Chemistry
posted by Anonymous on .
What is the pressure, in torr, of a gas whose density is 8.0 g/L at a temperature of 25 C above standard temperature and whose molecular weight is 75 g/mol?

Use the gas law and solve for the pressure:
PV=nRT
Where
n=moles of gas
L=volume
R=62.3637 L·Torr/mol·K
and
T=273.15K + 25 C=298.15K
The density of the gas is 8.0g/L and the molecular weight of the gas is 75 g/mol
8.0g//75g/mol= x mol/L
Rearrangement of the gas law gives the following:
P=(n/V)*RT
Plug in x mol/L into the equation and plug and chug. 
**Fixed a typo that probably would cause confusion.
Use the gas law and solve for the pressure:
PV=nRT
Where
n=moles of gas
L=volume
R=62.3637 L·Torr/mol·K
and
T=273.15K + 25 C=298.15K
The density of the gas is 8.0g/L and the molecular weight of the gas is 75 g/mol
8.0g/L**/75g/mol= x mol/L
***This leaves mol/L
Rearrangement of the gas law gives the following:
P=(n/V)*RT
Plug in x mol/L into the equation and plug and chug.