Question

If 32.0g cac2 are consumed in this reaction, how many moles of h2o are needed

Answer 1

To react 32.0g of CaC2 with H2O, 0.998 moles of H2O are required, based on the balanced chemical equation and the molar mass calculation for CaC2.

Step-by-step explanation:

To determine how many moles of H2O are needed when 32.0g of CaC2 are consumed in the reaction, we must first write down the chemical equation and balance it. The reaction between calcium carbide (CaC2) and water (H2O) to form calcium hydroxide (Ca(OH)2) and acetylene (C2H2) is as follows:

CaC2 + 2H2O → Ca(OH)2 + C2H2

This balanced equation indicates that for every mole of CaC2, two moles of H2O are required. The molar mass of CaC2 is approximately 64.1 g/mol. Therefore, 32.0 g of CaC2 corresponds to:

32.0 g ÷ 64.1 g/mol = 0.499 moles of CaC2

Since the ratio is 1:2, you need twice the amount of moles of H2O as CaC2. Therefore, you need:

0.499 moles of CaC2 × 2 = 0.998 moles of H2O

Answer 2

The reaction equation is:
CaC₂ + 2H₂O → Ca(OH)₂ + C₂H₂

Moles of CaC₂ = 32 / (40 + 12 x 2)
Moles of CaC₂ = 0.5

Molar ratio of CaC₂ to H₂O = 1 : 2
Moles of H₂O = 2 x 0.5 = 1 mole of H₂O needed