Consider the reaction for the dissolution of AgCl in water below at 25⁰C: AgCl(s) DAg+(aq) + Cl-(aq)...

Question

Question

Consider the reaction for the dissolution of AgCl in water below at 25⁰C: AgCl(s) DAg+(aq) + Cl-(aq)...

Consider the reaction for the dissolution of AgCl in water below at 25⁰C: AgCl(s) DAg⁺(aq) + Cl^-(aq)
1. Using the standard free energy of formation values (ΔG⁰_f) from the appendix, calculate the Kc value for this reaction.
2. Calculate the ΔG for the dissolving of AgCl in water at 25⁰C when:

[Ag⁺]=[Cl^-]= 1.00 x 10^-4M

science chemistry

Add a comment Improve this question Transcribed image text

Answer 1

Answer #1

Add a comment

Answer 2

Similar Homework Help Questions

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)...

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=
To decide whether AgCl should dissolve in water ( spontaneous reaction ) at 25 degrees celcius, the delta H and T delta...

To decide whether AgCl should dissolve in water ( spontaneous reaction ) at 25 degrees celcius, the delta H and T delta S must be used in the Gibbs Free Energy equation to calculate delta G AgCl (s) + H2O (I) -> Ag+ + Cl- + H2O Standard Enthalpies of formation and standard entropies of common compounds substance state AgCl s -127010 96.20 Cl- aq -167080. 56.50 Ag+ aq. 105790. 72.70
AgCl (s) + --> <-- Ag + (aq) + Cl- (aq) Shown above is information about...

AgCl (s) + --> <-- Ag + (aq) + Cl- (aq) Shown above is information about the dissolution of AgCl in water at 298 K. In a chemistry lab a student wants to determine the value of s, the molar solubility of AgCl, by measuring [Ag+] in a saturated solution prepared by mixing excess AgCl and distilled water. How would the results of the experiment be altered if the student mixed excess AgCl with tap water (in which [Cl-] =...

For the dissolution of thenardite shown below, calculate the following (at STP, 25 °C and 1...

For the dissolution of thenardite shown below, calculate the following (at STP, 25 °C and 1 atm):Na2SO4 (s) ↔ 2Na+(aq) + SO42-(aq) (a) standard??° enthalpy of reaction (∆????°), ??° (b) standard Gibbs free energy of reaction (∆?? ) using standard Gibbs free energy of formation values (∆?? ), and (c) equilibrium constant (K). (d) Is this a spontaneous reaction [i.e., the dissolution reaction (left to right)]? Explain.
When solutions containing silver ions and chloride ions are mixed, silver chloride precipitates: Ag+(aq)+Cl−(aq)→AgCl(s)ΔH=−65.5kJ A.) Calculate...

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.
When solutions containing silver ions and chloride ions are mixed, silver chloride precipitates: Ag+(aq)+Cl−(aq)→AgCl(...

When solutions containing silver ions and chloride ions are mixed, silver chloride precipitates: Ag+(aq)+Cl−(aq)→AgCl(s)ΔH=−65.5kJ Calculate ΔH for formation of 0.490 mol of AgCl by this reaction. Calculate ΔH for the formation of 7.50 g of AgCl. Calculate ΔH when 9.23×10−4 mol of AgCl dissolves in water.

Question 8 (1 point) The standard potential of the cell Sn(s) Sn2(aq) || Cl(aq)| AgCl(s) |...

Question 8 (1 point) The standard potential of the cell Sn(s) Sn2(aq) || Cl(aq)| AgCl(s) | Ag(s) is +0,36 V at 25°C. If the standard reduction potential of the AgCl|Ag Cl-couple is 0.22 V, calculate the standard reduction potential of the Sn? Isn couple. 0 -0.14 V +0.36 V -0.07 V +0.14 V +0.58 V
Consider the following Gibbs energies at 25 "C Substance Ag (aq) Cr(aq) AgCI(s) Br(aq) AgBr(s) 77.1...

