2 Ag20(s) → 4 Ag(s) + O2(g) Thermodynamic data are given below. 2 Ag20(s) → 4 Ag(s) + 02(g) AfH°(kJ/mol) -31.1 S°(J/K•mol) 121.3 42.55 - 205.07 Is the decomposition of silver(I) oxide product-favored at 25 °C? AH° = 62.2 kJ AS° = 132.7 J/K %3D AG° = 22.66 kJ

2 Ag20(s) → 4 Ag(s) + O2(g) Thermodynamic data are given below. 2 Ag20(s) → 4 Ag(s) + 02(g) AfH°(kJ/mol) -31.1 S°(J/K•mol) 121.3 42.55 - 205.07 Is the decomposition of silver(I) oxide product-favored at 25 °C? AH° = 62.2 kJ AS° = 132.7 J/K %3D AG° = 22.66 kJ

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

Related questions

Q: Use the data from this table of thermodynamic properties to calculate the values of ASixn for each…

A: ΔS°rxn = Σni x S°(Product) - Σni x S°(Reactant)Where,ni is stoichiometric coefficient of respective…

Q: chapter 12: 9) What are ΔH°rxn, ΔS°rxn, and ΔG239.0 K for the following reactions at 239.0 K?…

A: Given Temperature = 239.0°K Compound ΔHºf (kJ/mol) Sº (J/mol • K) H2S(g) –20.17 205.6…

Q: Hydrogen reacts with nitrogen to form ammonia (NH3) according to the following reaction: 3 H2 (g) +…

Q: In a reaction, 1.00 mole of H2 is produced at a constant pressure of 1.00 atm and at 298 K (1 L atm…

A: Therefore, ΔE in this reaction is +483.6 kJ.Explanation:The equation for calculating ΔE is:ΔE = ΔH -…

Q: For a particular reaction, Δ?=120.5 kJ/mol and Δ?=758.2 J/(mol·K). Calculate Δ? for this reaction at…

A: Given data is ΔH = 120.5 KJ/mol = 120500 J/mol And ΔS = 758.2 J/mol.K Since ΔG = ΔH - TΔS where T =…

Q: Calculate AG° for the reaction shown below using the provided thermodynamic properties information.…

A: Gibbs energy chane (∆G°) of a reaction is given by the relation ∆G° = ∆H° - T∆S° ∆H° = enthalpy…

Q: free

Q: ΔrS = 94.6 J K−1mol−1 ΔrH = 175.98 kJ/mol NH4Cl (s) → NH3 (g) + HCl (g) a) Calculate the ΔrG for…

A: #(d): Given the total pressure of the reaction mixture, Pt = 56 kPa

Q: Use the values found in Thermodynamic Properties to determine AS°, AH° and AGO at 298 K for the…

A: The Answer to the following question is-

Q: What is the free energy change when silver chloride form at 2000.0 K? Ag+ (aq) + Cl– (aq) →…

Q: 15) Consider the reaction for the decomposition of carbon tetrachloride gas: CCIA(g) C(s, graphite)…

Q: Consider the reaction, HQ = H+(aq) + Q¯(aq). At 350.0 K, the AS°rxn = -81.0 J/mol K and the AH°rxn =…

Q: For a particular reaction, Δ?=139.99 kJ and Δ?=298.7 J/K. Calculate Δ? for this reaction at 298 K.…

A: Given, ∆H = 139.99 KJ ∆S = 298.7 J / K T = 298 K.

Q: Calculate the temperature of the following reaction, If ΔGrxn° = -29.22 kJ/mol, ΔH°= 9.12 kJ/mol…

Q: Calculate ΔGrxn at 400 K for the reaction below when PCO = 2.40 atm and PCO2 = 4.10 atm. Fe2O3(s)…

A: ΔG°rxn = –28.0 kJ T = 400K

Q: Given the following data, predict whether the reaction below is spontaneous at 25°C: NO2(9) + N20(9)…

A: The given reaction is as follows: NO2(g) + N2O(g) →3NO(g) The ∆rG° of the reaction can be calculated…

Q: Calculate the standard free energy change (kJ/mol) for the reaction shown at a temperature of 298.15…

Q: For the reaction, A + B --> C, AHO = +30 kJ; AS° = +50 J/K. Therefore the reaction is: spontaneous…

A: For the reaction: For a spontaneous reaction,

Q: For the reaction below AH = +92.2 kJ, and AS = +198.7 J/K. Estimate the temperature at which this…

A: To find the temperature.

