Question

Acetylene gas, C2H2, is produced as a result of the following reaction: CaC2 + 2H2O ----> C2H2 + Ca(OH)2.

(a) If 32 grams of CaC2 are consumed in this reaction, how many moles of water are needed ?

(b) How Many moles of each product would form ?

Answer 1

To produce acetylene from CaC2 and water, 0.998 moles of water are needed for 32 grams of CaC2, resulting in the formation of 0.499 moles of acetylene and 0.499 moles of calcium hydroxide.

Step-by-step explanation:

The student has asked about the stoichiometry involved in producing acetylene gas (C2H2) from calcium carbide (CaC2) and water. Here is the solution to the question:

1. First, determine the molar mass of CaC2 which is 64.1 g/mol.
2. Calculate the number of moles of CaC2 consumed in the reaction: 32 g CaC2 × (1 mol/64.1 g) = 0.499 moles of CaC2.
3. According to the balanced chemical equation, 2 moles of H2O are required for 1 mole of CaC2. Hence, the moles of water needed are 0.499 moles × 2 = 0.998 moles of H2O.
4. For the products, 1 mole of CaC2 produces 1 mole of C2H2 and 1 mole of Ca(OH)2. Thus, 0.499 moles of CaC2 will produce 0.499 moles of C2H2 and 0.499 moles of Ca(OH)2.

In summary, 0.998 moles of water are needed, and 0.499 moles of each product (C2H2 and Ca(OH)2) would be formed.