Use the molar ∆Hf° under formulas to calculate ∆H°rxn for the equations as balanced: 1. 4Al2O3 + 3CH4 → 8Al + 3CO2 + 6H2O     ∆H°rxn = ______ kJ  exo ? endo_thermic ∆H°f = –1676   –75 ___  –394 –242 kJ/mol 2. MnO2(s) + 2CO(g) → Mn(s) + 2CO2(g)  ∆H°rxn = ______ kJ  ∆H°f = –520       –111         ___  –394  kJ/mol exo ? endo_thermic 3. CF4(g) + 2H2O(g) → CO2(s) + 4HF(g)    ∆H°rxn = ______ kJ  ∆H°f =  –934   –242   –394  –273  kJ/mol exo ? endo_thermic

Q: The equation for the corrosion of iron to form iron (III) oxide (aka, rust) is: 4 Fe(s) + 3 O2(g) -à…

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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: Calculate ΔGrxn at 338 K under the conditions shown below for the following reaction.

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Q: The reaction                         2 NO(g)   ⇆  N2O4(g) occurs at 25oC under standard state…

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Q: Consider the reaction 3NO (g) → NO2(g) + N2O (g) a. Using a thermodynamic data table, calculate Go…

A: Given reaction: 3NO (g) → NO2(g) + N2O (g) Given: ∆G∘f(NO2)= 51.84 KJ/mol ∆G∘f(N2O) = 103.59 KJ/mol…

Q: What is Δ G° at 25 °C?   N 2O 4(g) → 2 NO 2(g) Δ H° = 58.03 kJ Δ S° = 176.7 J/K

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Q: Given the following table of thermodynamic data,   Substance ΔH∘f(kJ/mol)   S∘(J/mol⋅K)   H2(g)…

A: The "spontaneous reactions" always favor "forward reactions" where more product gets yielded and…

Q: The neutralization of a strong acid and strong base has an enthalpy change, ∆H°, = -55.9 kJ/mol. The…

A: The relationship between the ΔG0 and equilibrium constant is given by  RTln(K) = -ΔG0  where R = gas…

Q: 2 ClO2 (g)   +  2 TiCl4 (l)    →     2 TiO2 (s)   +   5 Cl2 (g)         Delta H =  – 343.8 kJ when…

A: Please have a look on the solutiion:

Q: Calculate ΔS°rxn for the balanced chemical equation:2 H2S(g) + 3 O2(g)¡2 H2O(g) + 2 SO2(g)

A: The given reaction is: ∆S˚rxn for the reaction is given by:

Q: Given the thermodynamic data, which of the following is acceptable in regards to the reaction shown?…

A: Explained as follows

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: At 869 K, ΔGo equals -82.7 kJ for the reaction, Cl2(g) 2 Cl(g).  Calculate the value of ln K for…

A: The equilibrium constant can be written as the ratio of concentration of products to the…

Q: [Referenc A student determines the value of the equilibrium constant to be 2.41x1016 for the…

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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: Calculate AH and AS for the following reaction at 25 °C. Use the AH; and S" values in this table of…

A: To calculate the enthalpy change (ΔH), entropy change (ΔS), and Gibbs free energy change (ΔG) for…

Q: This industrial chemical reaction process generates nitrogen monoxide, an important component in the…

A: The question is based on the concept chemical thermodynamics.   We have been given  chemical…

Q: An endothermic reaction can be demonstrated by freezing an Erlenmeyer flask to a piece of plywood…

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Q: AH°rxn = -150 kJ/mol and AS°rxn = -413 J/mol* АВ (g) + 2C (g) > АВС2 (g) plied reaction data, what…

A: A reaction is spontaneous when value of change in Gibbs Free Energy is negative i.e. value of ∆G.

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: Given the following: P,(s) + 50,(g) → P,0,(s) A G° = – 2697.0 kJ/mol2H, (g) +0,(g) → 2H,0(g) A G° =…

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Q: A student determines the value of the equilibrium constant to be 4.03×10-18 for the following…

A: Solution-  ∆Gorxn is given as,-∆Gorxn=-RT ln Keq.=-8.314 Jmol-1K-1×298K× ln( 4.03×10-18)=-8.314…

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: Calculate ΔSϴ for the reduction of aluminum oxide by hydrogen gas: Al2O3(s) + 3H2(g) → 2Al(s) +…

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Q: A reaction will be spontaneous only at low temperatures if both ΔH and ΔS are negative. For a…

A: given: ∆H=-320.1KJ/mol        =-320100J/mol∆S=-95J/K.mol

Q: C3H8 (g)  +  5 O2 (g) →   3 CO2 (g)   +  4 H2O (l)  Calculate the Gibb’s Free Energy at 2000.°C…

A: Gibbs free energy, (measured in joules in SI) is the maximum amount of non-expansion work that can…

Q: At 25 °C, what is the Keq for a reaction where ΔH∘= –9.3 kJ/mol and ΔS∘= 75.5 J/mol·K?

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Q: Calculate ΔGº, ΔHº, and ΔSº at 25ºC for the reaction below in the indicated units. [Use…

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Q: ion 3: (a) What is the second law of thermodynamics? For any process, there are four possible sign…

A: Given,                             Enthalpy of Vaporization = 58.51 KJ / mol…

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

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Q: Given the following equation, H2O(g) + CO(g) → H2(g) + CO2(g)             ΔG°rxn = -28.6 kJ…

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Q: Ammonia can be produced by the reaction of hydrogen gas and nitrogen gas, as shown below: N₂(g) +…

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

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

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Q: Urea (NH2CONH2), an important nitrogen fertilizer, is produced industrially by the following…

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Q: A particular reaction has a ΔHo value of -157. kJ and ΔSo of -343. J/mol K at 298 K. Assuming that…

A: ∆H° = -157 kJ/mol ∆S° = -343 J/mol-K T = 298 K  We have to determine the temperature when…