Final answer:
By calculating the conversion of 5.29 kg of ammonium perchlorate to moles and using the stoichiometry from the balanced chemical equation for its decomposition, it is determined that 180.08 moles of gases are produced.
Step-by-step explanation:
To determine how many moles of gases are produced by the reaction of 5.29 kg of ammonium perchlorate, NH4ClO4, one would need both the molar mass of ammonium perchlorate and the balanced chemical equation of the reaction where it decomposes. If the reaction is the thermal decomposition of ammonium perchlorate, the reaction it undergoes is typically:
2 NH4ClO4 (s) → 2 N2 (g) + 4 H2O (g) + O2 (g) + 2 Cl2 (g)
First, we convert 5.29 kilograms to moles by dividing it by the molar mass of NH4ClO4, which is 117.5 g/mol:
(5.29 kg) * (1000 g/kg) / (117.5 g/mol) = 45.02 moles of NH4ClO4
According to the balanced equation, every 2 moles of NH4ClO4 produce a total of 8 moles of gas (2 moles of N2, 4 moles of H2O, and 2 moles of Cl2). Thus, we use the mole ratio to find the total moles of gas produced:
(45.02 moles NH4ClO4 / 2 moles NH4ClO4) * 8 moles of gas = 180.08 moles of gas
This result assumes the gases are at standard temperature and pressure conditions and that the reaction goes to completion.