Posted by **Anonymous** on Tuesday, May 13, 2014 at 9:48pm.

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?

- Chemistry -
**Devron**, Tuesday, May 13, 2014 at 10:13pm
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.

- Chemistry-Typo Fix -
**Devron**, Tuesday, May 13, 2014 at 10:15pm
**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.

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