Respuesta :
Answer: The mass of water produced is 44.28 g
Explanation:
We are given:
Volume of oxygen gas = 27.50 L
At STP conditions:
22.4 L of volume is occupied by 1 mole of a substance
27.50 L of oxygen gas will be occupied by = [tex]\frac{1mol}{22.4L}\times 27.50L=1.23mol[/tex]
The chemical equation for the formation of water follows:
[tex]2H_2+O_2\rightarrow 2H_2O[/tex]
By the stoichiometry of the reaction:
If 1 mole of oxygen gas produces 2 moles of water
So, 1.23 moles of oxygen gas will produce = [tex]\frac{2}{1}\times 1.23=2.46mol[/tex] of water
The number of moles is defined as the ratio of the mass of a substance to its molar mass. The equation used is:
[tex]\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}[/tex] ......(1)
Molar mass of water = 18 g/mol
Plugging values in equation 1:
[tex]\text{Mass of water}=(2.46mol\times 18g/mol)=44.28g[/tex]
Hence, the mass of water produced is 44.28 g
