Question

How many grams of calcium carbonate will I need to form 13.0 grams of carbon dioxide?

C2H4 + 3O2 -------> 2CO2 + 2H2O

Answer 1

To form 13.0 grams of carbon dioxide, you will need approximately 14.75 grams of calcium carbonate.

Step-by-step explanation:

To determine the number of grams of calcium carbonate needed to form 13.0 grams of carbon dioxide (CO2), we can use the balanced chemical equation provided: C2H4 + 3O2 -> 2CO2 + 2H2O

From the equation, we can see that for every 2 moles of CO2 produced, 1 mole of calcium carbonate is needed. We can convert grams of CO2 to moles by dividing by the molar mass of CO2. Then we can use the mole ratio from the balanced equation to determine the moles of calcium carbonate needed. Finally, we can convert moles of calcium carbonate to grams by multiplying by the molar mass of calcium carbonate.

Let's calculate:

1. Convert grams of CO2 to moles: 13.0 g CO2 * (1 mol CO2 / 44.01 g CO2) = 0.295 mol CO2
2. Using the mole ratio from the balanced equation, the moles of calcium carbonate needed = 0.295 mol CO2 * (1 mol CaCO3 / 2 mol CO2) = 0.1475 mol CaCO3
3. Convert moles of CaCO3 to grams: 0.1475 mol CaCO3 * (100.09 g CaCO3 / 1 mol CaCO3) = 14.7525 g CaCO3

Therefore, you will need approximately 14.75 grams of calcium carbonate to form 13.0 grams of carbon dioxide.