A sample of 3.2 moles of N2 gas is being held in a container that has a volume of 2.4 L. ?

Question

If the temperature is 28oC, what is the pressure in the container?

Answer 1

PV = nRT

P = nRT / V = (3.2)(0.0821)(301) / 2.4 = 33 atm

Answer 2

ok, so from the information given in the question you know that...

V=2.4L

n=3.2 mols

R=.0821L*atm / K*mol  (constant R value)

T=28C

P=?

The equation you must use for this is The Ideal Gas Law, which is PV=nRT

There is a problem though. First you have to convert the temperature, which is in degrees celsius to Kelvin by adding 28C+273K= 301K

Your new temperature is 301K

Since you want to solve for the pressure, you have to do some manipulation to the equation. After the manipulation your equation will look like this:

nRT/ V= P

You do some plug and chuck...

(3.2mols)(.0821L*atm/ K*mol)(301K) / 2.4L= 32.94atm

Meaning that the pressure in the container is 32.94atm

Answer 3

ideal gas law: PV=nRT

    P is the absolute pressure (SI unit: pascal)

    V is the volume (SI unit: cubic metre)

    n is the amount of substance (loosely number of moles of gas)

    R is the ideal gas constant (SI: 8.3145 J/(mol K))

    T is the thermodynamic temperature (SI unit: kelvin).