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3 cards from this section. Quick, good the night before a test.
Determine if the following reaction is exothermic or endothermic: H₂(g) + ½ O₂(g) → H₂O(l).
Refer to the standard enthalpy of formation values.
Identify the enthalpy of formation for CO₂(g).
Standard formation values should be in reference tables.
What type of reaction occurs if ΔH is negative?
Think about the definitions of exothermic and endothermic reactions.
Do standard enthalpies of formation apply to reactions at any temperature?
Consider what 'standard conditions' means in thermochemistry.
Calculate the enthalpy change for the reaction: 2 H₂(g) + O₂(g) → 2 H₂O(g). Given ΔH_f°[H₂O(g)] = -241.8 kJ/mol.
Use the standard enthalpy of formation for water and apply the equation properly.
Using Hess's Law, determine the enthalpy change for the combustion of 1 mole of C2H6(g) given the following equations: ΔH for C2H6(g) → 2C(s) + 3H2(g) and C(s) + O2(g) → CO2(g) with their respective ΔH values.
Remember to reverse any equations if necessary and change the sign of the enthalpy.
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