Question

For the balanced equationLaTeX: 2Li\left(s\right)\:+\:2H_2O\left(l\right)\:\longrightarrow\:2LiOH\left(aq\right)\:+\:H_2\left(g\right)identify what is:
oxidized

reduced

oxidizing agent

reducing agent

Answer 1

Answer: Lithium is getting oxidized and is a reducing agent. Hydrogen is getting reduced and is oxidizing agent.

Explanation:

Oxidation reaction is defined as the reaction in which an atom looses its electrons. Here, oxidation state of the atom increases.

$X\rightarrow X^{n+}+ne^-$

Reduction reaction is defined as the reaction in which an atom gains electrons. Here, the oxidation state of the atom decreases.

$X^{n+}+ne^-\rightarrow X$

Oxidizing agents are defined as the agents which oxidize other substance and itself gets reduced. These agents undergoes reduction reactions.

Reducing agents are defined as the agents which reduces the other substance and itself gets oxidized. These agents undergoes reduction reactions.

For the given chemical reaction:

$2Li(s)+2H_2O(l)\rightarrow 2LiOH(aq.)+H_2(g)$

The half reactions for the above reaction are:

Oxidation half reaction: $2Li(s)\rightarrow 2Li^{+}(aq.)+2e^-$

Reduction half reaction: $2H^(aq.)+2e^-\rightarrow H_2(g)$

From the above reactions, lithium is loosing its electrons. Thus, it is getting oxidized and is considered as a reducing agent.

Hydrogen is gaining electrons and thus is getting reduced and is considered as an oxidizing agent.