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Acetylene gas, C2H2, is produced as a result of the following reaction: CaC2 + 2H2O ----> C2H2 + Ca(OH)2.

(a) If 32 grams of CaC2 are consumed in this reaction, how many moles of water are needed ?

(b) How Many moles of each product would form ?

Sagot :

Eduard22sly

Given the data from the question,

A. The number of mole of water needed for the reaction is 1 mole

Bi. The number of mole of C₂H₂ formed is 0.5 mole

Bii. The number of mole of Ca(OH)₂ formed is 0.5 mole

How to determine the mole of CaC₂

  • Mass of CaC₂ = 32 g
  • Molar mass of CaC₂ = 40 + (12×2) = 64 g/mol
  • Mole of CaC₂ =?

Mole = mass / molar mass

Mole of CaC₂ = 32 / 64

Mole of CaC₂ = 0.5 mole

A. How to determine the mole of water neede

Balanced equation

CaC₂ + 2H₂O —> C₂H₂ + Ca(OH)₂

From the balanced equation above,

1 mole of CaC₂ required 2 moles of H₂O

Therefore,

0.5 mole of CaC₂ will require = 0.5 × 2 = 1 mole of H₂O

Thus, 1 mole of H₂O is needed for the reaction.

Bi. How to determine the mole of C₂H₂ produced

Balanced equation

CaC₂ + 2H₂O —> C₂H₂ + Ca(OH)₂

From the balanced equation above,

1 mole of CaC₂ reacted to produce 1 mole of C₂H₂

Therefore,

0.5 mole of CaC₂ will also react to produce 0.5 mole of C₂H₂

Thus, 0.5 mole of C₂H₂ was obtained from the reaction

Bii. How to determine the mole of Ca(OH)₂ produced

Balanced equation

CaC₂ + 2H₂O —> C₂H₂ + Ca(OH)₂

From the balanced equation above,

1 mole of CaC₂ reacted to produce 1 mole of Ca(OH)₂

Therefore,

0.5 mole of CaC₂ will also react to produce 0.5 mole of Ca(OH)₂

Thus, 0.5 mole of Ca(OH)₂ was obtained from the reaction

Learn more about stoichiometry:

https://brainly.com/question/14735801

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