Answered

According to the following balanced reaction, how many moles of KO are required to exactly react with 4.33 moles of H2O?4 KO(s) + 2 H2O(l) → 4 KOH(s) + O2(g)

Answer :

Answer : The number of moles of KO required is, 8.66 moles.

Explanation : Given,

Moles of [tex]H_2O[/tex] = 4.33 mol

The given chemical reaction is:

[tex]4KO(s)+2H_2O(l)\rightarrow 4KOH(s)+O_2(g)[/tex]

From the balanced chemical reaction we conclude that,

As, 2 moles of [tex]H_2O[/tex] react with 4 moles of KO

So, 4.33 moles of [tex]H_2O[/tex] react with [tex]\frac{4}{2}\times 4.33=8.66[/tex] moles of KO

Thus, the number of moles of KO required is, 8.66 moles.

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