Final answer:
To find the volume of Oxygen gas required at STP when 25.0g of Zinc Oxide are produced, we can use the ideal gas law. By calculating the number of moles of Zinc Oxide produced and using the stoichiometry of the reaction, we can determine that the number of moles of Oxygen gas required is equal to the number of moles of Zinc Oxide. With this information, we can use the ideal gas law to find the volume of Oxygen gas.
Step-by-step explanation:
This is a stoichiometry problem. Given the mass of Zinc Oxide produced, we need to find the volume of Oxygen gas required at STP. The balanced equation for the reaction is Zn + O₂ → ZnO. From the equation, we can see that 1 mole of Zinc reacts with 1 mole of Oxygen to produce 1 mole of Zinc Oxide. We can use the ideal gas law, PV = nRT, to find the volume of Oxygen.
We first need to find the number of moles of Zinc Oxide produced. The molar mass of Zinc Oxide (ZnO) is 81.38 g/mol. So, the number of moles of Zinc Oxide produced is equal to the mass of Zinc Oxide (25.0 g) divided by its molar mass (81.38 g/mol).
Since the stoichiometry of the reaction is 1:1, the number of moles of Oxygen gas required is also equal to the number of moles of Zinc Oxide produced. We can then use the ideal gas law to find the volume of Oxygen gas, substituting the values for pressure (1 atm), temperature (273 K), number of moles (calculated from the mass of Zinc Oxide), and the ideal gas constant (0.0821 L.atm/mol.K).