Answer:
33.01 grams of NaOH is required to absorb the whole CO2 produced in the reaction.
Step-by-step explanation:
To find the mass of NaOH required to absorb all the CO2 produced in the reaction between 25 g of pure CaCO3 and 0.75 moles of HCl, you need to consider the stoichiometry of the reaction and the molar mass of CO2.
The balanced chemical equation for the reaction between CaCO3 and HCl is:
CaCO3 + 2HCl -> CaCl2 + H2O + CO2
From the balanced equation, you can see that 1 mole of CaCO3 produces 1 mole of CO2. Therefore, the number of moles of CO2 produced in the reaction is also 0.75 moles (since you have 0.75 moles of HCl).
Now, you need to find the molar mass of CO2. Carbon (C) has a molar mass of approximately 12.01 g/mol, and oxygen (O) has a molar mass of approximately 16.00 g/mol. So, the molar mass of CO2 is:
Molar mass of CO2 = 12.01 g/mol (C) + 2 * 16.00 g/mol (O) = 44.01 g/mol
Now, you can calculate the mass of CO2 produced:
Mass of CO2 = moles of CO2 * molar mass of CO2
Mass of CO2 = 0.75 moles * 44.01 g/mol = 33.01 g
Since NaOH is used to absorb the CO2, the mass of NaOH required to absorb 33.01 g of CO2 is also 33.01 g.
So, 33.01 grams of NaOH is required to absorb the whole CO2 produced in the reaction.