Answer: Th enthalpy of combustion for the given reaction is 594.244 kJ/mol
Explanation: Enthalpy of combustion is defined as the decomposition of a substance in the presence of oxygen gas.
W are given a chemical reaction:
[tex]Mg(s)+\frac{1}{2}O_2(g)\rightarrow MgO(s)[/tex]
[tex]c=5760J/^oC[/tex]
[tex]\Delta T=0.570^oC[/tex]
To calculate the enthalpy change, we use the formula:
[tex]\Delta H=c\Delta T\\\\\Delta H=5760J/^oC\times 0.570^oC=3283.2J[/tex]
This is the amount of energy released when 0.1326 grams of sample was burned.
So, energy released when 1 gram of sample was burned is = [tex]\frac{3283.2J}{0.1326g}=24760.181J/g[/tex]
Energy 1 mole of magnesium is being combusted, so to calculate the energy released when 1 mole of magnesium ( that is 24 g/mol of magnesium) is being combusted will be:
[tex]\Delta H=24760.181J/g\times 24g/mol\\\\\Delta H=594244.3J/mol\\\\\Delta H=594.244kJ/mol[/tex]
