10.5: Stoichiometry and the Ideal Gas Law
Many reactions that are carried out in the laboratory involve the formation or reaction of a gas, so chemists must be able to quantitatively treat gaseous products and reactants as readily as
Writing balanced equations for some redox reactions that occur in aqueous solutions is simplified by using a systematic approach called the half-reaction method. A balanced chemical equation may be used to describe a reaction's stoichiometry (the relationships between amounts of reactants and products).
Note that the balanced chemical equation states that 483.6 kJ of energy is released per two mol hydrogen used up: Second, determine the amount of heat that can be released by burning the 10.0 g oxygen in excess hydrogen. Note that the balanced chemical equation states that 483.6 kJ of energy is released per one mol oxygen used up:
That is, we can now add an energy amount to the equivalences — the enthalpy change of a balanced chemical reaction. This equivalence can also be used to construct conversion factors so that we can relate enthalpy change to amounts of substances reacted or produced. Note that these equivalences address a concern.
The balanced thermochemical equation relates the energy change to moles, not grams, so we first convert the amount of N 2 to moles and then use the thermochemical equation to determine the energy change: Determine how much heat is given off when 1.00 g of H 2 reacts in the following thermochemical equation: −15.1 kJ
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