To derive the net ionic equation for the reaction between solid aluminum (Al) and aqueous sulfuric acid (H2SO4), we first need to understand the overall reaction that takes place. Aluminum reacts with sulfuric acid to produce aluminum sulfate and hydrogen gas.
The balanced molecular equation for this reaction is:
2 Al (s) + 3 H2SO4 (aq) → Al2(SO4)3 (aq) + 3 H2 (g)
Next, we will write the complete ionic equation. In this case, aluminum sulfate is soluble in water and dissociates into ions:
2 Al (s) + 3 H2SO4 (aq) → 2 Al3+ (aq) + 3 SO42- (aq) + 3 H2 (g)
Now, we can identify the spectator ions. Spectator ions do not participate in the actual reaction. In our case, they are the sulfate ions. We will remove them from both sides of the equation:
Original ionic equation:
2 Al (s) + 6 H+ (aq) + 3 SO42- (aq) → 2 Al3+ (aq) + 3 SO42- (aq) + 3 H2 (g)
Removing the sulfate ions gives us:
2 Al (s) + 6 H+ (aq) → 2 Al3+ (aq) + 3 H2 (g)
Finally, simplifying, we arrive at the net ionic equation:
2 Al (s) + 6 H+ (aq) → 2 Al3+ (aq) + 3 H2 (g)
This net ionic equation shows the actual chemical change taking place in the reaction, highlighting the aluminum and hydrogen ions involved.