Use the data given to calculate the value of Κ for the reaction
at 5°C
Ag+(aq) + Cl− (aq) AgCl(s)
AgCl(s) | Ag+(aq) | Cl− (aq) | |
S° (J K−1 mol−1) | 96.2 | 72.68 | 56.4 |
ΔH°f (kJ/mol) | −127.07 | 105.58 | −167.2 |
a. |
5.7 × 109 |
|
b. |
1.0 |
|
c. |
3.7 × 1010 |
|
d. |
1.3 × 106 |
|
e. |
1.9 × 1012 |
Use the data given to calculate the value of Κ for the reaction at 5°C Ag+(aq)...
so (K-1 moll) AHºf (kJ/mol) crac) 56.4 +1672 72.68 105.58 for the reaction at 25°C Agche 196.2 127.0 Use the data given to calculate the value of AG AgCl(s) - Ag" (aq) + (aq) O a -55.71) b. -32.5 kJ OC -75.21 d. -55.7 kJ Oe-7520
so (K-1 moll) AHºf (kJ/mol) crac) 56.4 +1672 72.68 105.58 for the reaction at 25°C Agche 196.2 127.0 Use the data given to calculate the value of AG AgCl(s) - Ag" (aq) + (aq) O a -55.71) b. -32.5 kJ OC -75.21 d. -55.7 kJ Oe-7520
When solutions containing silver ions and chloride ions are mixed, silver chloride precipitates: Ag+(aq)+Cl−(aq)→AgCl(s)ΔH=−65.5kJ A.) Calculate ΔH for formation of 0.100 mol of AgCl by this reaction. I got A ΔH=-6.55 kJ B.) Calculate ΔH for the formation of 2.80 g of AgCl. C.) Calculate ΔH when 0.110 mmol of AgCl dissolves in water. Need help with B and C.
< Question 13 of 18 > Consider the Gibbs energies at 25 °C. Substance AG (kJ. mol-!) Ag+ (aq) 77.1 Cl(aq) -131.2 AgCl(s) -109.8 Br" (aq) -104.0 AgBr(s) -96.9 (a) Calculate AGran for the dissolution of AgCl(s). kJ. mol- (b) Calculate the solubility-product constant of AgCl. kJ. mol- (b) Calculate the solubility product constant of AgCl. K = Enter numeric value (c) Calculate AGtx for the dissolution of AgBr(s). kl. mol-? (d) Calculate the solubility-product constant of AgBr. K=
Consider the Gibbs energies at 25 ∘C. SubstanceSubstance ΔG∘f (kJ⋅mol−1)ΔGf∘ (kJ·mol−1) Ag+(aq)Ag+(aq) 77.177.1 Cl−(aq)Cl−(aq) −131.2−131.2 AgCl(s)AgCl(s) −109.8−109.8 Br−(aq)Br−(aq) −104.0−104.0 AgBr(s)AgBr(s) −96.9−96.9 (a) Calculate ΔG∘rxn for the dissolution of AgCl(s)AgCl(s). kJ⋅mol−1 (b) Calculate the solubility-product constant of AgCl. K= (c) Calculate ΔG∘rxnΔGrxn∘ for the dissolution of AgBr(s)AgBr(s). kJ⋅mol−1kJ⋅mol−1 (d) Calculate the solubility-product constant of AgBr. K=K=
Please List Steps, show all work & explain logicCalculate [Ag^+] at 298K for the following reaction as written using the conditions listed below: AgCl (s) rightarrow Ag^+ (aq) + Cl^-(aq) [Cl^-] = 1.0 times 10^-10 M delta G = -58.496 kJ/mol delta G degree = +55.600 kJ/mol 1.0 times 10^-10 M 1.0 M 1.3 times 10^-5 M 7.9 times 10^-8 M There is no Ag^+ (aq) in the solution.
Calculate ΔG°rxn,298 and ΔGrxn,298 for the following. a) Ag+(aq) + Cl-(aq) -> AgCl (s) b) Ag+(aq) + I-(aq) -> AgI (s) c) Ag+(aq) + NO3-(aq) -> AgNO3 (aq) d) Ag+(aq) + SO4 2-(aq) -> Ag2SO4(aq) e) Ba 2+(aq) + 2Cl- (aq) + 2H2O (l) -> BaCl2 • 2H2O f) Ba 2+(aq) + 2NO3-(aq) -> Ba(NO3)2 (aq) ΔGo, 298 values for 1M solutions NO3 -108.74 -33.41 SO42 -744.53 -618.41 Cl -109.789 -1296.32 W2 -384.138 Anions (kJ/mol) Cations (kJ/mol) -51.57 -66.19 Ag...
The salt ammonium chloride dissolves in water according to the reaction: NH4Cl(s) NH4+(aq) + Cl-(aq) (a) Calculate the standard enthalpy change ΔH° for this reaction, using the following data: NH4Cl(s) = -314.4 kJ mol-1 NH4+(aq) = -132.5 kJ mol-1 Cl-(aq) = -167.2 kJ mol-1 kJ (b) Calculate the temperature reached by the solution formed when 35.3 g of NH4Cl is dissolved in 0.160 L of water at 24.6 °C. Approximate the heat capacity of the solution by the heat capacity...
Determine the standard entropy change of the universe at 25°C for the reaction NHİ (aq) + Cl-(aq) NH, Cl (s) given the following information. Is the reaction spontaneous under standard conditions? Substance Δ AHP(kJ/mol) S° (J/mol K) NH,Cl(s) NH (aq) Cl (aq) -314.4 -132.5 -167.2 94.6 113.4 56.5 +124.6 J/K, yes +26.0 J/K, yes d. a. -26.0 J/K, no b. +49.3 J/K, yes c. -75.3 J/K, no e.
QUESTION 45 For the reaction Ag+ (aq) + Cr (aq) - AOCI (5) Given the following table of thermodynamic data, Substance AHF (k]/mol) S (I/mol.K) Ag+ (aq) 105.90 73.93 a- (aq) -167.2 56.5 AgCl (5) -127.0 96.11 determine the temperature at which the reaction becomes spontaneous O 1640 K O 1914 K 0 432K O 850K O 522K QUESTION 46 What is the low for a solution at 25°c that has a pH of 8 647 O 1.2 x 10-10...