Question

If 500 g of carbon disulfide burns in the presence of oxygen to produce carbon dioxide and sulfur dioxide, how many liters of sulfur dioxide collected over water measured at 27°C and 740-mmHg, are produced?

Answer 1

$CS_2 + 3O_2 \rightarrow CO_2 + 2SO_2$

Find moles of $SO_2$

$500 g CS_2 (\frac{1 mole CS_2}{76.14 g CS2})(\frac{2 moleSO_2}{1 mole CS_2}) = 13.1 mol SO_2$

Use Ideal Gas Law to find the volume of $SO_2$

$PV = nRT$

$V =\frac{nRT}{P}$

$n=13.1 mol$

$T(K) = 273 + 27 = 300 K$

$P(atm) = 740 mm Hg (\frac{1 atm}{760 mm Hg})= 0.974 atm$

$R = 0.0821 \frac{L\times atm}{mol\times K}$

$V = \frac{13.1\times 0.0821 \times 300}{0.974} = 331 L$