$$2Al(s) + 3H_2SO_4(aq) → Al_2(SO_4)_3(aq) + 3H_2(g)$$

Explanation:

Aluminum is a reactive metal, and it reacts with dilute sulfuric acid to produce aluminum sulfate and hydrogen gas. The reaction is exothermic, meaning that it releases heat. The hydrogen gas produced in the reaction is flammable and can be used as a fuel. Aluminum sulfate is a white, crystalline solid that is soluble in water. It is used in a variety of applications, including papermaking, water purification, and as a mordant in dyeing.

The reaction between aluminum and dilute sulfuric acid can be broken down into two half-reactions:

Oxidation half-reaction:

$$2Al(s) → 2Al^{3+}(aq) + 6e^-$$

Reduction half-reaction:

$$6H^+ (aq) + 6e^- → 3H_2(g)$$

The overall reaction is the sum of the two half-reactions:

$$2Al(s) + 6H^+(aq) → 2Al^{3+}(aq) + 3H_2(g)$$

This reaction is an example of a redox reaction, in which one substance is oxidized (loses electrons) and another substance is reduced (gains electrons). In this case, aluminum is oxidized and hydrogen is reduced.