[Abasem098]

I was looking for help to solve this question since i am not good in thermochemistry
*In the reaction : 2H₂O₂ 2H₂O + O₂
ΔH = -196 kJ
What is the change in the enthalpy of the decomposition of 0.34 g of hydrogen peroxide 2H₂O₂                     [ H = 1, O = 16]
+I need to understand what is change in ethalp is. I made an answer but i think it's wrong the only thing i deduced is that number of mole=0.01 mol

[Borek]

ΔH = -196 kJ

Is it how it was given? This is actually not entirely correct - the unit should read a bit different. And once the unit would be right, it would be a strong hint.

[MaleMailMan]

Since the ΔH is associated with a chemical equation, there is no need to write the unit as kJ/mol

2H₂O₂ ---> 2H₂O + O₂    ΔH = -196 kJ

In fact, the ΔH value is actually associated with 2H₂O₂ and if the term mol was to be included, the ΔH would have to be divided by 2.

The solution to the problem:

(-98 kJ/mol) (0.01 mol) = -0.98 kJ