A 211 g sample of barium carbonate, BaCO3,

reacts with a solution of nitric acid to give bar- ium nitrate, carbon dioxide and water. If the acid is present in excess, what mass and volume of dry carbon dioxide gas at STP will be produced

BaCO3 + 2HNO3 ==> H2O + CO2 + Ba(NO3)2

mols BaCO3 = grams/molar mass
Using the coefficients in the balanced equation convert mols BaCO3 to mols CO2.
Now convert mols CO2 to grams. g = mols x molar mass.
Convert mols CO2 to L. L = mols x 22.4.

To determine the mass and volume of dry carbon dioxide gas (CO2) produced when reacting 211 g of barium carbonate (BaCO3) with excess nitric acid, you need to use stoichiometry, which involves converting from mass of the reactant to the moles of the reactant, and then using the balanced chemical equation to determine the moles of the product (CO2). Finally, you can convert the moles of CO2 to mass and volume at standard temperature and pressure (STP).

1. Calculate the moles of BaCO3:
- Look up the molar mass of BaCO3:
Ba: 1 x 137.33 g/mol = 137.33 g/mol
C: 1 x 12.01 g/mol = 12.01 g/mol
O: 3 x 16.00 g/mol = 48.00 g/mol
- Add up the molar mass:
Molar mass of BaCO3 = 137.33 g/mol + 12.01 g/mol + 48.00 g/mol = 197.34 g/mol
- Convert grams of BaCO3 to moles:
Moles of BaCO3 = Mass of BaCO3 / Molar mass of BaCO3
= 211 g / 197.34 g/mol

2. Use the balanced chemical equation to determine the stoichiometric ratio between BaCO3 and CO2:
The balanced chemical equation for the reaction is:
BaCO3 + 2 HNO3 -> Ba(NO3)2 + CO2 + H2O
From the equation, the stoichiometric ratio between BaCO3 and CO2 is 1:1. This means that for every 1 mole of BaCO3, 1 mole of CO2 is produced.

3. Calculate the moles of CO2 produced:
Moles of CO2 = Moles of BaCO3 (from step 1) x Stoichiometric ratio (1 mole CO2 / 1 mole BaCO3)

4. Use the ideal gas law to calculate the volume of CO2 at STP:
The ideal gas law equation is:
PV = nRT
Where:
P = Pressure (STP = 1 atm)
V = Volume
n = Moles of gas
R = Ideal gas constant (0.0821 L⋅atm/(K⋅mol))
T = Temperature (STP = 273.15 K)

Rearranging the equation to solve for V, we get:
V = nRT / P

Substituting the values:
V = (Moles of CO2) x (R constant) x (Temperature in Kelvin) / (Pressure)

Since it's STP, we plug in the values:
V = (Moles of CO2) x (0.0821 L⋅atm/(K⋅mol)) x (273.15 K) / (1 atm)

5. Calculate the mass of CO2 produced:
Mass of CO2 = Moles of CO2 (from step 3) x Molar mass of CO2
= Moles of CO2 x (Molar mass of C + (2 x Molar mass of O))
= Moles of CO2 x (12.01 g/mol + 2 x 16.00 g/mol)

Finally, plug in the calculated values from steps 1, 3, 4, and 5 to find the mass and volume of dry CO2 gas produced at STP.