Given the reactions,   X(s)+12O2(g)⟶XO(s)   Δ?=−959.7 kJX(s)+12O2(g)⟶XO(s)   ΔH=−959.7 kJ     XCO3(s)⟶XO(s)+CO2(g)Δ?=+283.9 kJXCO3(s)⟶XO(s)+CO2(g)ΔH=+283.9 kJ   what is Δ?ΔH for this reaction?   X(s)+12O2(g)+CO2(g)⟶XCO3(s)X(s)+12O2(g)+CO2(g)⟶XCO3(s)   Δ?=

Q: Using values from Appendix C of your textbook, calculate the value of AHO for each of the following…

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Q: Calculate the ΔH for the reaction: 4 NH3 (g) + 5 O2 (g) --> 4 NO (g) + 6 H2O (g) from the following…

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Q: Calculate the enthalpy of the reaction 4B(s)+3O2(g)→2B2O3(s)4B(s)+3O2(g)→2B2O3(s) given the…

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Q: Use the standard reaction enthalpies given below to determine AH°rxn for the following reaction: 4…

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Q: Given the reactions, X(s)+12O2(g)⟶XO(s) Δ?=−635.1 kJ XCO3(s)⟶XO(s)+CO2(g)…

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Q: Calculate ΔfH∘(SO3) from the following information in kJ/mol .  S(s)+O2(g)⟶SO2(g)ΔrH∘= −296.8…

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Q: What is the standard enthalpy change for this reaction at 298 K? 2 K(s) + 1/2 O2(g)  K2O(s)  kJ

A: For given reaction, ∆H°  = 722 KJ  Calculation ∆ H° for  2K (s) + 1/2 O2 (g)  ---> K2O (s)

Q: Use the data below to determine the ΔHrxn for the following reaction: H2C=CH2(g) + 3O2(g) è 2CO2(g)…

A: ∆Hrxn can be calculated using given bond energies.

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Q: Consider the reaction N2(g)+3H2(g)→2NH3(g),N2(g)+3H2(g)→2NH3(g), ΔHΔH =−92.3kJ mol−1=−92.3kJ mol−1…

A:

Q: From experiments, you know the following thermochemical equations: CaO(s) + 2HCl(aq) ---> CaCl2(aq)…

A: Given: CaO(s)+2HCl(aq)→CaCl2(aq)+H2O(l)       ∆H1=-186 kJ ---eqn(1)CaO(s)+H2O(l)→Ca(OH)2(s)…

Q: Ammonia will burn in the presence of a platinum catalyst to produce nitric oxide, NO: 4 NH3(g) + 5…

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Q: Given the reactions, X(s)+1/2 O2(g)⟶XO(s)   Δ?=−613.7 kJ XCO3(s)⟶XO(s)+CO2(g) Δ?=+148.1 kJ what is…

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Q: Given the dataN2(g)+ O2(g)-----> 2 NO(g) ΔH = +180.7 kJ2 NO(g) + O2(g)----> 2 NO2(g) ΔH =…

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Q: Predict the sign of the enthalpy change for the following processes. Give a reason for your…

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Q: Given the reactions, X(s)+12O2(g)⟶XO(s)   Δ?=−840.9 kJX(s)+12O2(g)⟶XO(s)   ΔH=−840.9 kJ…

A:

Q: Which of the following is ΔH for the process Hg2Cl2 (s) → 2Hg(l) + Cl2(g)? Given: (1) Hg(l) + Cl2(g)…

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Q: Given the following reactions and corresponding ΔH values, find the ΔH (to the nearest whole #) for…

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Q: [tot] 3Li(s) + (1/2)N2(g) → Li3N(s) ΔH(tot) = ___________? [1] 2Li(s) + 2HCl(aq) → 2LiCl(aq) +…

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Q: 5. Given the following equations and AH values, determine the heat of reaction (kJ) at 298 K for the…

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Q: Aluminum chloride can be formed from its elements: (i) 2Al(s) + 3Cl2(g) ⟶ 2AlCl3(s) ΔH° = ? Use the…

A: Given data, HCl(g)→ HCl(aq)                         ;ΔH°=-74.8kJ      ---1H2 (g) + Cl2 (g) →2HCl(g)…

Q: Given the reactions, X(s)+12O2(g)⟶XO(s)   Δ?=−676.5 kJ XCO3(s)⟶XO(s)+CO2(g)Δ?=+324.9 kJ what is Δ?…

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Q: the

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Q: Given the thermochemical equation 4AlCl3(s) + 3O2(g) → 2Al2O3(s)  +  6Cl2(g); ΔrH= –529 kJ find ΔrH…

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Q: Given the reactions below, calculate ΔHrxn (in kJ/mol) for the reaction of solid carbon with gaseous…

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Q: Calculate  ΔH⁰298   (in kJ) for the process Co3O4(s) → 3 Co(s) + 2 O2(g) from the following…

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Q: The standard enthalpy change for the following reaction is -774 kJ at 298 K. Fe(s) + 5…

A: The standard enthalpy change for the following reaction is -774 kJ at 298 K. Fe(s) + 5…

Q: Given these reactions, where X represents a generic metal or metalloid 1)…

A: Given equations are : H2 (g) + ½ O2 (g) ⟶ H2O (g)        ΔH1 = −241.8 kJ ………(1) X (s) + 2 Cl2 (g) ⟶…

Thermochemistry

Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.    

Exergonic Reaction

The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.