Answer:
Volume of O₂ = 56 dm³
mass of water vapors (H₂O) = 90 g
Explanation:
Data Given:
mass of Oxygen = 10 g
Volume of Oxygen = ?
mass of the water vapor = ?
Reaction Given:
2H₂+O₂---->2H₂O
Solution:
First we have to look at the reaction for the information required
2H₂ + O₂ -------> 2H₂O
2 mol 1mol 2 mol
now convert moles to grams
molar mass of H₂ = 2(1) = 2 g/mol
molar mass of O₂ = 2(16) = 32 g/mol
molar mass of H₂0 = 2(1) + 16 = 18 g/mol
So the masses will be
2H₂ + O₂ -------> 2H₂O
2 mol (2 g/mol) 1mol (32 g/mol) 2 mol (18 g/mol)
4 g 32 g 36 g
So now we know that
4 g of hydrogen combine with 32 g of Oxygen and give 36 g of water vapors.
By using above information
First we find the volume of Oxygen:
For this first we find mass and then moles of Oxygen
As we know
if 4 g of hydrogen combine with 32 g of Oxygen then how much oxygen will react with 10 g of hydrogen
Apply unity formula
4 g of hydrogen H₂ ≅ 32 g of Oxygen O₂
10 g of hydrogen H₂ ≅ X g of Oxygen O₂
by doing Cross multiplication
g of Oxygen O₂ = 32 g x 10 g / 4 g
g of Oxygen O₂ = 80 g
So,
mass of oxygen = 80 g
now find moles of oxygen
formula used:
no. of moles = mass in grams/ molar mass . . . . . . (1)
Put values in above equation 1
no. of moles = 80 g / 32 g/mol
no. of moles = 2.5
Now to find volume of oxygen
Formula used
Volume of O₂ = no. of moles x molar volume (22.4 dm³/ mol) . . . . . . (2)
Put values in equation 2
Volume of O₂ = 2.5 moles x 22.4 dm³/mol
Volume of O₂ = 56 dm³
______________________
Now to find mass of water vapors
As we now
if 4 g of hydrogen produce 36 g of water vapors then how much water vapor will produce from 10 g of hydrogen
Apply unity formula
4 g of hydrogen H₂ ≅ 36 g of water vapors (H₂O)
10 g of hydrogen H₂ ≅ X g of water vapors (H₂O)
by doing Cross multiplication
g of water vapors (H₂O) = 36 g x 10 g / 4 g
g of water vapors (H₂O) = 90 g
So,
mass of water vapors (H₂O) = 90 g
