Question

Aluminum metal reacts with dilute sulfuric acid to produce aluminum sulfate and hydrogen gas. what mass of aluminum will react with 5.890 g of sulfuric acid

Answer 1

Aluminium reacts with dilute sulfuric acid based on the following reaction:

2Al + 3H2SO4 ..............> Al2 (SO4)3 + 3H2

From the periodic table:

mass of aluminium = 27 grams

mass of hydrogen = 1 gram

mass of oxygen = 16 grams

mass of sulfur = 32 grams

Therefore:

molar mass of aluminium = 27 grams

molar mass of sulfuric acid = 2(1) + 32 + 4(16) = 98 grams

From the balanced chemical equation:

2 moles of aluminium react with 3 moles of dilute sulfuric acid.

This means that 34 grams of Al react with 294 grams of the acid

To get the amount of aluminium that reacts with 5.890 g of sulfuric acid, we will do cross multiplication as follows:

amount of Al = (5.890 x 34) / 294 = 0.6811 grams

Step-by-step explanation:

Answer 2

Aluminium reacts with dilute sulfuric acid based on the following reaction:
2Al + 3H2SO4 ..............> Al2 (SO4)3 + 3H2

From the periodic table:
mass of aluminium = 27 grams
mass of hydrogen = 1 gram
mass of oxygen = 16 grams
mass of sulfur = 32 grams

Therefore:
molar mass of aluminium = 27 grams
molar mass of sulfuric acid = 2(1) + 32 + 4(16) = 98 grams

From the balanced chemical equation:
2 moles of aluminium react with 3 moles of dilute sulfuric acid.
This means that 34 grams of Al react with 294 grams of the acid

To get the amount of aluminium that reacts with 5.890 g of sulfuric acid, we will do cross multiplication as follows:
amount of Al = (5.890 x 34) / 294 = 0.6811 grams