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.

Learn more: link

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.

since the atomic number is the number of protons in the nucleus, as we move to the left on the periodic table, the electrostatic pull between the nucleus and the valence electron shell decreases. as we move down a group (vertical column), the valence shell energy level gets further and further from the nucleus.