Answer:
793.6g of oxygen
Step-by-step explanation:
Step 1:
We'll begin by writing a balanced equation for the reaction between hydrogen and oxygen. This is illustrated below:
2H2 + O2 —> 2H2O
Step 2:
Determination of the masses of H2 and O2 that reacted from the balanced equation. This is illustrated below:
Molar Mass of H2 = 2 x 1.008 = 2.016g/mol
Mass of H2 from the balanced equation = 2 x 2.016 = 4.032g
Molar Mass of O2 = 2 x 15.999 = 31.998g/mol
Summary:
From the balanced equation above,
4.032g of H2 reacted with 31.998g of O2.
Step 3:
Determination of the mass of O2 that will react with 100g of H2. This is illustrated below:
From the balanced equation above,
4.032g of H2 reacted with 31.998g of O2.
Therefore, 100g of H2 will react with = (100 x 31.998) /4.032 = 793.6g of O2.
Therefore, 793.6g of oxygen gas will be consumed if 100g of Hydrogen is consumed.