D. Calculate the enthalpy of dissociation (or bond energy) of the X-X bond. Treat multiplication as consecutive addition for the purpose of sig. figs.

Q: 25. Calculate the standard enthalpy change, AH", for the following reaction: 2CH,OH+ 30 2 CO+4H,0…

A: Calculate standard enthalpy change for the following reaction--

Q: Define the term average bond enthalpy. b) Determine a value for the hydrogenation of propene.

A: Hydrogenation of propene which means enthalpy of hydrogenation of propene. This is calculated using…

Q: Calculate ΔrH° for the combustion of methane gas, CH4 : CH4(g)  +   2 O2(g)  →   CO2(g)  +  2…

A: Given  CH4(g)  +   2 O2(g)  →   CO2(g)  +  2 H2O(g) molecule                                  ΔfH°…

Q: ow.com/ilrn/takeAssignment/takeCovalentActivity.do?locator=Dassignment-take [References] The…

A:

Q: Using the table of bond enthalpies in your textbook, predict ΔrH for the following reaction. Express…

A:

Q: Use the bond energies in table 9.4 on page 396 to determine ΔH for the formation of hydrazine, N2H4,…

A: Given N2(g) + 2 H2(g) ---> N2H4(g) Enthalpy of the reaction is the difference between the energy…

Q: KCl has a lattice energy of −701 kJ/mol. Consider a generic salt, AB, where A2+ has the same radius…

A: The Lattice energy of KCl is given as −701 kJ/mol. It is composed of  K +  and Cl- ions. The given…

Q: 1. Use the bond energy to estimate the heat of reaction at 25 °C for the reaction below. CH¿(g) + 2…

A:

Q: In the reaction: CH4  + 2O2  -->  CO2   +    2H2O Where the bond energies are C-H 414KJ/mol; O-O…

A: The reaction taking place is CH4 + 2 O2 -------> CO2 + 2 H2O

Q: Determine the enthalpy of reaction for P4O10(s) + 6PCI5(g) → 10POCI3(g) Pa(s) + 6CI2(g) → 4PCI3(g)…

A:

Q: (d) Calculate the average bond enthalpy for the N-H bond using the following data: NH₂(g) → NH₂(g) +…

A:

Q: Explain why the bond dissociation energy for bond (a) is lower than the bond dissociation energy for…

A: The energy required to break one mole of bond is termed as the bond dissociation energy. it depends…

Q: Use the bond dissociation energies shown below to estimate ΔH° for the following reaction step:

A: Thus the enthalpy of formation is 22 kcal/mol

Q: Using the equations H2 (g) + F2 (g) → 2 HE (g) AH° = -79.2 kJ/mol C (s) + 2 F2 (g) → CF, (g) AH° =…

A: H2 (g)  +  F2 (g) ----->   2HF (g)  ∆H1° = -79.2 kJ/mol  .................(1) C (s) + 2F2…

Q: The enthalpy change in the hydrogen combustion reaction is H2(g) + O2(g) H2O(1) AH-241.8 kJ/mol.…

A:

Q: Using the equations 2 CHe (1) + 15 O2 (g) → 12 CO2 (g) + 6 H20 (g)AH° = -6271 kJ/mol 2 H2 (g) + O2…

A: The given reactions are,

Q: Judge whether O2- is likely to have larger or smaller dissociation energy than O2.

A: We know that bond dissociation energy and bond order have a direct relationship i.e compound with…

Q: 11. Calculate the enthalpy of reaction (AH). 4CO2 (g) + 6H2O (g) → 2C2H6 (g) + 702 (g) AHfo [CO2(g)]…

A:

Q: Using the equations N2 (g) + O2 (g) → 2 NO (g) AH° = 180.6 kJ/mol N2 (g) + 3 H2 (g) → 2 NH3 (g) AH°…

A: The reactions given are, 1) N2 (g) + O2 (g) ------> 2 NO (g)                      ΔHo = 180.6…

Q: Given that   Δ?∘f[Cl(g)]=121.3 kJ⋅mol−1Δ⁢Hf∘⁡[Cl(g)]=121.3 kJ⋅mol−1     Δ?∘f[C(g)]=716.7…

A: The average molar bond enthalpy is the average amount of energy needed to break the specific bond.

