what volume of hydrogen gas at STP can be produced by reacting 15.0 grams of uluminum with sulfuric acid? the equation is: 2Al+ 3H2SO4---> Al2(SO4)3+ 3H2
Follow these steps.
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To find the volume of hydrogen gas produced, we need to use the stoichiometry of the balanced chemical equation and the ideal gas law.
Step 1: Calculate the number of moles of aluminum (Al) in 15.0 grams.
To do this, we divide the mass of aluminum by its molar mass.
Molar mass of Al = 26.98 g/mol
Number of moles of Al = mass of Al / molar mass of Al
Number of moles of Al = 15.0 g / 26.98 g/mol
Step 2: Use the stoichiometry of the balanced equation to find the number of moles of hydrogen gas (H2) produced.
From the balanced equation: 2Al + 3H2SO4 → Al2(SO4)3 + 3H2
We can see that 2 moles of Al react to produce 3 moles of H2.
Number of moles of H2 = (Number of moles of Al) × (3 moles of H2 / 2 moles of Al)
Step 3: Calculate the volume of hydrogen gas at STP (Standard Temperature and Pressure).
At STP, 1 mole of ideal gas occupies 22.4 liters.
Volume of H2 gas at STP = (Number of moles of H2) × (22.4 liters / 1 mole)
By substituting the values we calculated in the previous steps, we can find the answer.