00,%3D%3DNe = 20.18, CI = 35.45, K = 39.10, Ar = 39.95,Cu = 63.55, Ag = 107.87wwmConstants:R = 8.314 J/mol:K = 0.08206 L·atm/mol·Kw wwwF= 96,485 C/mol = 96,485 J/V-mol%D 9.The dissolution reactions of gold (Au) in 1M HNO3 and 1M aqua regia (1M HNO3 + 1M HCI) aregiven below.Au(s) + NO3+ 4 H+,(aq)→ Au3+(аq)+ NO(9) + 2 H20(1)(1)(аq)Au(s) + NO3+ 4 H* (aq)(aq)+ 4 Cl (aq)→ AuCl4"+ NO(9) + 2 H200(2)(аq)(g)Reduction Half – ReactionE° (V)-Au3+ + 3 e- 2 Au1.36AuCl4¯ + 3 e¯ → Au + 4 Cl-1.00NO3- + 4 H* + 3 e¯ → NO + 2 H200.962 H30* + 2 e-= H2 + 2 H209. a) Calculate E°cell and Keg for the dissolution of gold in 1M HNO3 under standard conditions.9. b) Calculate E°cell and Keg for the dissolution of gold in aqua regia under standard conditions.9. c) Using the values calculated in a) and b), determine the formation constant (K;) of AuCla".The formation reaction is given below. [Hint, express Kf as a function of the Keg values from a)and b)].3+Aušt (aa) + 4 Cl¯(ад)→ AuCl4(aq)

Whenever there is a reversal in the direction of reaction , the concerning Eo value gets changed.

The dissolution reactions of gold (Au) in 1M HNO3 and 1M aqua regia (1M HNO3 + 1M HCI) are given below. + N03 + 4 H* (aq) (ад) Au** (aq) + NO (g) +2 H20(1) Au(s) (1) Au(s) + NO3 + 4 H+, (aq) +4 Cl¯ (aq) AuCl4 + NO (g) (aq) + 2 H201) (2) (аq) Reduction Half – Reaction E° (V) Au3+ + 3 e¯ = Au 1.36 АuCly + 3 е — Аи + 4 cI- 1.00 NO3 + 4 H* + 3 e¯ → NO +2 H20 0.96 2 H30* + 2 e¯ = H2 +2 H20 Calculate E°cell and Keg for the dissolution of gold in 1M HNO3 under standard conditions. Calculate E°, cell and Keg for the dissolution of gold in aqua regia under standard conditions. Using the values calculated in a) and b), determine the formation constant (K;) of AuCl4. The formation reaction is given below. [Hint, express Kf as a function of the Keg values from a) and b)]. + 4 Cl (aq) (ад) AuCl4 (aq) Au³+

The dissolution reactions of gold (Au) in 1M HNO3 and 1M aqua regia (1M HNO3 + 1M HCI) are given below. + N03 + 4 H* (aq) (ад) Au** (aq) + NO (g) +2 H20(1) Au(s) (1) Au(s) + NO3 + 4 H+, (aq) +4 Cl¯ (aq) AuCl4 + NO (g) (aq) + 2 H201) (2) (аq) Reduction Half – Reaction E° (V) Au3+ + 3 e¯ = Au 1.36 АuCly + 3 е — Аи + 4 cI- 1.00 NO3 + 4 H* + 3 e¯ → NO +2 H20 0.96 2 H30* + 2 e¯ = H2 +2 H20 Calculate E°cell and Keg for the dissolution of gold in 1M HNO3 under standard conditions. Calculate E°, cell and Keg for the dissolution of gold in aqua regia under standard conditions. Using the values calculated in a) and b), determine the formation constant (K;) of AuCl4. The formation reaction is given below. [Hint, express Kf as a function of the Keg values from a) and b)]. + 4 Cl (aq) (ад) AuCl4 (aq) Au³+

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

Metal sulfides are prepared by bubbling hydrogen sulfide gas, H, S, through an aqueous solution containing the metal ion, and then adjusting the pH. When the solution is saturated with H, S, which occurs when [H,S] = 0.100 M, the equilibrium shown is established. H, S(aq) + 2 H, O(1) = s²-(aq) + 2H,O*(aq) Keq = 1.1 x 10-20 An aqueous solution containing 0.0521 M Pb2+ and 0.0521 M Ag* is saturated with H, S. Above what concentration of S²- will PbS precipitate? The Kyp of PbS is 8.9 × 10-29. [s²-] = M Above what concentration of S²- will Ag,S precipitate? The Kşp of Ag,S is 3.3 × 10-50. [s²-] = M If the pH of the solution is adjusted to 2.32, which species will precipitate from the saturated H, S solution? both PbS and Ag,S PbS neither species O Ag,S
Question attached
The solubility of salts that contain the conjugates of weak acids increase in acidic solution. Given the reaction of CUCN (Ksp = 3.47 x 10-20) with an acid in the form H3O+ shown below, find the equilibrium constant for this reaction given that Ka HCN = 4.9 x 10-10. CUCN(s) + H:O*(aq) = Cu"(aq) + HCN(aq) + H2O(1)
Among the solubility rules previously discussed is the statement: Carbonates, phosphates, borates, andarsenates—except those of the ammonium ion and the alkali metals—are insoluble. (a) Write the expression for the equilibrium constant for the reaction represented by the equationCaCO_3(s) ⇌ Ca^2+(aq) + CO3^1−(aq). Is Kc > 1, < 1, or ≈ 1? Explain your answer. (b) Write the expression for the equilibrium constant for the reaction represented by the equation3Ba^2+(aq) + 2PO_4^3−(aq) ⇌ Ba_3(PO_4)_2(s). Is Kc > 1, < 1, or ≈ 1? Explain your answer.
At 25 °C, only 0.0110 mol of the generic salt AB2 is soluble in 1.00 L of water. What is the Ksp of the salt at 25 °C? AB, (s) = A2+(aq) + 2B¯(aq)
Could you please baland identify what type of reaction this is?
What is the molar solubility of a hypothetical compound AB in pure water given a Ksp = 5 x 102? AB(5)= A"(aq) + B´(aq)
Parts 4A and 4B please
At 25°C only 0.0687 moles of LiCl is soluble in 1.00 L of water. What is the Kp of the salt at this temperature? LICI (s) = Li* (aq) + Cl- (aq) Give your answer to 3 significant figures.
Write the equilibrium constant expression for acetic acid, and calculate a K value and an apparent percent dissociation for each concentration + ICE tables for 0.10 M HC2H302 +0.010 M +0.0010 M. (ph for 0.10M is 3.3, pH for 0.010 M is 3.7, ph for0.0010 M is 4.4) HA(aq) = H+(aq) + A-(aq)
You have found the following: CaSO4(s) <=> Ca+2(aq) + SO4-2(aq) K = (6.053x10^-5) What is the value of K for the following reaction? 2 CaSO4(s) <=> 2 Ca+2(aq) + 2 SO4-2(aq) Note: Your answer is assumed to be reduced to the highest power possible. Please provide neat and clean handwriting and clear image Give answer correctly
If a solution initially contains 0.240 M HC2H3O2, what is the equilibrium concentration of H3O+ at 25 ∘C?