Respuesta :
Step 1
Gases are assumed to be ideal. Therefore, it is used:
p x V = n x R x T
p = pressure = 744.8 torr (1 atm = 760 torr) => 744.8 torr x (1 atm/760 torr) = 0.98 atm
T = absolute temperature = 36.01 °C + 273 = 309.01 K
V = volume
R = gas constant = 0.082 atm x L/mol x K
n = number of moles = mass/molar mass = m/M
-----------------------
Step 2
p x V = n x R x T can be written as:
[tex]\begin{gathered} p\text{ x V = }\frac{m}{M}\text{ x R x T} \\ p\text{ = }\frac{m}{VxM}xRxT \\ p\text{ = }\frac{m}{V}x\text{ }\frac{RxT}{M} \\ Clear\text{ M and m/V = density:} \\ M=density\text{ x }\frac{RxT}{p} \\ M\text{ = 6.607 g/L x }\frac{0.082\text{ atm x L/mol x K x 309.01K}}{0.98\text{ atm}} \\ \end{gathered}[/tex]Answer: Molar mass = 170.83 g/mol
