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

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

It is a mixture. simply put, a compound must be pure, that is, of only one chemical structure and composition. a mixture is made of different chemical substances (i.e. elements, molecules, compounds) that are not chemically bonded to each other, but instead physically grouped together, as in the case of gasoline (a homogeneous solution).