Burning of fuel in air is called combustion. CH4(g) + 2O2(g)  CO2 (g)+ 2H2O(l) a) Calculate the heat of reaction for the above reaction by using the following bond energies . (3 Marks) C-H single bond is 412 kJ , O=O double bond is 496 kJ, C=O double bond is 743 kJ, H-O single bond is 463 kJ b) Draw the energy profile diagram for the above reaction .On your diagram label the • Products, Reactants • enthalpy for the reaction • activation energy, Ea.

Explanation:

ΔH = ∑ BREAKING BONDS + ∑ GREATING NEW BONDS

  =( 4×412 + 2×496) _ ( 2×743  +  4×463)

 =  2640    KJ             _   3338 KJ       =  - 698 KJ/Mole

exothermic reaction

b) CH4  +  O2 are the reactant

    CO2   +H2O are the product

answer: the value of enthalpy change will be -152.80 kj.

solution:

pressure = 1atm , temperature = = 298 k

given that pressure and temperature are same in both gases , the number of moles of both gases can be determined by the ideal gas equation.

according to reaction 3 moles no are reacting with 1 mol of ,then 0.49 mol of no will react with moles of ozone that is 0.16 moles of ozone. since, no is limiting reagent and is an excessive reagent.

enthalpy change for the reaction between the given volumes of the gases is :

i think it's c. if you look search electronic symbol on google and then click on wiki it shows you a