How much energy is evolved during the formation of 120 g of Fe, according to the reaction below?     Fe2O3(s) + 2 Al(s) → Al2O3(s) + 2 Fe(s) ΔH°rxn = -852 kJ

Q: How much energy is released during the formation of 98.7 g of Fe according to the reaction below?…

A: Given reaction is :  Fe2O3 (s) + 2Al (s) ----> Al2O3 (s) + 2Fe (s) , ΔHrxn = -852 KJ/mole  How…

Q: The standard enthalpy change for the following reaction is -822 kJ at 298 K.2 Na(s) + Cl2(g)    2…

A:

Q: Calculate the enthalpy of reaction (ΔHrxn), in kJ, for the following reaction: Fe2O3(s) + 3 CO(g) →…

A: According to Hess's law change of enthalpy in a chemical reaction is same regardless of whether the…

Q: How much energy is evolved during the formation of 102 g of Al2O3, according to the reaction…

A: Given, the heat evolved in the reaction is -852kJ.

Q: Consider the following chemical reaction which produces HCI from its constituent elements: H2 (g) +…

A: The correct option with explanation is provided in the next step:

Q: 3. Consider the following two reactions:                         A → 2B           ΔH0rxn = 456.7…

A: A → 2B ; ΔH°rxn = 456.7 kJ/mol                    .......(1) A → C   ; ΔH°rxn = -22.1 kJ/mol…

Q: The enthalpy change for the reaction of hydrogen gas with fluorine gas to produce hydrogen fluoride…

A:

Q: Sand is converted to pure silicon in a three step process. The third step is   SiCl4(g) + 2Mg(s) →…

A: Given:SiCl4(g)  + 2Mg(s) → 2MgCl(s)  + Si(s)        ΔH  = –625.6 kJ

Q: Calculate ΔH (in kJ/mol) for the reaction shown below: ClF(g)+F2(g)→ClF3(g) Use the following…

A:

Q: Given: 4 NH3 (g) + 3 O2 (g) → 2 N2 (g) + 6 H2O (l) ΔH = -1500 kJ How many grams of ammonia (MM =…

A: As per the given balanced chemical equation, 4 moles of ammonia react to release 1500 kJ of heat.

Q: Balance the following reactions, calculate [delta]Hrxn, calculate the energy released (or required)…

A:

Q: $ A chemist measures the enthalpy change AH during the following reaction: 3 CH₂ Br(g) +…

A: The thermochemical equations can be treated as algebraic equation which can be added,  subtracted,…

Q: How much heat is released when a 0.79 g magnesium ribbon is burned

A: given, mass of Mg = 0.79 g molar mass of Mg = 24.305 g/mol number of moles of Mg = given mass of Mg…

Q: How much energy is evolved during the formation of 296 g of Fe, according to the reaction below?…

A:

Q: The standard enthalpy change for the following reaction is -479 kJ at 298 K.

A: 1) Heat energy change at constant temperature and pressure is called enthalpy change (or) Heat of a…

Q: Determine the enthalpy of reaction for HCI(g) + NANO2(s) → HNO2(1) + NaCI(s) 2NACI(s) + H2O(1) →…

A:

Q: Calculate ΔH for the following reaction, CaO(s) + CO2(g) → CaCO3(s) given the thermochemical…

A: The given problem relates to Hess's law, which states that the amount of heat evolved or absorbed in…

Q: The standard enthalpy change for the following reaction is -576 kJ at 298 K. 2 Na(s) + I2(s) –→ 2…

A: Given,

Q: The combustion of 0.1559 g benzoic acid increases the temperature of a bomb calorimeter by 2.52°C.…

A:

Q: Calculate the enthalpy change for the reaction: 2 H2O2(l) → 2 H2O(l) + O2(g)2 H2O2(l) → 2 H2O(l) +…

A: Given, 2H2O2(l) → 2H2O(l) + O2(g) Enthalpy change for the reaction (∆H°rxn) = ? Species enthalpy…

Q: When 1.42 g of iron reacts with 1.80 g of chlorine, 3.22 g of FeCl2(s) and 8.60 kJ of heat is…

A: Iron reacts with chlorine to form iron(II) chloride. When 3.22 g of FeCl2s is formed, 8.60 kJ of…

Q: Part A. In the late eighteenth century Priestley prepared ammonia by reacting HNO3(g) with hydrogen…

A: HNO3(g) + 4H2(g) → NH3(g) + 3H2O(g) ΔH = –637 kJ From this data we get that , When 4 mole Hydrogen…

Q: Given the following reactions: 2S(s) + 3O2(g) → 2SO3(g)                 ΔH = -790 kJ S(s) + O2(g)…

A: Hess's law is defined as amount of energy released or absorbed is same wheather the reaction take…

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.