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?\nhydrogen is oxidized from +1 to 0.\nchlorine is reduced from -1 to 0.\naluminum is oxidized from 0 to +3.\nhydrogen 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?\nhydrogen is oxidized from +1 to 0.\nchlorine is reduced from -1 to 0.\naluminum is oxidized from 0 to +3.\nhydrogen is reduced from 0 to -1.

Answer

Explanation:

Step1: Determine oxidation states of reactants

In $Al(s)$, oxidation state of $Al$ is $0$. In $HCl(aq)$, oxidation state of $H$ is $+ 1$ and of $Cl$ is $-1$.

Step2: Determine oxidation states of products

In $AlCl_3(aq)$, oxidation state of $Al$ is $+3$ and of $Cl$ is $-1$. In $H_2(g)$, oxidation state of $H$ is $0$.

Step3: Analyze oxidation - reduction

Oxidation is increase in oxidation state. Reduction is decrease in oxidation state. $Al$ goes from $0$ to $+3$, so it is oxidized. $H$ goes from $+1$ to $0$, so it is reduced. $Cl$ oxidation state remains $-1$ throughout.

Answer:

Aluminum is oxidized from $0$ to $+3$.