Answer:
10.09g
Explanation:
Step 1:
The balanced equation for the reaction.
We'll begin by writing a balanced equation for the reaction. This is illustrated below:
2C6H14 + 19O2 —> 12CO2 + 14H2O
Step 2:
Determination of the masses of C6H14 and O2 that reacted and the mass of H2O produced from the balanced equation. This is illustrated below:
Molar Mass of C6H14 = (12x6) + (14x1) = 72 + 14 = 86g/mol
Mass of C6H14 from the balanced equation = 2 x 86 = 172g
Molar Mass of O2 = 16x2 = 32g/mol
Mass of O2 from the balanced equation = 19 x 32 = 608g
Molar Mass of H2O = (2x1) + 16 = 18g/mol
Mass of H2O from the balanced equation = 14 x 18 = 252g
Summary:
From the balanced equation above,
172g of C6H14 reacted with 608g of O2 to produce 252g of H2O.
Step3:
Determination of the limiting reactant.
It essential that we determine the limiting reactant because it will be use to determine the theoretical yield.
From the balanced equation above,
172g of C6H14 reacted with 608g of O2.
Therefore, 6.89g of C6H14 will react with = (6.89 x 608)/172 = 24.36g of O2.
We can see that there are left over for O2 as only 24.36g of O2 reacted out of 47.4g that was given. Therefore, C6H14 is the limiting reactant.
Step 4:
Determination of the theoretical yield of water from the reaction.
The limiting reactant will be used to obtain theoretical yield of water. This is illustrated below:
From the balanced equation above,
172g of C6H14 produce 252g of H2O.
Therefore, 6.89g of C6H14 will produce = (6.89 x 252)/172 = 10.09g of H2O.
Therefore, the theoretical yield of water (H2O) is 10.09g
