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The combustion of acetylene gas is represented by this equation: 2c2h2(g) + 5o2(g) → 4co2(g) + 2h2o(g) how many grams of co2 and grams of h2o are produced when 52.0 g c2h2 burn in oxygen?

Respuesta :

kenmyna
2C2H2 (g) +  5O2 (g) ---->  4CO2(g)  +  2H20 (g)

Calculate  the  moles of C2H2  used
that  52g/  26  g/mol(molar   mass of  C2H2)=   2moles

by   of  use  of reacting  ratio  between  C2H2  to  CO2  which  is  2  :4  therefore  the  moles  of  CO2  = 2  x4/2  =   4 moles
mass  of  CO2 is therefore  =   4 mol   x    44 g/ mol(molar  mass  of  CO2) =  176  grams

the  mole  of   water  is  calculated  by   use    mole  ratio  between  C2H2  to  H20  which  is  2:2  therefore  also =  2 moles
mass  of  water  is =    2  moles  x   18  g/mol  =  36grams

Eduard22sly

A. The mass of CO₂ produced is 176 g.

B. The mass of H₂O produced is 36 g

We'll begin by calculating the mass of C₂H₂ that reacted and the masses of CO₂ and H₂O produced from the balanced equation.

2C₂H₂ + 5O₂ —> 4CO₂ + 2H₂O

Molar mass of C₂H₂ = (2×12) + (2×1) = 26 g/mol

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

Molar mass of CO₂ = 12 + (16×2) = 44 g/mol.

Mass of CO₂ from the balanced equation = 4 × 44 = 176 g

Molar mass of H₂O = (2×1) + 16 = 18 g/mol

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

SUMMARY:

From the balanced equation above,

52 g of C₂H₂ reacted to produce 176 g of CO₂ and 36 g of H₂O.

From the above, we can see that 52 g of C₂H₂ produced:

  • 176 g of CO₂
  • 36 g of H₂O

Learn more about stoichiometry:

https://brainly.com/question/25812506

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