How much energy is required to break all of the bonds in 5.75g of H2O (g)?

Q: The enthalpy of formation of XeF2(g) is -108 kJ/mol and the bond dissociation enthalpy of the F-F…

A: We have to calculate the average bond dissociation enthalpy of Xe-F bond

Q: Calculate the heat of reaction for 40.0 mL of 0.400 M HCl with 40.0 mL of 0.100 M Ba(OH)2 with a…

A: VHCl= 40ml = 0.040 L MHCl= 0.400 M VBa(OH)2= 40ml = 0.040 L MBa(OH)2= 0.400 M Lets assume the…

Q: The energy diagram shown represents the chemical reaction between solid ammonium chloride and solid…

A: Reaction given 2NH4Cl(s) +Ba(OH)2 ⋅8H2O(s)→2NH3 (aq) +BaCl2 (aq) +10H2O(l) ∆H(reaction) = 54.8 kJ…

Q: 12. Estimate the enthalpy change for the reaction 2CO + O2 →2CO2 given the following bond energies.…

A: The chemical reaction :  2CO + O2  -----> 2CO2   The binding energy of :   C≡O = 1074 KJ/mol. O=O…

Q: How much energy (kJ) is released when 3.50 moles of O2(g) react with iron?

A:

Q: How much heat is produced by the combustion of 4.67g of magnesium (24.30 g/mol)? Mg(s) + 1/2 O2(g)…

A: Here we have to apply mole concept, first we need to find for 1 gram Mg combustion how much energy…

Q: How much heat is produced by burning 4.00 moles of acetylene under standard state conditions?

A: Moles of acetylene= 4

Q: Consider the reaction of carbon and hydrogen. Draw the covalent bonds that would form to produce a…

A:

Q: how many grams of this compound must you burn to release 997.40 kJ997.40 kJ of heat?

A: Given :-  Heat of combustion of a compound = -1030.0 kJ/mol  Molar mass of compound = 72.51 g/mol…

Q: Write the law for this reaction and explain how it is determined SO2CL2 ->SO2 + CL2

A:

Q: Use the bond energies provided to estimate the mass of O₂(g) required to produce 1,023 kJ of energy.…

A: Amount of O2 required to produce 1023 kJ of energy is to be calculated.

Q: If the heat of combustion for a specific compound is −1370.0 kJ/mol and its molar mass is 47.85…

A: Given, Heat of combustion for specific compound , Q= -1370 kJmol Molar mass, M = 47.85 gmol Required…

Q: iven the data below, calculate the enthalpy of reaction (in units of kJ) for the reaction:  2 C2H2…

A: Enthalpy of a reaction = Sum of enthalpies of products – Sum of enthalpies of reactants

Q: Compound X and Y are being tested for their capacity as insulators. a. In the first experiment,…

A: a.The amount of heat transferred from heated compound X to water bath is first determined first then…

Q: After writing and balancing the equation, what is the next step in using bond energies to calculate…

A: Bond energies of the reactants and products can be used to calculate the enthalpy of the reaction:…

Q: How much energy is absorbed during the complete reaction of 3.00 kg carbon (MW = 12.01 g/mol) given…

A: Mole=Weight of substance/Molar mass of substance

Q: The heat of combustion of methane is 212.8 kcal per mole. How much heat will be produced in the…

A:

Q: (C) Balance this reaction. Then use the bond enthapies given in the table below to calculate the…

A: The reaction taking place is  C3H4 + O2  ----> CO2 + H2O Since in the above reaction we have 3 C…

Q: What is the enthalpy change if 45.0 g of CaO is allowed to react with an excess of carbon?

A: The standard enthalpy for a given reaction can be called as the enthalpy change for a given…

Q: Which one of the following statements is not true concerning the equation below? N2(g) + 3 H2(g) → 2…

A: Since, heat is released in this reaction so this is an exothermic reaction. And mol ratio of N2 and…

Q: Fe2O3(s) + 3CO(s) → 2Fe(s) + 3CO2(g) ΔH = -28.0 kJ 3Fe(s) + 4CO2(s) → Fe3O4(s) + 4CO(g) ΔH = +12.5…

A: Enthalpy of reaction 1 -  ∆H = -28.0 KJ  Enthalpy of reaction 2 -  ∆H = +12.5 KJ  Enthalpy for final…

Q: For the reaction H2(g) + 1/2 O2(g) --> H2O(g), DHo = -241.8 kJ. What quantity of heat, in kJ,…

A: Balanced Reaction H2(g) + 1/2 O2(g) --> H2O(g) Here heat is released during the reaction.

Q: The energy diagram shown represents the chemical reaction between solid ammonium chloride and solid…

A: Given, 2NH4Cl(s) + Ba(OH)2⋅8H2O(s) → 2NH3(aq) + BaCl2(aq) +10H2O(l)   ∆H = 54.8 kJ mass of NH4Cl…

Q: 7. Calculate the number of grams of CO2 that are produced by heating 116.4 grams of magnesium…

A: 60.72 gram of CO2 is produced from 116.4 gram of MgCO3.

Q: It is interesting to compare the “fuel value” of a hydrocarbonin a hypothetical world where oxygen…

A: If we have to find which reaction is more exothermic we can do it by finding the deltaH value for…

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: Consider these reactions: Reaction 1: H2(g)+Cl2(g)⟶2HCl(g)ΔH=−184.6 kJ Reaction 2:…

A:

Q: Consider the following reaction: 2H2 + O2--> 2H2O Hrxn= -483.6 kj/mol  a. is this reaction…

A: The given reaction is shown below.

Q: Tow many kilojoules of energy will be needed to decompose 10.8 g of N205 gas? N205 (g) + 110 kJ-> 4…

A:

Q: CH4(g) + 4Cl2(g) → CCl4(g) + 4HCl(g), ΔH = –434 kJ Based on the above reaction, what energy change…

A:

Q: The energy produced (-286 kJ/mol) in the reaction H₂ and O₂ comes from: A) Breaking the H-H and O=O…

A: The reactions are of two types Exothermic and endothermic,  in exothermic reactions heat is released…

Q: 12. Consider the following process. + 2H,O(e) AH = -802 kJ %3D CH4 (8) + 202 (8) 2 CO2 (8) A) Is the…

A: We have to predict the change in enthalpy and it's nature.

Q: Use the bond energies in the table to estimate the enthalpy of reaction for the oxidation of…

A:

Q: 2NO2 (g) ↔ N2O4 (g) 30 mL of NO2 gas is compressed in a syringe to 15 mL. Is this reaction…

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.