Acetylene gas (C2H2) is produced as a result of the following reaction. CaC2 (s) + 2H20(I) -> C2H2(g) + Ca (OH)2 (aq) a. If 3.20 moles of CaC2 are consumed in this reaction, how many grams of H2O are needed? Given: Requested:

Answers

Answer 1

Answer:

Answer:approximately 115.33 grams of H2O are needed to react with 3.20 moles of CaC2 in the given reaction.

Explanation:To determine how many grams of H2O are needed to react with 3.20 moles of CaC2 in the given reaction, we can use stoichiometry and the molar ratios between CaC2 and H2O in the balanced chemical equation.

First, let's write down the balanced chemical equation:

CaC2 (s) + 2H2O (l) -> C2H2 (g) + Ca(OH)2 (aq)

From the balanced equation, we can see that 1 mole of CaC2 reacts with 2 moles of H2O.

Now, let's use this information to calculate the moles of H2O required to react with 3.20 moles of CaC2:

Moles of H2O = (3.20 moles CaC2) * (2 moles H2O / 1 mole CaC2)

Moles of H2O = 3.20 moles * 2

Moles of H2O = 6.40 moles

Now that we know we need 6.40 moles of H2O, we can calculate the grams of H2O needed using the molar mass of H2O:

Molar mass of H2O = 2(1.01 g/mol) + 16.00 g/mol = 2.02 g/mol + 16.00 g/mol = 18.02 g/mol

Now, calculate the grams of H2O:

Grams of H2O = (6.40 moles) * (18.02 g/mol)

Grams of H2O ≈ 115.33 grams

So, approximately 115.33 grams of H2O are needed to react with 3.20 moles of CaC2 in the given reaction.

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