Rewrite the following using a thermochemical equation with a deltaH value: a) The standard molar enthalpy of combustion for propane is -2220kJ/ mol.
What do you mean?
Your post says to rewrite the following using a thermochemical equation but you don't give anything to rewrite. Sorry. Now I see the combustion of propane.
C3H8 + 5O2 ==> 3CO2 + 4H2O dH = -2220 kJ
I have also seen these written as
C3H8 + 5O2 ==>? 3CO2 + 4H2O + 2220 kJ
ok thanks a lot for your help but why did you put a question mark after the > in the equation you gave?
I made a typo.The question mark key is next to the > key and I hit both at the same time.
Ok thanks again for all your help :D
To rewrite the statement using a thermochemical equation with a deltaH value, we can represent the combustion of propane using the following equation:
C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(g) ΔH = -2220 kJ/mol
In this equation, C3H8 represents propane, O2 represents oxygen, CO2 represents carbon dioxide, and H2O represents water vapor. The coefficients in front of each compound indicate the stoichiometric ratio.
The deltaH value (-2220 kJ/mol) represents the heat absorbed or released during the combustion reaction. In this case, the negative sign indicates that the reaction is exothermic, meaning it releases heat.
By using this thermochemical equation, we can calculate the heat released or absorbed if a certain amount of propane is combusted. Just multiply the number of moles of propane used with the deltaH value.
For example, if we combust 2 moles of propane, the heat released would be:
2 moles C3H8 × (-2220 kJ/mol) = -4440 kJ