Question

Calcium carbide (CaC₂) reacts with water to produce acetylene (C₂H₂): CaC₂ (s) + 2H₂O (g) → Ca(OH)2 (s) + C₂H₂ (g). The production of 6.5 g of C₂H₂ requires the consumption of ________ g of H₂O?

Answer 1

To produce 6.5 g of acetylene (C₂H₂), 8.98 g of water (H₂O) would be consumed in the reaction.

Step-by-step explanation:

To determine the mass of water (H₂O) consumed when producing 6.5 g of acetylene (C₂H₂), we need to use the balanced chemical equation:

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

From the equation, we can see that 1 mole of C₂H₂ is produced from the reaction of 2 moles of H₂O. Using the molar masses of C₂H₂ (26.04 g/mol) and H₂O (18.02 g/mol), we can calculate the number of moles of H₂O consumed:

Moles of C₂H₂ = 6.5 g / 26.04 g/mol = 0.2494 mol

Moles of H₂O consumed = 2 * 0.2494 mol = 0.4988 mol

To calculate the mass of H₂O consumed, we can use the moles of H₂O consumed and its molar mass:

Mass of H₂O consumed = 0.4988 mol * 18.02 g/mol = 8.98 g

Therefore, the consumption of 6.5 g of C₂H₂ requires the consumption of 8.98 g of H₂O.