Question

1.0 moles of an ideal gas are held in a container under 2.0 atm of pressure and 310 K. What must be the volume of this container?

Answer 1

Answer: 12.7 L

Step-by-step explanation:

P=2.0atm

V= ???

n=1.0 mol

R= 0.0821

T= 310K

PV=nRT--> (2)V=(1)(0.0821)(310)

V=12.7 L

Answer 2

12.7 L (3 s.f.)

Step-by-step explanation:

Since it is an ideal gas, we can apply the ideal gas law:

`\boxed{pV=nRT}`

☆ where p= pressure

V= volume

n= number of moles

R= ideal gas constant

T= temperature

Substitute all the given information into the formula:

2V= 1(0.08206)(310)

2V= 25.4386

V= 25.4386 ÷2

V= 12.7 L (3 s.f.)

Further explanation:

The ideal gas constant, R, has different values depending on what units are being used. Two examples are listed below:

`• \: 0.08206 \: L \: atm ^( - 1) \: mol \: K`

`• \: 8.314 \: J \: {mol}^( - 1) \: {K}^( - 1)`

In the above question, we use the value 0.08206 because the pressure was given in atm and the temperature was given in Kelvin. Thus, the unit used for volume is L.