Question

How many grams of oxygen are formed when 8.20 moles of KOH are formed? 4 KO(s) + 2 H2O(l) → 4 KOH(s) + O2(g)

Answer 1

49.7g02* that's the answer

Answer 2

Answer : The mass of oxygen formed are 65.6 grams.

Explanation :

First we have to calculate the moles of
`O_2`

The given balance chemical reaction is:

`4KO(s)+2H_2O(l)rightarrow 4KOH(s)+O_2(g)`

From the balanced chemical reaction we conclude that,

As, when 4 moles of KOH formed then 1 mole of
`O_2` will be formed

So, when 8.20 moles of KOH formed then
`(8.20)/(4)=2.05` mole of
`O_2` will be formed

Now we have to calculate the mass of
`O_2`

`\text{ Mass of }O_2=\text{ Moles of }O_2* \text{ Molar mass of }O_2`

Molar mass of
`O_2` = 32 g/mole

`\text{ Mass of }O_2=(2.05moles)* (32g/mole)=65.6g`

Therefore, the mass of oxygen formed are 65.6 grams.