2Al(s) + 3H2SO4(aq) → Al2(SO4)3(aq) + 3H2(g)
In this reaction, aluminum metal (Al) reacts with sulfuric acid (H2SO4) to form aluminum sulfate (Al2(SO4)3) and hydrogen gas (H2). The reaction is exothermic, meaning that it releases heat.
Here is a step-by-step explanation of the reaction:
1. Initially, the solid aluminum metal (Al) is in its elemental form.
2. When the aluminum comes into contact with the aqueous sulfuric acid (H2SO4), it undergoes an oxidation-reduction reaction.
3. Aluminum acts as the reducing agent, meaning it loses electrons and gets oxidized from a neutral state to a +3 oxidation state.
4. On the other hand, hydrogen ions (H+) from the sulfuric acid act as the oxidizing agent, accepting electrons and getting reduced from a +1 oxidation state to a 0 oxidation state.
5. As a result of the electron transfer, aluminum atoms combine with sulfate ions (SO4^2-) from the sulfuric acid to form aluminum sulfate [Al2(SO4)3].
6. Simultaneously, hydrogen gas (H2) is produced as a byproduct of the reaction. The hydrogen atoms formed by the reduction of hydrogen ions combine to form diatomic hydrogen molecules (H2).
Overall, the reaction involves the oxidation of aluminum and the reduction of hydrogen ions, leading to the formation of aluminum sulfate and hydrogen gas.
