How many liters of carbon dioxide are formed from the complete decomposition of 50.0 g of iron (III) carbonate at STP?

V = 1.57 L

Explanation:

Given data:

Mass of iron(III) carbonate = 50.0 g

Volume of CO₂ formed = ?

Temperature = standard = 273 K

Pressure = standard = 1 atm

Solution:

Chemical equation:

Fe₂(CO₃)₃     → Fe₂O₃ + 3CO₂

Number of moles of Fe₂(CO₃)₃ :

Number of moles = mass/molar mass

Number of moles = 50.0 g /235.8 g/mol

Number of moles = 0.21 mol

Now we will compare the moles of Fe₂(CO₃)₃  and CO₂.

                          Fe₂(CO₃)₃         :             CO₂

                              1                    :               3

                            0.21                :            1/3×0.21 = 0.07 mol

Volume of CO₂:

PV = nRT

R = general gas constant = 0.0821 atm.L/mol.K

By putting values,

1 atm × V =0.07 mol × 0.0821 atm.L/mol.K × 273 K

V = 1.57 atm.L / 1 atm

V = 1.57 L

particle   p is an electron and particle q is a neutron