Question

4) How many grams of carbon dioxide would be needed to produce 3.382 grams of

acetylene (C2H,) using the following reaction?
4 CO2(g) + 2 H20(g) → 2 C2H2(g) +5 02(g)

Answer 1

11.4 g CO₂

Step-by-step explanation:

Your chemical equation is:

4 CO₂ + 2 H₂O ⇒ 2 C₂H₂ + 5 O₂

You need to produce 3.382 g of acetylene. To find out how many grams of carbon dioxide you need, first convert grams of acetylene to moles using the molar mass. The molar mass of acetylene is 26.04 g/mol.

(3.382 g)/(26.04 g/mol) = 0.130 mol C₂H₂

Now, use the mole ratio between acetylene and carbon dioxide to convert from moles of acetylene to moles of carbon dioxide. You can find the mole ratio by looking at the chemical equation. The mole ratio is (4 mol CO₂)/(2 mol C₂H₂).

(0.130 mol C₂H₂) × (4 mol CO₂)/(2 mol C₂H₂) = 0.260 mol CO₂

Since you now have moles of carbon dioxide, you can convert to grams using the molar mass. The molar mass of carbon dioxide is 44.01 g/mol.

0.260 mol × 44.01 g/mol = 11.4 g CO₂

You will need 11.4 g of CO₂ to produce 3.382 g of C₂H₂.