Consider the following Gibbs energies at 25 "C Substance Ag (aq) Cr(aq) AgCI(s) Br(aq) AgBr(s) 77.1 - 131.2 - 109.8 - 104.0 -96.9 (a) Calculate AG rn for the dissolution of AgCl(s). (b) Calculate the solubility-product constant of AgCl Number Number kJ mol (c) Calculate Δ3rxn for the dissolution of AgBr(s). (d) Calculate the solubility-product constant of AgBr Number Number kJ mol
< Question 13 of 18 > Consider the Gibbs energies at 25 °C. Substance AG (kJ....

< 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=

2. (20%) The standard potential of the AgCl/Ag, Cr couple fits the expression FO 0.23659-4.8564x10 0-3.4205x106 +5.869x10 8 Unit: E (V; 0 °c) Where: [4G"(H) = 0]; [4,Ge(Ag) = 0]; [4H.(H): 0];...

2. (20%) The standard potential of the AgCl/Ag, Cr couple fits the expression FO 0.23659-4.8564x10 0-3.4205x106 +5.869x10 8 Unit: E (V; 0 °c) Where: [4G"(H) = 0]; [4,Ge(Ag) = 0]; [4H.(H): 0]; [4m(Ag) = 0] (a) Evaluate the standard reaction Gibbs energy (G enthalpy (4,He) and entropy (4,Se ) at 298K (b) Calculate the standard Gibbs energy (ApG"(cr)and enthalpy(A4"(cr)of formation of Cl (aq) 2. (20%) The standard potential of the AgCl/Ag, Cr couple fits the expression FO 0.23659-4.8564x10 0-3.4205x106 +5.869x10...

Consider the reaction for the dissolution of AgCl in water below at 25⁰C: AgCl(s) DAg+(aq) + Cl-(aq)...

Homework Answers

Add Answer to:
Consider the reaction for the dissolution of AgCl in water below at 25⁰C: AgCl(s) DAg+(aq) + Cl-(aq)...

Post as a guest

Earn Coins

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)...

To decide whether AgCl should dissolve in water ( spontaneous reaction ) at 25 degrees celcius, the delta H and T delta...

AgCl (s) + --> <-- Ag + (aq) + Cl- (aq) Shown above is information about...

For the dissolution of thenardite shown below, calculate the following (at STP, 25 °C and 1...

When solutions containing silver ions and chloride ions are mixed, silver chloride precipitates: Ag+(aq)+Cl−(aq)→AgCl(s)ΔH=−65.5kJ A.) Calculate...

When solutions containing silver ions and chloride ions are mixed, silver chloride precipitates: Ag+(aq)+Cl−(aq)→AgCl(...

Question 8 (1 point) The standard potential of the cell Sn(s) Sn2(aq) || Cl(aq)| AgCl(s) |...

Consider the following Gibbs energies at 25 "C Substance Ag (aq) Cr(aq) AgCI(s) Br(aq) AgBr(s) 77.1...

< Question 13 of 18 > Consider the Gibbs energies at 25 °C. Substance AG (kJ....

2. (20%) The standard potential of the AgCl/Ag, Cr couple fits the expression FO 0.23659-4.8564x10 0-3.4205x106 +5.869x10 8 Unit: E (V; 0 °c) Where: [4G"(H) = 0]; [4,Ge(Ag) = 0]; [4H.(H): 0];...

Consider the reaction for the dissolution of AgCl in water below at 25⁰C: AgCl(s) DAg+(aq) + Cl-(aq)...

Homework Answers

Add Answer to: Consider the reaction for the dissolution of AgCl in water below at 25⁰C: AgCl(s) DAg+(aq) + Cl-(aq)...

Post as a guest

Earn Coins

Add Answer to:
Consider the reaction for the dissolution of AgCl in water below at 25⁰C: AgCl(s) DAg+(aq) + Cl-(aq)...