Answer:
1.07g
Explanation:
Step 1:
We will begin by writing the balanced equation for the reaction. This is given below:
CH4 + 2O2 —> CO2 + 2H2O
Step 2:
Determination of the masses of CH4 and O2 that reacted and the mass of H2O produced from the balanced equation. This is illustrated below:
Molar Mass of CH4 = 12 + (4x1) = 12 + 4 = 16g/mol
Molar Mass of O2 = 16x2 = 32g/mol
Mass of O2 from the balanced equation = 2 x 32 = 64g
Molar Mass of H2O = (2x1) + 16 = 2 + 16 = 18g/mol
Mass of H2O from the balanced equation = 2 x 18 = 36g
Summary:
From the balanced equation above,
16g of CH4 reacted with 64g of O2 to produce 36g of H2O.
Step 3:
Determination of the limiting reactant.
We need to know which of the reactant is limiting the reaction in order to obtain the maximum mass of water.
This is illustrated below:
From the balanced equation above,
16g of CH4 reacted with 64g of O2.
Therefore, 0.802g of CH4 will react with = (0.802 x 64)/16 = 3.21g of O2.
From the above calculations, a higher mass of O2 is needed to react with 0.802g of CH4. Therefore, O2 is the limiting reactant.
Step 4:
Determination of the mass of H2O produced from the reaction.
To obtain the maximum mass of H2O produced, the limiting reactant will be used because it will generate the maximum yield of the product.
From the balanced equation above,
64g of O2 produce 36g of H2O.
Therefore, 1.9g of O2 will produce = (1.9 x 36)/64 = 1.07g of H2O.
The maximum mass of water (H2O) produced by the reaction is 1.07g
