Question
Given the following thermochemical equation:
NO2 (g) + O2 (g) → NO (g) + O3 (g)
ΔH = - 212 kJ
Which has more enthalpy, the reactants
NO2 (g) + O2 (g), or the products NO(g) + O3 (g) ?
The reactants have more enthalpy.
The products have more enthalpy.
The reactants and products have exactly equal enthalpy values.
This cannot be determined with the given information
NO2 (g) + O2 (g) → NO (g) + O3 (g)
ΔH = - 212 kJ
Which has more enthalpy, the reactants
NO2 (g) + O2 (g), or the products NO(g) + O3 (g) ?
The reactants have more enthalpy.
The products have more enthalpy.
The reactants and products have exactly equal enthalpy values.
This cannot be determined with the given information
Answers
Kate
Well look at the value given
a negative enthalpy means that energy was absorbed while a positive enthalpy means that energy was released
take a look at Hess' law
Enthalpy of products - Enthalpy of reactants = -212 kJ
If it's negative then that means the products are at a higher energy state (higher enthalpy) than the reactants
a negative enthalpy means that energy was absorbed while a positive enthalpy means that energy was released
take a look at Hess' law
Enthalpy of products - Enthalpy of reactants = -212 kJ
If it's negative then that means the products are at a higher energy state (higher enthalpy) than the reactants