consider the redox reaction below. 2al(s) + 6hcl(aq)→2alcl3(aq)+3h2(g) which statement correctly describes a…

consider the redox reaction below. 2al(s) + 6hcl(aq)→2alcl3(aq)+3h2(g) which statement correctly describes a half - reaction that is taking place? hydrogen is oxidized from +1 to 0. chlorine is reduced from -1 to 0. aluminum is oxidized from 0 to +3. hydrogen is reduced from 0 to -1.

consider the redox reaction below. 2al(s) + 6hcl(aq)→2alcl3(aq)+3h2(g) which statement correctly describes a half - reaction that is taking place? hydrogen is oxidized from +1 to 0. chlorine is reduced from -1 to 0. aluminum is oxidized from 0 to +3. hydrogen is reduced from 0 to -1.

Answer

Explanation:

Step1: Determine oxidation - states

In Al(s), the oxidation state of Al is 0. In HCl, H has an oxidation state of +1 and Cl has an oxidation state of -1. In AlCl₃, Al has an oxidation state of +3 and Cl has an oxidation state of -1. In H₂, the oxidation state of H is 0.

Step2: Analyze oxidation and reduction

Oxidation is the increase in oxidation state and reduction is the decrease in oxidation state.

  • For hydrogen in HCl (+1) and H₂ (0), hydrogen is reduced from +1 to 0.
  • Chlorine has an oxidation state of -1 in HCl and AlCl₃, so it is neither oxidized nor reduced.
  • Aluminum in Al(s) (0) and AlCl₃ (+3) is oxidized from 0 to +3.

Answer:

Aluminum is oxidized from 0 to +3.