Question

How many grams CaCO3 will be formed if 5 grams of CaO are used for this reaction?

Assume there are enough reactants CaO (s)
+CO2(g) --> CaCO3 (s)
Calculate the volume of CO2(g)

Answer 1

Step-by-step explanation:

The balanced chemical equation for the reaction between calcium oxide (CaO) and carbon dioxide (CO2) to form calcium carbonate (CaCO3) is:

CaO + CO2 -> CaCO3

From the equation, we can see that for every 1 mole of CaO, 1 mole of CO2 is needed to form 1 mole of CaCO3. If we have 5 grams of CaO, we can calculate the number of moles as follows:

5 g CaO / 56 g CaO/mol = 0.089 mol CaO

Since we need an equal number of moles of CO2, we can calculate the mass of CO2 needed as follows:

0.089 mol CO2 * 44 g CO2/mol = 3.9 g CO2

To calculate the volume of CO2 at standard temperature and pressure (STP), we need to know its molar volume, which is 24.45 L/mol. Using this, we can calculate the volume of CO2 as follows:

0.089 mol CO2 * 24.45 L CO2/mol = 2.16 L CO2

So, 5 grams of CaO will result in the formation of 5 grams of CaCO3, and the volume of CO2 produced will be 2.16 liters.