Q: able to calculate energy change for a reaction when bond strengths are given              (ΔG =…

A:

Q: Use the molar bond enthalpy data in the table to estimate the value of Δ?∘rxnΔHrxn° for the equation…

A:

Q: Given that AH: [H(g)] = 218.0 kJ-mol¬1 AH; [C(g)] = 716.7 kJ-mol¬1 AH: [CH_(g)] = –74.6 kJ-mol-1…

A: Average enthalpy can be calculated as follows:

Q: Use the bond energies provided to estimate ΔH°rxn for the reaction below.…

A:

Q: Once it is in the vapor phase, the methanol can react with oxygen in the air according to CH3OH(g) +…

A: The average bond enthalpies are – C-O =358 kJ/mol C-H = 413 kJ/mol O=O = 495 kJ/mol C=O = 805 kJ/mol…

Q: Using the bond enthalpies in Table 8.6 of your textbook, determine the enthalpy change for the…

A: Given: Combustion of Methanol: CH3OH(l) + 1.5 O2 (g) -----> CO2 (g) + 2H2O(g)

Q: (b) Use the bond enthalpies in the table below to calculate a numerical estimate of AH for the…

A: The reactants given are CH4 (g) and F2 (g) and the products given are CH3F (g) and HF (g). Hence the…

Q: Given that   Δ?∘f[H(g)]=218.0 kJ⋅mol−1   Δ?∘f[C(g)]=716.7 kJ⋅mol−1     Δ?∘f[CH4(g)]=−74.6…

A:

Q: so, H,SO, Br2 ON Zn FeBr, HCI(aq) HNO, H,SO,

A:

Q: For the given reaction % H2(g) + % Br:(g) → HBr(g) Molecule Bond energy (kJ/mole) H2 436 Brz 193 HBr…

A: The given chemical reaction is as follows: 12H2(g) + 12Br2(g) → HBr(g) The enthalpy of the reaction…

Q: What is the total bond enthalpy for the molecule CHCI:? The following bond enthalpies, in kJ/mol,…

A:

Q: The incredibly heavy gas uranium hexafluoride, UFe(g), is an intermediate compound in the production…

A: Enthalpy of formation of UF6(g) = -2147 KJ/mol Enthalpy of formation of U(g) = 534 KJ/mol Number of…

Q: Estimate the enthalpy of reaction (in kJ/mol) for the combustion of methane. Be sure to show a lewis…

A:

Q: How can you use a table of bond energies to calculate the Hrxn for any reaction

A: The energy that is mainly required for complete bond's dissociation for the formation of individual…

Q: Explain why the bond dissociation energy for bond (a) is lower than the bond dissociation energy for…

A: The molecules carrying high s-character mainly require high energy for dissociating existing bond.…

Q: Bond Enthalpy (kJ/mol) H―H 436.4 H―O 460 C―H 414 C―C 347 C═C 620 C―O 351 O―O 142 O═O…

A:

Q: Given that: A(s) + B2(g) – AB2(g) AH = -242.3 kJ/mol A(s) + 3/2 B2(g) →AB3(g) AH = -319.1 kJ/mol…

A:

Q: In 1998 scientists using a special type of electron microscope were able to measure the force needed…

A: Given : Force required to break C-Si bond = 2.0 X 10-9 N And the distance to which the should be…

Q: Use the average bond enthalpies in the table to estimate AH for the combustion of propanc based on…

A: The answer to the following question is-

Q: Methanal can be made through the partial oxidation of methane using O2 in the presence of a…

A: The reaction taking place is given as, => CH4 (g) + O2 (g) ------> CH2O (g) + H2O (g)

Q: a Estimate the value of AH° for the following reaction from bond enthalpies using the data below. H2…

A: 539 kJ

Q: I need a prediction based on the chart.

A: Given reaction: 2C2H6 (g) + 7O2 (g) -----> 4CO2 (g) + 6H2O (g) To determine: Total Enthalpy of…

Q: Hydrogenation of double and triple bonds is an important industrial process. Calculate (in kJ) the…

A: Introduction-  To determine the  standard enthalpy change ΔH° (  in KJ ) for the hydrogenation of…

Q: From the following data, calculate the average bond enthalpy for the N-H bond. NH3(g) NH2(g) + H(g)…

A:

Q: How much energy is required to break the bonds in the molecule of NO, BCl3, and NO2?  and How do I…

A: By the estimate of the enthalpy of reaction by looking at the individual bonds involved. If we know…

Q: Explain why the bond dissociation energy for bond (a) is lower than the bond dissociation energy for…

A:

Q: How can bond energies be used to estimate ∆H for a reaction?

A: Bond energy:- It is defined only for gaseous molecules. So, enthalpy change during the breaking of 1…

Q: Use bond energies from the table to estimate ΔrH for the following reaction. C2H2(g)+H2(g)→C2H4(g)…

A:

Q: If hydrogen were used as a fuel, it could be burned according to this reaction: H2(g) + 1/2 O2(g)…

A: Solution -  TheΔHreaction = -243 kJ/mol ΔHreaction CH4(methane) = -802 = kJ/mol The fuel yields…

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.