A sample of gas has a mass of 0.311 g. Its volume is 0.225 L at a temperature of 55 °C and a pressure of 886 mm Hg. Find its molar mass.
GIVEN:
m = 0.311 g
V = 0.225 L
t = 55 °C
P = 886 mm Hg
FIND: Molar mass (g/mol)
RELATIONSHIPS USED
PV = nRT (Ideal gas law, presented in this section)
Molar mass = \frac{\operatorname{Mass}\left(m\right)}{\operatorname{Moles}\left(n\right)} (Definition of molar mass from Section 6.3)
PV = nRT
n\,=\,{\frac{P V}{R T}} \\ P\,=\,886\,\cancel{\mathrm{mm}\,\mathrm{Hg}}\times\frac{1\,\mathrm{atm}}{760\,\cancel{\mathrm{mm}\,\mathrm{Hg}}}\,=1.1\underline{6}58 atmT = 55 °C + 273 = 328 K
n=\frac{1.1\underline{6}58\,\,\cancel{\mathrm{atm}} \times 0.225 \cancel{L}}{0.0821\,\frac{{ \cancel{L}}\cdot{\cancel {atm}}}{{\cancel mo l}\cdot{\cancel{ K}}}\,\,\times\,328\,\,{\cancel{K}}}= 9.7\underline{4}06 × 10^{-3} mol
Molar mass = \frac{\operatorname{Mass}\left(m\right)}{\operatorname{Moles}\left(n\right)} \\ =\;\frac{0.311 g}{9.7\underline{4}06}\times10^{-3}\,\mathrm{mol}
= 31.9 g/mol