Q: Recovering aluminum directly from its ore, which is primarily aluminum oxide, involves the following…

Q: Consider the following reaction: 2 O3(g) → 3 O2(g) ΔS∘∘ = 137.4 J/K; ΔH∘∘ = −285.4 kJ…

A: To calculate ΔGo for the given reaction.

Q: Сalculate ∆H° for the reaction: N2O(g) + 1/2 O2(g) → 2NO(g)

Q: Given the thermodynamic data below, calculate the value of the equilibrium constant for the reaction…

A: Given data, ∆H° = 180.50 KJ = 180500 J ∆S° = 24.77 J/K Temperature (T) = 25°C = (273+25) = 298 K

Q: From the values of AH and AS, predict which of the following reactions would be spontaneous at 25°C:…

A: H for A = 10.5 kJ/molS for A = 30 J/molKH for B = 1.8 kJ/molS for B = -113 J/molKT=25oC=25+273=298K

Q: Consider the (endothermic) thermal decomposition of calcium carbonate: CaCO3(?) → CaO(?) + CO2(?).…

A: Given, Thermal decomposition of calcium carbonate. CaCO3(s)⇌CaO(s)+CO2 (g) It is an example of…

Q: Which are spontaneous at high temperatures? Choose one or more: A 2H,S(g) + 30,(g) –→ 2H,0(g) +…

Q: Calculate the standard free energy change (kJ/mol) for the reaction shown at a temperature of 298.15…

Q: Consider the following thermodynamic table. S* (J/mol-K) H (kJ/mol) G (kJ/mol) Ca(ОН)2 (5) 83.4…

A: Here we have to predict from the given thermodynamics data for dissolution of Ca(OH)2 is exothermic…

Q: Calculate ΔrS° at 25°C for the combustion of methanol: ΔrH°= -638.6 unbalanced equation: CH3OH(l) +…

A: Given :- The Balanced equation for combustion of methanol CH3OH(l) + 3/2 O2(g) → CO2(g) + 2…

Q: The value of AS°

Q: Calculate ASO for the reaction SICI4(g) + 2Mg(s) → 2MgCl2(s) + Si(s) Substance SICI4(g) Mg(s)…

A: Entropy (S) :- Entropy is a measure of disorderness or randomness in a system. The change in…

Q: For the following hypothetical reaction, use the thermodynamic data provided below to determine the…

Q: Find AG for the following reaction, at 25°C, using AH and S f NH4Cl(s) NH3(g) + HCl(g) kJ Substance…

A: Answer: Enthalpy change for a reaction is equal to the difference between enthalpy of formation of…

Q: The temperature at which the following process reaches equilibrium at 1.0 atm is the normal boiling…

Q: Consider the reaction: FeO (s) + Fe (s) + O2 (g) → Fe2O3 (s) Given the following table of…

Q: Estimate ΔG°rxn for the following reaction at 317 K. HCN(g) + 2 H2(g) → CH3NH2(g) ΔH°= -158.0 kJ;…

Q: Calculate ΔrH° at 25°C for the combustion of methanol: Unbalanced reaction: CH3OH(l) + 3/2O2(g) →…

Q: Consider the reaction: CO(g) + Cl2(g)–→COC12(g) Using standard thermodynamic data at 298K, calculate…

A: Free energy change of a reaction is deltGo=[deltaGo products-deltaGoreactants ] KJ/mol

Q: Calculate the ΔG∘rxn for 2ClF (g) + Br2 (g) <------> 2ClBr (g) + F2 (g) _____ kJ/mol

Q: Consider the following reaction. Use the information here to determine the value of ΔSsurr at 355…

Q: Calculate the ΔS°rxn of the following reaction at 215°C and standard pressure. C2H4 (g)+302…

A: The values of standard entropy – C2H4 = 219.5 J/mol.K O2 = 205 J/mol.K CO2 = 213.6 J/mol.K H2O =…

Q: Which reaction(s) will be spontaneous at all temperatures? : 4NH3(g) + O2(g) → 2N2(g) + 6H2O(g) ΔrH…

A: For a chemical reaction to be spontaneous, Gibbs free energy, ∆rG should be negative. ∆rG is…

Q: Calculate Δ S° for the following reaction. N 2( g) + 2 O 2( g) → 2 NO 2( g) a: -121.5 J/K b: 636.5…

A: The formula used to get the Δ S° for any reaction is given as - Δ S°rxn = Δ S°pdt - Δ S°rct

