Calculate ΔH° for the reaction 2 C4H10 (g) + 13 O2 (g) → 10 H2O(g) + 8 CO2 (g) using the following information:

Q: 1. Use the given information to calculate the enthalpy of reaction for the following reaction: P,O10…

A: Here we have to calculate change of enthalpy of above given reaction-

Q: Determine ΔH for the third reaction from the information given. S(s) + O2(g) ↔ SO2(g) ΔH = -296.1…

A: Given;

Q: Using the equations Sro (s) + CO, (g) → SrCO, (s) AH° = -234 kJ/mol 2 Sr(s) + O, (g) → 2 SrO (š) AH°…

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Q: Use the given average bond energy values to estimate ΔH for the following reaction in the gas phase.…

A: Answer: Enthalpy of the reaction is actually the difference between the bond energies of reactants…

Q: 2.045 g of a new compound with formula C9H8O2 is burned in a bomb calorimeter.  During the…

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Q: The reaction 2 Ti (s) + 3 I2 (g) –→2 Til3 (s) having AH = -839 kJ/mol is: (a) endothermic and, thus,…

A: Given, Chemical Reaction  2 Ti (s) + 3 I2(g) ---> 2 TiI3(s)  Change in enthalpy , ∆H = - 839…

Q: Calculate: C(graphite) + O2(g) → CO2(g) ΔH° = -393.5 kJ H2(g) + ½O2(g) → H2O(l) ΔH° = -285.8 kJ…

A: the solution of the problem can be solved by using kirchhoff's equation.

Q: whats the chemical equation defined as ∆Hof for H2O (l)

A: Formation reactions are the chemical reactions that form one mole of a substance from its…

Q: Given the following reaction: CO(g) + O(g) →→→→CO₂(g) AH,º=? Calculate the enthalpy of reaction…

A: We have to calculate the enthalpy of reaction given the following enthalpies of formation

Q: Consider the following thermochemical data to: 2CO2(g) → 2 C (s, graphite) + 2 O2 (g) H2 (g) +…

A: Given  Equation No Reaction.                       ∆H°(kJ/mol) A 2CO2 (g) → 2 C (s, graphite)…

Q: Determine ΔrH° in kJ/mol for the reaction,  4 NO(g) + 6 H2O(g) →4 NH3(g) + 5 O2(g) using the…

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Q: Energy is released when hydrogen and oxygen react to produce water. This energy comes  from the fact…

A: Given question is related to the calculation of amount of energy released when one mole of water is…

Q: The meals-ready-to-eat (MREs) in the military can be heated on a flameless heater. You can purchase…

A: Recall the given reaction,                            Mg s  +  2 H2O l  →  MgOH2 s  +  H2 g45 mL…

Q: Calculate the standard enthalpy of the reaction for the process 3RO(g) → R20(g) + RO2(g) using the…

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Q: Given that the enthalpy of neutralization for the reaction of HCl (a strong acid) and NaOH (a strong…

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Q: Calculate the ΔH°298 for the reaction CH4(g) + 2O2(g) → CO2(g) + 2H2O(l). Given the following…

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Q: The meals-ready-to-eat (MREs) in the military can be heated on a flameless heater. You can purchase…

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Q: Enthalpy change for the final reaction = (2*1.638 kJ) - (3.0225 kJ) = 0.2535 kJ 1. Comment on why…

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Q: Given the standard enthalpy changes for the reactions: Pals) + 302(8) → PaO6[s) AH° = -1640 kJ/mol…

A: Equation 1: P4(s) + 3O2(g) → P4O6(s)    ∆H° = - 1640 KJ/mol  Equation 2: P4(s) + 5O2(g)→ P4O10(s)…

Q: Use average bond enthalpies (look in intstructor add-ons) to calculate the enthalpy change (in kJ)…

A: 3) Given, CH4(g) + 2O2(g) → CO2(g) + 2H2O(g) Enthalpy change for the reaction (∆Hrxn) = ? Note: bond…

Q: Consider the following reaction: 3 C(s) + 4 H₂(g) → C3H8(g) Which of the following statements is…

A: The spontaneous nature of a system can also be predicted by the Gibbs free energy change of the…

Q: reaction. Use the Standard Enthalpies of Formation in your textbook to determine the AH° for the…

A: From the standard enthalpy of formation data  ∆Hf for CO2 is -393.51 kJ  ∆Hf for NaCl is -407.25 kJ…

Q: Determine ΔrH° in kJ/mol for the reaction,  4 NO(g) + 6 H2O(g) →4 NH3(g) + 5 O2(g) using the…

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Q: 17. The enthalpy of formation for H20(g), CO2(g), and C2H5OH(1), in kJ/mol, are given as follows…

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Q: ammonia

A: Dear student I have given answer to your question in the image format.

Q: Use the given standard enthalpies of formation to calculate the ΔHo (in kJ) for the hypothetical…

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Q: Calculate ΔH (in kJ/mol) for the reaction described by the equation. 6 NH3(g) + 5 O3(g) → 6 NO(g) +…

A: Tha delta H represents the enthalpy change during the reaction. Now if the enthalpy change is…

Q: ) of the following reaction: ?

A: ∆H°formation for pure substance at room temperature value is Zero . Here C(graphite) and Hydrogen…

Q: Calculate AH for the reaction NH3 (g) + CH4 (g) → HCN (g) + 3 H, (g), from the following data. N2…

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Q: Determine the enthalpy of reaction for HCI(g) + NaNO2(s) -> HNO2 (l) + NaCl(s) 2NaCl(s) + H2O(l) →…

A: Given data 2NaCl(s) + H2O(l) → 2HCI(g) + Na2O(s); ∆H ° =-507.1 kJ/mol NO(g) + NO2(g) + Na2O(s)→…

Q: formation

A: Standard change in enthalpy of the Reaction formula is :  ∆H°rxn = [ ∆H°(product) ] - […

Q: Hydrobromic acid (HBr) is a commonly used acid for adding bromine to organic compounds. As bromine…

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Q: Determine the enthalpy of reaction for HCl(g) + NaNO₂(s) → HNO₂(l) + NaCl(s) 2NaCl(s) + H₂O(l) →…

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Q: 1. Calculate the heat evolved when 13.56g of oxygen gas (O2) is used to burn  white phosphorus at…

A: 1) Given, P4(s) + 5O2(g) → P4O10(s), ΔH = -3013 kJ/mol ∆H is in negative (-) which indicate the…

Q: 6. Enthalpies of Formation: A common experiment in industrial chemistry application is when Ethanol…

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Q: Determine the enthalpy (in kJ/mol) for the reaction 3 SiCl₄ (s) + 4 Fe (s) → 4 FeCl₃ (s) + 3 Si (s)…

A: To solve this we have to do some  mathematical operations with the given  two equations to get the…

Q: The following reaction is classified as and CHĄ(g) + 202(g) CO2(9) + 2H2O(g) exothermic reaction

A: The correct answer about reaction types is given below

Q: Calculate total work done (in Joules) when 50 g of iron is dissolved in HCl in an open beaker at…

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Q: According to the following reaction, how much energy is evolved during the reaction of 53.2 g Fe2O3…

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Q: Which of the following compounds has the standard formation of free energy Δ G°f = 0? C (g) O (g)…

A: The element which is in its standard state has ∆G°f equals to zero.

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.