Question

In the reaction 2Al (s) + 3H₂SO₄ (aq) -> Al₂(SO₄)₃ (s) + 3H₂ (g) involving 10.6g of aluminum, how many grams of sulfur are contained in the Al₂(SO₄)₃ formed?

a) 4.48 g
b) 8.96 g
c) 13.44 g
d) 17.92 g

Answer 1

The grams of sulfur in Al₂(SO₄)₃ can be calculated using the molar mass of the compound and the given mass of aluminum.

Step-by-step explanation:

To determine the grams of sulfur in Al₂(SO₄)₃, we first need to find the molar mass of Al₂(SO₄)₃. The molar mass of Al₂(SO₄)₃ is calculated by adding the atomic masses of each element in its formula:

Molar mass of Al₂(SO₄)₃ = 2(Al) + 3(S) + 12(O) + 4(O)

= 2(26.98 g/mol) + 3(32.07 g/mol) + 12(16.00 g/mol) + 4(16.00 g/mol)

= 342.14 g/mol

Now we can use the molar mass to calculate the grams of sulfur in Al₂(SO₄)₃:

Grams of sulfur = (grams of Al₂(SO₄)₃ formed) * (molar mass of S / molar mass of Al₂(SO₄)₃)

= 10.6 g * (96.06 g/mol / 342.14 g/mol)

= 2.997 g

Therefore, the correct answer is 2.997 g, which is closest to 4.48 g (option a).