Calcium carbide (CaC₂)reacts with water to produce acetylene (C₂H₂): CaC₂(s)+ 2H₂O (g)→ Ca(OH)₂ (s)+ C₂H₂ (g) Production of 6.5 g of C₂H₂ requires consumption of ________ g of H₂O. A)2.3 B)4.5 C)9.0 D)480 E)0.048

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Quizplus · Accepted Answer

To solve this, first, we need to balance the chemical equation and then use stoichiometry to find the mass of water consumed. The balanced chemical equation is already given: $$CaC_2(s) + 2H_2O(g) \rightarrow Ca(OH)_2(s) + C_2H_2(g)$$. This shows a 1:2 molar ratio between calcium carbide and water. The molar mass of acetylene ($C_2H_2$) is approximately 26 g/mol. Therefore, to produce 6.5 g of acetylene, $\frac{6.5 \, \text{g}}{26 \, \text{g/mol}} = 0.25 \, \text{mol}$ of acetylene are produced. Since the reaction requires 2 moles of water for every mole of acetylene produced, we need $0.25 \, \text{mol} \times 2 = 0.5 \, \text{mol}$ of water. The molar mass of water ($H_2O$) is approximately 18 g/mol, so $0.5 \, \text{mol} \times 18 \, \text{g/mol} = 9.0 \, \text{g}$ of water are consumed.

Calcium Carbide (CaC2)reacts with Water to Produce Acetylene (C2H2): CaC2

Calcium Carbide (CaC₂)reacts with Water to Produce Acetylene (C₂H₂): CaC₂