Final answer:
The question involves Chemistry at the High School level, where 5.25 g of zinc reacts with sulfuric acid to produce hydrogen gas. The volume of hydrogen produced at STP is calculated using stoichiometry and the molar volume of a gas at STP. The resulting volume is 1.80 liters.
Step-by-step explanation:
The subject of the question is Chemistry, and it falls under High School level. When zinc metal reacts with excess sulfuric acid, hydrogen gas is produced. To calculate the volume of hydrogen at STP (standard temperature and pressure), we use the ideal gas law where the molar volume of an ideal gas at STP is 22.4 liters per mole.
Firstly, we must find the moles of zinc that reacted using its molar mass (65.38 g/mol). Using the given mass of 5.25 g:
5.25 g Zn * (1 mol Zn / 65.38 g Zn) = 0.0803 mol Zn.
Since the stoichiometry of zinc reacting with sulfuric acid to produce hydrogen gas is 1:1, we have 0.0803 mol of hydrogen gas as well. The volume of hydrogen gas produced is then:
0.0803 mol H₂ * (22.4 L/mol) = 1.80 L.
Therefore, the volume of hydrogen generated at STP from the reaction of 5.25 g of zinc metal with excess sulfuric acid is 1.80 liters.