Given the unbalanced equation, for the species that is the reducing agent, enter

Question

Given the unbalanced equation, for the species that is the reducing agent, enter the symbol and the initial oxidation state of the specific element that will donate electrons.

Enter sign followed by Arabic numeral for oxidation state magnitude. Use 0 if the oxidation state is zero.

Example:

Element: S

Oxidation state: -2

Li(s) + H2O(l) ? Li+(aq) + OH-(aq) + H2(g)

Given the unbalanced equation, for the species that is the reducing agent, enter the symbol and the initial oxidation state of the specific element that will donate electrons. Enter sign followed by Arabic numeral for oxidation state magnitude. Use 0 if the oxidation state is zero. Example: Element: S Oxidation state: -2 Li(s) + H2O(l) ? Li+(aq) + OH-(aq) + H2(g) Element: Oxidation state:

Explanation / Answer

Write out the oxidation half reaction:
Li(s) ---> Li+(aq) + e-

We know water can autoionize into a proton and hydroxide.

H2O(l) ---> H+(aq) + OH-(aq)

So water is simply a proton and hydroxide together.

In a strongly reducing environment protons can be reduced into diatomic hydrogen gas.

-e + 2H+(aq) ---> H2(g)

Whats left after the proton is striped from the water OH-(aq)

We have:

Li(s) + H2O(l) ---> H2(s) + OH-(aq) + Li+(aq)

Simplify & Balance:

2Li(s) + 2H2O(l) ---> H2(g) + 2LiOH(aq)

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