Carbon dioxide, when it is at -145 degreesC has a density of 2.54 g/L. What is the pressure in torr??

The pressure in torr is 461 torr

Explanation:

To calculate the relation of density and molar mass of a compound, we use the ideal gas equation:

PV=nRT

P = pressure

V = Volume

n = number of moles

R = gas constant = 0.0821 Latm/Kmol

T = temperature =

Number of moles (n) can be written as:

where, m = given mass

M = molar mass  = 44 g/mol

where,

where d = density = 2.54 g/L

The relation becomes:

PM=dRT  

   (760torr=1atm)

Thus the pressure in torr is 461 torr