Question

You react an excess of hydrogen gas with 8.00 g of oxygen gas to form water (as shown in the balanced equation below). what mass of water is formed, assuming a complete reaction?

Answer 1

2H₂ + O₂ = 2H₂O

m(H₂O)=2M(H₂O)m(O₂)/M(O₂)

m(H₂O)=2*18*8/32= 9 g

Answer 2

The mass of water formed by the complete reaction of oxygen has been 9 grams.

The balanced chemical reaction for the formation of water has been:

$\rm 2\;H_2\;+\;O_2\;\rightarrow\;2\;H_2O$

Since hydrogen has been in access, oxygen has been the limiting reactant.

The moles of oxygen = $\rm \dfrac{mass}{molecular\;mass}$

Moles of 8 grams oxygen = $\rm \dfrac{8}{32}$

Moles of 8 grams oxygen = 0.25 mol.

From the balanced equation,

1 mole oxygen = 2 moles water

0.25 moles oxygen = 0.25 × 2 moles water

= 0.5 moles of water.

Mass of water = Moles × molecular weight

Mass of water = 0.5 mol × 18 g/mol

Mass of water = 9 grams.

The mass of water formed by the complete reaction of oxygen has been 9 grams.

For more information about the chemical reaction, refer to the link:

https://brainly.com/question/19085755