5.5: Enthalpy Changes of Chemcial Reactions
- Page ID
- 167655
Endothermic or Exothermic Reactions
Exercise \(\PageIndex{1}\)
Decide whether each of these reactions is exothermic or endothermic:
- When two chemicals mix their temperature rises
- A solid burns brightly and releases heat, light and sound
- When two chemicals are mixed their temperatures drops
- Two chemicals will only react if you heat them continually
- Plants take in light energy for photosynthesis
- Answer
-
- exothermic
- exothermic
- endothermic
- endothermic
- endothermic
Enthalpy Change per Mole
Exercise \(\PageIndex{2}\)
What quantity, in moles, of hydrogen is consumed when 185.6 kJ of energy is evolved from the combustion of a mixture of H2(g) and O2(g)?
H2(g) + O2(g) → H2O(l); ΔrH° = –285.8 kJ/mol-rxn
- Answer
-
0.6494 moles
\(\frac{185.6 kJ}{285.8 kJ/mol} = 0.649405 moles\)
Exercise \(\PageIndex{3}\)
The following reaction of iron oxide with aluminum is an exothermic reaction.
Fe2O3(s) + 2 Al(s) → 2 Fe(s) + Al2O3(s)
The reaction of 7.50 g of Fe2O3 with excess Al(s) evolves 31.5 kJ of energy in the form of heat. Calculate the enthalpy change per mole of Fe2O3.
- Answer
-
-6.71*102 kJ*mol-1 (heat evolved, negative sign)
Exercise \(\PageIndex{4}\)
How much heat is liberated at constant pressure if 0.675 g of calcium carbonate reacts with 45.1 mL of 0.498 M hydrochloric acid?
CaCO3(s) + 2HCl(aq) → CaCl2(aq) + H2O(l) + CO2(g); ΔrH° = –15.2 kJ/mol-rxn
- Answer
-
ΔH = -0.103 kJ