How many moles of CaC2 are needed to react completely with 45.0g H2O?

Equation: CaC2+2 H2O—-> C2H2 + Ca(OH)2.

The number of mole of CaC₂ needed to completely react with 45 g of H₂O is 1.25 mole

We'll begin by calculating the number of mole in 45 g of H₂O.

Mass of H₂O = 45 g

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

Mole = mass / molar mass

Mole of H₂O = 45 / 18

CaC₂ + 2H₂O —> C₂H₂ + Ca(OH)₂

From the balanced equation above,

2 moles of H₂O reacted with 1 mole of CaC₂.

Therefore,

2.5 moles of H₂O will react with = 2.5 / 2 = 1.25 mole of CaC₂.

Thus, 1.25 mole of CaC₂ is needed for the reaction.

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In order to react with 45 g of water 1.25 moles of CaC₂ are required.

Explanation:

Given data:

Moles of CaC₂ needed = ?

Mass of water = 45.0 g

Solution:

Chemical equation:

CaC₂ + 2H₂O      →      C₂H₂ + Ca(OH)₂

Number of moles of water:

Number of moles = mass/ molar mass

Number of moles = 45 g/ 18 g/mol

Number of moles = 2.5 mol

Now we will compare the moles of water and CaC₂ from balance chemical equation:

                     H₂O             :             CaC₂

                       2                :                1

                     2.5              :             1/2×2.5 =1.25 mol

In order to react with 45 g of water 1.25 moles of CaC₂ are required.

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