consider the redox reaction below.\n2al(s) + 6hcl(aq)→2alcl3(aq)+3h2(g)\nwhich statement correctly describes…

consider the redox reaction below.\n2al(s) + 6hcl(aq)→2alcl3(aq)+3h2(g)\nwhich statement correctly describes a half - reaction that is taking place?\no hydrogen is oxidized from +1 to 0.\no chlorine is reduced from -1 to 0.\no aluminum is oxidized from 0 to +3.\no hydrogen is reduced from 0 to -1.

consider the redox reaction below.\n2al(s) + 6hcl(aq)→2alcl3(aq)+3h2(g)\nwhich statement correctly describes a half - reaction that is taking place?\no hydrogen is oxidized from +1 to 0.\no chlorine is reduced from -1 to 0.\no aluminum is oxidized from 0 to +3.\no hydrogen is reduced from 0 to -1.

Answer

Brief Explanations:

  1. First, determine oxidation - states:
    • In elemental aluminum ((Al(s))), the oxidation state of (Al) is (0). In (AlCl_3), since (Cl) has an oxidation state of (- 1) and the compound is neutral, the oxidation state of (Al) is (+3).
    • In (HCl), (H) has an oxidation state of (+1) and (Cl) has an oxidation state of (-1). In (H_2(g)), the oxidation state of (H) is (0).
  2. Recall definitions: Oxidation is an increase in oxidation state, and reduction is a decrease in oxidation state.
    • Aluminum goes from an oxidation state of (0) in (Al(s)) to (+3) in (AlCl_3), so it is oxidized.
    • Hydrogen goes from an oxidation state of (+1) in (HCl) to (0) in (H_2), so it is reduced. Chlorine's oxidation state remains (-1) in (HCl) and (AlCl_3).

Answer:

Aluminum is oxidized from 0 to +3.