Question

Given 10g of carbon dioxide at STP what volume would you have?

Answer 1

1) List the known and unknown quantities.

Sample: Carbon dioxide (CO2)

Mass: 10 g

STP means standard temperature and pressure.

Temperature: 273.15 K.

Pressure: 100000 Pa = 0.986923 atm

Ideal gas constant: 0.082057 L * atm * K^(-1) * mol^(-1)

2) Set the equation.

$PV=nRT$

2.1- Convert g of CO2 to moles of CO2.

The molar mass of CO2 is 44.0095 g/mol.

$mol\text{ }CO_2=10\text{ }g\ast\frac{1\text{ }mol\text{ }CO_2}{44.0095\text{ }g\text{ }CO_2}$$mol\text{ }CO_2=0.2272$

3) Plug in the known quantities in the ideal gas equation and solve for V (liters).

$(0.986923\text{ }Atm)(V)=(0.2272\text{ }mol\text{ }CO_2)(0.082057\text{ }L\ast atm\ast K^{-1}\ast mol^{-1})(273.15\text{ }K)$$V=\frac{(0.2272molCO_2)(0.082057\text{ }L\ast atm\ast K^{-1}mol^{-1})(273.15K)}{0.986923\text{ }atm}$$V=5.15991\text{ }L$

10g CO2 would occupy 5.2 L.

Volume: 5.2 L.

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