Chemistry 2

Gas Stoichiometry

  1. Just as in every other stoichiometry problem that you have done, they all boil down to knowing some information about one substance so that you can use the mole ratio depicted in the chemical equation to determine some information about another substance.
  2. Try the following examples:
    Given the chemical equation for Butane burning in a lighter:
    2 C4H10(l) + 13 O2(g) ---> 8 CO2(g) + 10 H2O(g)
    1. How many liters of oxygen are needed to combine with 5.00g of butane if the pressure is 1.07atm and the temperature is 25.0°C? 12.8 L
    2. If 2.0L of water are produced at a temperature of 500°C and a pressure of 734 mmHg, then how many grams of butane were burned? 0.35 g