What mass of CO2 could be absorbed by 1.34 g of CaO?
To determine the mass of CO2 that can be absorbed by 1.34 g of CaO, we need to know the stoichiometry of the reaction between CaO and CO2.
The balanced equation for the reaction 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. The molar mass of CaO is approximately 56.08 g/mol, and the molar mass of CO2 is approximately 44.01 g/mol.
Step 1: Calculate the number of moles of CaO.
Number of moles of CaO = mass of CaO / molar mass of CaO
Number of moles of CaO = 1.34 g / 56.08 g/mol
Step 2: Use the stoichiometry of the reaction to determine the number of moles of CO2.
Number of moles of CO2 = Number of moles of CaO
Step 3: Calculate the mass of CO2.
Mass of CO2 = number of moles of CO2 x molar mass of CO2
Mass of CO2 = (1.34 g / 56.08 g/mol) x 44.01 g/mol
By performing these calculations, you can determine the mass of CO2 that could be absorbed by 1.34 g of CaO.
CaO + CO2 ==> CaCO3
Convert 1.34 g CaO to moles. moles = grams/molar mass
Using the coefficients in the balanced equation, convert moles CaO to moles CO2.
Convert moles CO2 to grams. g = moles x molar mass.