A 0.152mol sample of CH2O2 reacted completely according to the reaction shown and 38.7 kJ of heat was released. What is delta H for this reaction?

Question

2CH2O2+O2---->2CO2+2H2O

can someone please explain.

Answer 1

2CH₂O₂ + O₂ --> 2CO₂ + 2H₂O

The ∆H for the reaction is based on the moles of reactants and products in the balanced equation. So, in this case, it will be the heat associated with the combustion of TWO moles of CH₂O₂. We are given the heat associated with combustion of 0.152 moles. So, it is a simple matter to do the conversion.

38.7 kJ/0.152 moles CH₂O₂ x 2 mol CH₂O₂ = 509 kJ = ∆Hrxn