Respuesta :

PhyCS
C2H2, or acetylene, has a molar mass of 26g. That means it has 113/26 = around 4.34 mols. Assuming complete combustion, the balanced equation comes out to this:

C2H2 + 3O2 --> 2H2O + 2CO2

Using the molar ratios, we get that we get 8.68 mols of water for every 4.34 mols, so since the molar mass of water is 18 grams per mol, we multiply 18 * 8.68 = about 156.24 grams.
Eduard22sly

The mass of water that can be formed when 113 g of acetylene, C₂H₂ is burned is 78.23 g

Balanced equation

2C₂H₂ + 5O₂ —> 2H₂O + 4CO₂

Molar mass of C₂H₂ = 26 g/mole

Mass of C₂H₂ from the balanced equation = 2 × 26 = 52 g

Molar mass of H₂O = 18 g/mole

Mass of H₂O from the balanced equation = 2 × 18 = 36 g

SUMMARY

From the balanced equation above,

52 g of C₂H₂ reacted to produce 36 g of H₂O

How to determine the mass of water produced

From the balanced equation above,

52 g of C₂H₂ reacted to produce 36 g of H₂O

Therefore,

113 g of C₂H₂ will react to produce = (113 × 36) / 52 = 78.23 g of H₂O

Thus, 78.23 g of H₂O were obtained from the reaction

Learn more about stoichiometry:

https://brainly.com/question/14735801

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