Consider the following thermochemical data: Cl2(g) → 2CI(g) AH° = 242.3 kJ l2(g) → 21(g) AH° = 151.0 kJ IC(g) → 1(g) + Cl(g) AH° = 211.3 kJ l2(s) → 12(g) AH° = 62.8 kJ Calculate AH° for the following reaction: ½l2(s) + ½CI2(g) → ICI(g)

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: When one mole of calcium carbonate reacts with ammonia, solid calcium cyanamide, CaCN2, and liquid…

A: To solve this problem first we have to write the balanced chemical equation then we will calculate…

Q: Find the standard enthalpy of formation of ethylene, C2H4(g), given the following data: C2H4(g) + 3…

A: Answer:Properties that depend on the size of the system are called extensive properties. They are…

Q: Given the thermal chemical reactions below Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g) ∆H°= −26.7 kJ…

A: Enthalpy measures  the heat content of a system. If change of enthalpy is positive then the reaction…

Q: Calculate ΔH° for the combustion of methane. CH4 (g) + 2 O2 (g) → CO2 (g) + 2 H2O (g) Given the…

A: We have to calculate the ∆H° for Reaction.

Q: Given the following combustion data for three different fuels: CH4 (g), C8H18 (l) and CH3OH (l), CH4…

A: The ratio of energy to the molar mass is known as energy density.

Q: Find the ΔH (in kJ) for the reaction: PCl3(l)  +  Cl2(g)  →  PCl5(s)   Given: 2 P (s)  +  3…

A: According to hess’s law :- When reactants are converted to products the chage in enthalpy is same…

Q: Top fuel dragsters and funny cars burn nitromethane (CH3NO2) as fuel according to the following…

A: The objective of this question is to calculate the standard enthalpy of formation, ΔfH°, for…

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

A:

Q: Use the information provided to determine ΔH°rxn for the following reaction: 3 A(s) + B(g) → 2 X(s)…

A: The standard enthalpy of the given reaction is calculated is follows :

Q: Calculate ΔHrxn for the following reaction: CaO(s)+CO2(g)→CaCO3(s) Use the following reactions and…

A: "Hess law" helps in the evaluation of enthalpy change (Delta H)  for any specific reaction. When the…

Q: Determine the amount of heat (in kJ) associated with the production of 5.91 x 10 g of ammonia…

A:

Q: Using the equations 2 H, (g) + O, (g)→ 2 H,O (1) AH° = -572 kJ/mol Ca (s) + ½ Ô, (g) → CaO (s) AH° =…

A:

Q: How much energy in kJ is released in burning 2.83 mL of gasoline (assuming that all of it is octane…

A:

Q: How much energy in kJ is released in burning 2.87 mL of gasoline (assuming that all of it is octane…

A:

Q: Given the following combustion data for three different fuels: CH4 (g), C8H18 (l) and CH3OH (l),…

A: For fuel CH4 energy per gram is  CH4 (g) + 2 O2 (g) → CO2 (g) + 2 H2O (l) ΔH° = −890 kJenergy per…

Q: Given the following thermochemical equations, 4NH3(g) + 702(g) → 4NO2(g) + 6H2O(g) 6NO2(g) + 8NH3(g)…

A: The enthalpy change is a state function and the Hess law states that the change of enthalpy in a…

Q: Given the standard enthalpy changes for the following two reactions: (1) 2Pb(s) + O2(g)2PBO(s) AH° =…

A: Given that -  (1) 2Pb(s) + O2(g) ----> 2PbO(s) , ∆H°1 = -434.6 kJ    (2) Pb(s) + Cl2(g) ---->…

Q: For the following reactions identify if they are exothermic or endothermic.    2NO2 → 2NO + O2 ΔH =…

A: The heat energy shift (∆H) that occurs when reactants become products is known as enthalpy of the…

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

A: Given  SrO(s)  +  CO2(g)   →   SrCO3(s)                     ∆H°   = -234 KJ/mol…

Q: Suppose 23.00 g ammonium chloride (53.491 g/mol) dissolves in water in a calorimeter to form 100.00…

A: Given,Mass of ammonium chloride ( NH4Cl ) =23.00 gMolar mass of ammonium chloride ( NH4Cl ) =53.491…

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

A:

Q: Using the equations 2 Sr(s) + O₂ (g) → 2 SrO (s) ∆H° = -1184 kJ/mol SrO (s) + CO₂ (g) → SrCO₃ (s)…

A: The given reactions given are as follows: The required equation is:

Q: A 1.00 g sample of MgCl2 produced a 10.00 °C increased in a calorimeter charged with 40.0mL of…

A: Mass of MgCl2 = 1.00 g Increase in temperature, ΔT = 10.00 °C Specific heat of MgCl2, C = 0.750…

Q: When one mole of calcium carbonate reacts with ammonia, solid calcium cyanamide, CaCN2, and liquid…

A: Enthalpy of reaction , ΔH can be calculated as : ΔH =  Sum of Enthalpy of formation of product - Sum…

Q: Given the following data, calculate ΔH for the reaction of two moles of carbon monoxide with oxygen…

A: The indirect calculation of enthalpy change by use of several reactions with known enthalpies is…

Q: How many moles of hydrogen is consumed when 288 kJ of energy is released from the complete…

A: From stoichiometric calculations, we will calculate the moles of hydrogen consumed when 288 KJ of…

Q: How much energy in kJ is released in burning 2.5 mL of gasoline (assuming that all of it is octane…

A: To solve this problem first we have to calculate the mole of octane by using its volume, density and…

Q: se the standard reaction enthalpies given below to determine Hᵒrn for the ollowing reaction: ven: 2…

A: Which one of the following is correct answer

Q: Use the data given below to find the enthalpy of reaction for the following reaction: CaCO3(s) →…

A:

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.