A sample of calcium carbonate that has a mass of 1.0 g is heated and completely decomposed-calculate.

a) the mass of carbon dioxide produced
b)the volume of carbon dioxide at SLC
c)the volume of carbon dioxide at STP

CaCO3 ==> CaO + CO3

mols CaCO3 = 1.0g/molar mass CaCO3.
Convert mols CaCO3 to mols CO2 using the coefficients in the balanced equation.

a. convert mols CO2 to volume CO2 at STP knowing 1 mol gas occupies 22.4L at STP
b. Do the same with 1 mol occupies 24.5 L at SLC

hjkl

To calculate these values, we need to know the molar mass of calcium carbonate, the balanced chemical equation for its decomposition, and the molar volume of a gas at standard temperature and pressure (STP) or standard liters per mole (SLC).

a) Calculate the mass of carbon dioxide produced:
1. Determine the molar mass of calcium carbonate (CaCO3):
- Calcium (Ca) has a molar mass of 40.08 g/mol.
- Carbon (C) has a molar mass of 12.01 g/mol.
- Oxygen (O) has a molar mass of 16.00 g/mol.
Thus, the molar mass of CaCO3 is: 40.08 g/mol + 12.01 g/mol + (16.00 g/mol × 3) = 100.09 g/mol.

2. Calculate the number of moles of calcium carbonate:
Mass of calcium carbonate = 1.0 g
Moles of calcium carbonate = 1.0 g / 100.09 g/mol = 0.009998 moles (rounded to 4 decimal places).

3. According to the balanced chemical equation, 1 mole of calcium carbonate produces 1 mole of carbon dioxide.
Therefore, the number of moles of carbon dioxide produced is also 0.009998 moles.

4. Calculate the mass of carbon dioxide produced:
Mass of carbon dioxide = Number of moles × molar mass of carbon dioxide
Mass of carbon dioxide = 0.009998 moles × 44.01 g/mol (molar mass of carbon dioxide)
Mass of carbon dioxide = 0.4400 g (rounded to 4 decimal places).

b) Calculate the volume of carbon dioxide at SLC (standard liters per mole):
The volume of 1 mole of any gas at standard temperature (0 °C or 273.15 K) and pressure (1 atm) is 22.4 L/mol.

Volume of carbon dioxide at SLC = Number of moles × molar volume at SLC
Volume of carbon dioxide at SLC = 0.009998 moles × 22.4 L/mol
Volume of carbon dioxide at SLC = 0.2241 L (rounded to 4 decimal places).

c) Calculate the volume of carbon dioxide at STP (standard temperature and pressure):
The volume of 1 mole of any gas at STP (0 °C or 273.15 K and 1 atm) is 22.7 L/mol.

Volume of carbon dioxide at STP = Number of moles × molar volume at STP
Volume of carbon dioxide at STP = 0.009998 moles × 22.7 L/mol
Volume of carbon dioxide at STP = 0.2270 L (rounded to 4 decimal places).

Thus, the answers to the questions are:
a) The mass of carbon dioxide produced is 0.4400 g.
b) The volume of carbon dioxide at SLC is 0.2241 L.
c) The volume of carbon dioxide at STP is 0.2270 L.

To calculate the mass of carbon dioxide produced, we need to use the balanced chemical equation for the decomposition of calcium carbonate, which is:

CaCO3(s) -> CaO(s) + CO2(g)

The molar mass of calcium carbonate (CaCO3) is approximately 100.1 g/mol.

a) Mass of carbon dioxide produced:
According to the balanced chemical equation, 1 mole of calcium carbonate produces 1 mole of carbon dioxide.
Therefore, we can calculate the number of moles of calcium carbonate by dividing the mass of calcium carbonate (1.0 g) by its molar mass (100.1 g/mol):

Number of moles of calcium carbonate = 1.0 g / 100.1 g/mol = 0.00999 mol (approximately)

Since 1 mole of calcium carbonate produces 1 mole of carbon dioxide, the mass of carbon dioxide produced is also equal to 0.00999 mol.

The molar mass of carbon dioxide (CO2) is approximately 44.01 g/mol.

Mass of carbon dioxide produced = 0.00999 mol * 44.01 g/mol = 0.4399 g (approximately)

Therefore, the mass of carbon dioxide produced is approximately 0.44 g.

b) To calculate the volume of carbon dioxide at standard temperature and pressure (STP), we need to use the ideal gas law, which states that:

PV = nRT

Where:
P = pressure (atm)
V = volume (L)
n = number of moles
R = ideal gas constant (0.0821 L.atm/mol.K)
T = temperature (K)

At standard temperature and pressure (STP), the pressure is 1 atm, and the temperature is 273 K.

First, we need to calculate the number of moles of carbon dioxide produced using the same calculation as in part (a):

Number of moles of carbon dioxide = 0.00999 mol

Using the ideal gas law, we can calculate the volume of carbon dioxide at STP by rearranging the equation:

V = (nRT) / P

V = (0.00999 mol * 0.0821 L.atm/mol.K * 273 K) / 1 atm

V = 0.2255 L (approximately)

Therefore, the volume of carbon dioxide at STP is approximately 0.23 L.

c) However, if you meant standard laboratory conditions (SLC) rather than standard temperature and pressure (STP), the temperature would be 298 K instead of 273 K.

Using the same formula as in part (b), the volume of carbon dioxide at SLC would be:

V = (0.00999 mol * 0.0821 L.atm/mol.K * 298 K) / 1 atm

V = 0.2417 L (approximately)

Therefore, the volume of carbon dioxide at SLC is approximately 0.24 L.