what mass of HCl is needed to decompose 50g of CaCO3
Assuming your reaction is
CaCO3 + 2HCl -> CaCl2 + H2O + CO2
then it will take two moles of HCl for each mole of CaCO3
So, how many moles of CaCO3 in 50g?
double that for HCl and figure the mass.
To determine the mass of HCl needed to decompose 50g of CaCO3, we need to first determine the balanced chemical equation for the reaction.
The balanced chemical equation for the reaction between HCl and CaCO3 is as follows:
CaCO3 + 2HCl -> CaCl2 + H2O + CO2
From the balanced chemical equation, we can see that 1 mole of CaCO3 reacts with 2 moles of HCl. We need to find the number of moles of CaCO3 in 50g.
To find the number of moles, we use the formula:
moles = mass / molar mass
The molar mass of CaCO3 can be calculated by adding up the individual atomic masses:
(1 * atomic mass of Ca) + (1 * atomic mass of C) + (3 * atomic mass of O)
Using the atomic masses from the periodic table, we get:
(1 * 40.08) + (1 * 12.01) + (3 * 16.00) = 100.09 g/mol
Now we can calculate the number of moles of CaCO3:
moles = 50g / 100.09 g/mol = 0.499 moles (approximately)
Since 1 mole of CaCO3 reacts with 2 moles of HCl, we need twice the number of moles of HCl. Therefore, we need:
2 * 0.499 moles = 0.998 moles of HCl
To find the mass of HCl needed, we use the formula:
mass = moles * molar mass
The molar mass of HCl is the sum of the atomic masses of hydrogen and chlorine:
(1 * atomic mass of H) + (1 * atomic mass of Cl) = 1.01 + 35.45 = 36.46 g/mol
Now we can calculate the mass of HCl needed:
mass = 0.998 moles * 36.46 g/mol = 36.40 g (approximately)
Therefore, approximately 36.40 grams of HCl is needed to decompose 50 grams of CaCO3.