Calculate the enthalpy of reaction for the decomposition of FBr (reaction shown below) using the bond energies provided in the table.2 FBr(g)  -->  F2(g)  +  Br2(g)Question 29Answer-127 kJ mol-1+127 kJ mol-1+110 kJ mol-1-110 kJ mol-1+320 kJ mol-1

Which of the following correctly represents reaction for estimating standard enthalpy of formation of HBr?

Given the following bond dissociation energies, calculated the enthalpy of the following reaction.CH4 + 2F2 → CF4 + 2H2Hint: You might need to draw Lewis Dot Structures for each of these before you can count the bonds on the reactant and product sides.C-F            450 kJ/molC-H            410 kJ/molF-F            158 kJ/molH-H            436 kJ/molGroup of answer choices318 kJ-716 kJ-318 kJ716 kJ

Given the following bond dissociation energies, calculated the enthalpy of the following reaction.H-C≡C-H + 2H2 → H3C-CH3C-C            350 kJ/molC≡C           807 kJ/molC-H            410 kJ/molH-H            436 kJ/molHint: There are 2 H-H bonds on the left and a total of 6 C-H bonds on the right.Group of answer choices-111 kJ/mol-211 kJ/mol-311 kJ/mol-11 kJ/mol

Calculate the heat of reaction ΔH for the following reaction:H2(g)+  Cl2(g)→2HCl(g)You can find a table of bond energies by using the Data button on the ALEKS toolbar.Round your answer to the nearest /kJmol.

The bond enthalpies for six selected chemical bonds are shown below.Bond Bond enthalpyΔH°298 (kJ/mol)H―H 436C―H 413C=O 532N―H 335O―H 499O=O 495For a reaction in which 2 moles of H2(g) reacts with 1 mole of O2(g) to form 2 moles of H2O(g), what is the heat of the reaction?A.1367 kJB.369 kJC.−629 kJD.−1996 kJ