Sulfuric acid dissolves aluminum metal according to the following reaction:
2Al(s) + 3H2SO4(aq) -> Al2(SO4)3(aq) + 3H2(g)
Suppose you wanted to dissolve an aluminum block with a mass of 15.9g .
A)What minimum mass of H2SO4 (in g) would you need?
[***A=86.7g***]
B)What mass of H2 gas (in g) would be produced by the complete reaction of the aluminum block?
how does this part work???
If the entire mass of Aluminum is reacted, convert that to moles (15.9g).
Then, according to the balanced equation, you will get 1.5 times that number of moles as moles of H2. Convert that number of moles of H2 to grams.
To determine the mass of H2 gas produced by the complete reaction of the aluminum block, we can use the balanced equation of the reaction.
From the balanced equation: 2Al(s) + 3H2SO4(aq) -> Al2(SO4)3(aq) + 3H2(g), we can see that 1 mole of Al reacts with 3 moles of H2 gas.
1 mole of a substance is equal to its molar mass in grams. The molar mass of Al is approximately 27 g/mol.
To find the number of moles of Al in the 15.9 g aluminum block, we divide the mass by the molar mass:
Number of moles of Al = 15.9 g / 27 g/mol ≈ 0.589 mol
Since the molar ratio between Al and H2 gas is 2:3, we multiply the number of moles of Al by the ratio to find the corresponding number of moles of H2 gas:
Number of moles of H2 gas = 0.589 mol Al × (3 mol H2 gas / 2 mol Al) ≈ 0.884 mol
Finally, to convert moles of H2 gas to grams, we multiply the number of moles by the molar mass of H2, which is approximately 2 g/mol:
Mass of H2 gas = 0.884 mol H2 gas × 2 g/mol ≈ 1.77 g
Therefore, approximately 1.77 grams of H2 gas would be produced by the complete reaction of the aluminum block.
To calculate the mass of H2 gas produced, you need to determine the stoichiometry of the reaction between aluminum and sulfuric acid.
The balanced equation tells us that 2 moles of aluminum react with 3 moles of sulfuric acid to produce 3 moles of H2 gas.
First, you need to convert the mass of aluminum to moles. The molar mass of aluminum is 26.98 g/mol, so:
moles of Al = mass of Al / molar mass of Al
= 15.9 g / 26.98 g/mol
≈ 0.59 mol
Next, using the stoichiometry of the balanced equation, we can determine the moles of H2 gas produced. From the equation, we know that 2 moles of aluminum produce 3 moles of H2 gas. Therefore:
moles of H2 gas = moles of Al * (3 mol H2 gas / 2 mol Al)
= 0.59 mol * (3 mol H2 gas / 2 mol Al)
≈ 0.89 mol
Finally, we can convert the moles of H2 gas to mass using its molar mass. The molar mass of H2 is 2.02 g/mol:
mass of H2 gas = moles of H2 gas * molar mass of H2 gas
= 0.89 mol * 2.02 g/mol
≈ 1.8 g
Therefore, approximately 1.8 g of H2 gas would be produced by the complete reaction of the 15.9 g aluminum block.