Question

If you burn 45.2g of hydrogen and produce 404g of water, how much oxygen reacted

Answer 1

45.2÷2= 22.6 moles of hydrogen 2H2 + O2 = 2H2O 404g÷ 18= 22.4 moles of water 2 moles of H2 reacts with 1 mole of O2 So 22.6 will react with 11.3 moles of O2 11.3×32= 361.6 grams.

Answer 2

`359gO_(2)`

Step-by-step explanation:

1. Write the balanced equation:

`_(2)H_(2)+O_(2)=_(2)H_(2)O`

2. Find the quantity of
`H_(2)O` produced by 45.2g of hydrogen:

`45.2gH_(2)*(1molH_(2))/(2.016gH_(2))*(2molesH_(2)O)/(2molesH_(2))*(18gH_(2)O)/(1molH_(2)O)= 404gH_(2)O`

So, 45.2g of
`H_(2)` produce 404g of
`H_(2)O`

3. Find the quantity of
`O_(2)` that reacted with 45.2g of
`H_(2)`:

`404gH_(2)O*(1molH_(2)O)/(18gH_(2)O)*(2molesO_(2))/(2molesH_(2)O)*(16gO_(2))/(1molO_(2))=359gO_(2)`