Question

What is the pressure in mm Hg of a 0.025 mole sample of CO2 at 350k in a 2.00L container?

Answer 1

`273\text{ mmHg}`

Step-by-step explanation:

Here, we want to get the pressure in mmHg

Using the ideal gas equation:

`\begin{gathered} PV\text{ = nRT} \\ P\text{ = }(nRT)/(V) \end{gathered}`

Where:

P is the pressure in atm which we want to calculate (we would convert to mmHg after calculation)

n is the number of moles which is 0.025 mole

T is the temperature in Kelvin which is 350K

V is the volume which is 2L

R is the molar gas constant which is 0.0821 L.atm/mol.K

Substituting the values, we have it that:

`\begin{gathered} P\text{ = }(0.025*0.0821*350)/(2) \\ \\ P\text{ = 0.36 atm} \end{gathered}`

Finally, we have to convert this to mmHg

Mathematically:

`\begin{gathered} 1\text{ atm = 760 mmHg} \\ 0.36\text{ atm = 0.36 }*\text{ 760} \\ =\text{ 273 mmHg} \end{gathered}`