Answer:
2643.08g of O2
Explanation:
Step 1:
The balanced equation for the reaction. This is given below:
2C2H2 + 5O2 —> 4CO2 + 2H2O
Step 2:
Determination of the masses of C2H2 and O2 that reacted from the balanced equation. This is illustrated below:
2C2H2 + 5O2 —> 4CO2 + 2H2O
Molar Mass of C2H2 = (12x2) + (2x1) = 24 + 2 = 26g/mol
Mass of C2H2 from the balanced equation = 2 x 26 = 52g
Molar Mass of O2 = 16x2 = 32g/mol
Mass of O2 from the balanced equation = 5 x 32 = 160g
From the balanced equation above,
52g of C2H2 reacted with 160g of O2.
Step 3:
Determination of the mass of oxygen that would be required to react completely with 859.0g of C2H2.
This is illustrated below:
From the balanced equation above,
52g of C2H2 reacted with 160g of O2.
Therefore, 859g of C2H2 will react with = (859 x 160)/52 = 2643.08g of O2.
From the calculations made above, 2643.08g of O2 will react completely with 895g of C2H2.
From the stoichiometry of the reaction 82.5 moles of oxygen is required.
A combustion reaction is a reaction in which a substance is burnt in oxygen. The equation of this reaction is; 2C2H2 + 5O2 ------> 4CO2 + 2H2O.
Number of moles of acetylene reacted = 859.0 g/26 g/mol = 33 moles
From the reaction equation;
2 moles of acetylene reacts with 5 moles of oxygen
33 moles of acetylene reacts with 33 × 5/2 = 82.5 moles of oxygen
Hence 82.5 moles of oxygen is required to react completely with acetylene.
Learn more about stoichiometry: https://brainly.com/question/12446045
