High School

If 6.00 moles of CaO are combined with CO2, how many grams of CaCO3 would be formed?

Answer :

Answer:

Mass of CaCO3 = 600.54g

Explanation:

The balanced chemical equation for the reaction between CaO and CO2 to form CaCO3 is:

CaO + CO2 → CaCO3

From the balanced equation, we can see that 1 mole of CaO reacts with 1 mole of CO2 to produce 1 mole of CaCO3.

To determine how many grams of CaCO3 will be formed from 6.00 moles of CaO, we need to use the molar mass of CaCO3, which is 100.09 g/mol.

The calculation is as follows:

6.00 moles of CaO × (1 mole of CaCO3 / 1 mole of CaO) × (100.09 g/mol) = 600.54 g

Therefore, 600.54 grams of CaCO3 will be formed from 6.00 moles of CaO.

600.54 g of CaCO3 would be formed

The chemical equation in balanced form for the reaction between CaO and CO2 to form CaCO3 is

CaO + CO2 -> CaCO3

Here 1 mol of CaO reacts with 1 mol of CO2 to form 1 mol of CaCO3

Therefore 6.00 moles will combine with 6.00 moles of CO2 to form 6.00 moles of CaCO3.

The molar mass of CaCO3= 100.09 g/mol

Number of moles of CaCO3=6.00 moles

we know that,

Number of moles of CaCO3= mass of CaCO3/molar mass of CaCO3

Therefore mass of CaCO3 =Number of moles of CaCO3* molar mass of CaCO3

Mass of CaCO3=6.00moles*100.09g/mol

= 600.54g

To learn more about questions related to chemical equations refer to:

https://brainly.com/question/14562573?