10cm of propane was sparked with 60cm3 of oxygen at s.t.p what is the volume of residual gas after the reaction is cooled
The reaction that occurs when propane is burned in oxygen is given by the following balanced chemical equation:
C₃H₈ + 5O₂ → 3CO₂ + 4H₂O
10 cm³ of propane (C₃H₈) is reacted with 60 cm³ of oxygen (O₂). According to the stoichiometry of the reaction, one mole of propane reacts with 5 moles of oxygen. To find the limiting reactant, we need to compare the ratios of the given volumes to the stoichiometric ratios:
The ratio for propane: (10 cm³) / (1 mole) = 10 cm³/mole
The ratio for oxygen: (60 cm³) / (5 moles) = 12 cm³/mole
The ratio for propane is smaller, so propane is the limiting reactant. Since the reactants are gaseous, we can use the relationship between volumes and moles at constant pressure and temperature:
(Volume of propane / volume of oxygen) = (1 mole / 5 moles)
So, we can find the volume of oxygen consumed during the reaction:
Volume of oxygen consumed = 10 cm³ × (5 moles / 1 mole) = 50 cm³.
Now, we can find the volume of residual oxygen:
Volume of residual oxygen = initial volume of oxygen - volume of oxygen consumed = 60 cm³ - 50 cm³ = 10 cm³.
Since the volume of propane is completely consumed and only oxygen is left as a residual gas, the volume of residual gas after the reaction is:
Volume of residual gas = volume of residual oxygen = 10 cm³.