Question

b Some metal oxides can be decomposed to the metal and oxygen under reasonable conditions.
2 Ag20(s) → 4 Ag(s) + O2(g)
Thermodynamic data are given below.
2 Ag20(s) → 4 Ag(s) + 02(g)
AfH°(kJ/mol) -31.1
S°(J/K•mol)
121.3
42.55 -
205.07
Is the decomposition of silver(I) oxide product-favored at 25 °C?
AH° = 62.2 kJ
AS° = 132.7 J/K
AG° = 22.66 kJ
Yes
No

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Answer

VIEW

Explanation

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Consider the reaction: NH3 (g) + HCI (g) → NH4Cl (s) Given the following table of thermodynamic data at 298 K: Substance AH° (kJ/mol) S° (J/K-mol) NH3 (g) -46.19 192.5 HCI (g) -92.30 186.69 NH4Cl (s) -314.4 94.6 The value of K for the reaction at 25 °C is 1.1-10-16 9.3 - 1015 1.4.108 150 8.4. 104 Submit Request Answer
chapter 12: 9) What are ΔH°rxn, ΔS°rxn, and ΔG239.0 K for the following reactions at 239.0 K? Compound ΔHºf (kJ/mol) Sº (J/mol • K) H2S(g) –20.17 205.6 O2(g) 0 205.0 H2O(g) –241.8 188.7 SO2(g) –296.8 248.2 SO3(g) –395.7 256.8 H2O(l) –285.8 70 H2SO4(l) –814.0 156.9 S(g) 277.2 167.8 a) 2H2S(g)+3O22H2O(g)+2SO2(g) ΔHºrxn = ΔSºrxn = ΔG239.0 K =
For a chemical reaction, ΔSrxn = –200 J/K, and ΔHrxn = –50 kJ at approximately 298 K. At what temperatures will the reaction be spontaneous, if ever? The reaction is never spontaneous at any temperature. The reaction is spontaneous at high temperatures. The reaction is spontaneous at any temperature. The reaction is spontaneous at low temperatures. (this is correct but why?)
Calculate the standard free energy change (kJ/mol) for the reaction shown at a temperature of 298.15 K using the information provided. Reaction ΔHrxn (kJ/mol) ΔSrxn (J/mol-K) 2 Mn(s) + 3 O2(g) → 2 Mn2O3(s) -1917.9 -458.7
Calculate ΔGrxn at 375 K for the reaction below when PCO = 2.20 atm and PCO2 = 5.10 atm. Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g) ΔG°rxn = –28.0 kJ
Give detailed mechanism Solution with explanation needed..don't give Handwritten answer
Calculate the standard free-energy changes for the following reactions at 25°C. CH4(g) + 2O2(g) → CO2(g) + 2H2O(l) 2MgO(s) → 2Mg(s) + O2(g) Inorganic Substances Substance ΔHo (kJ/mol) f ΔGo (kJ/mol) f So (J/K·mol) CO(g) -110.5 -137.3 197.9 CO2(g) -393.5 -394.4 213.6 H2(g) 0 0 131.0 H2O(l) -285.8 -237.2 69.9 O2(g) 0 0 205.0 Organic Substances CH4(g) -74.85 -50.8 186.2 Mg(s) 0 0 32.5 MgO(s) -601.8 569.6 26.78 Table 1. Selected Thermodynamic Data at 1 atm and 25°C* *The ΔHof, ΔGof and S° values for ions are based on the reference states ΔHof (H+) = 0, ΔGof (H+) = 0, and S°(H+) = 0.
A reaction has AH°= 100 kJ/mol and AS°= 250 J/mol.K. Is the reaction spontaneous at room temperature? If not, under what temperature conditions will it become spontaneous?
) Calculate ΔS°rxn for the following reaction. The S° for each species is shown below the reaction. 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g) S°(J/mol∙K) 192.8 205.2 210.8 188.8 A) +287.4 J/K B) -401.2 J/K C) +160.0 J/K D) -336.6 J/K E) +178.8 J/K
Consider the following reaction: CaCO 3(s) <—> CaO (g) +CO 2(g) For this reaction, delta S = +158.9 J/ mol and Delta * H ^ o = + 177.9kJ / (mol) . These values are fairly constant with changes in temperature. Over what specific temperature range is this reaction spontaneous in the forward direction?
For a particular reaction, Δ?=−14.20 kJ and Δ?=−198.5 J/K. Calculate Δ? for this reaction at 298 K
The enthalpy and entropy changes for a reaction at 298 K are ∆H = 46 kJ and ∆S = 190 J/K. Which of the following best describes this reaction A) The reaction is spontaneous and driven by favorable changes in the enthalpy and entropy. B) The reaction is not spontaneous because heat is absorbed. C) The reaction is not spontaneoius but could be spontaneous at a higher temperature. D) The reaction is spontaneous and driven by the favorable entropy change.