If 32.5 mol of an ideal gas occupies 61.5 L at 47.00 ∘C, what is the pressure of the gas?

You will need to use the Ideal Gas Law to solve this problem:

P

V

=

n

R

T

Explanation:

To find pressure

(

P

)

, derive from the Ideal Gas Law:

P

=

n

R

T

V

Gather up your known values, and plug them into the equation.

There are a few points to make here, Temperature

(

T

)

must be converted to Kelvin.

R

= Ideal Gas Constant. This can have many forms. The one I used below is the one that I am most familiar with. Be aware of this though, and check which value you should be using per your curriculum.

n

=

91.5

m

o

l

V

=

69.5

L

T

=

31.0

°

C

+

(

273.15

K

)

=

304.15

K

R

=

8.314

J

m

o

l

⋅

K

Finally,

P

=

(

91.5

m

o

l

)

(

8.314

J

m

o

l

⋅

K

)

(

304.15

K

)

69.5

L

P

=

(

x

)

a

t

m

Explanation:

the formula for the conversion of temperature from degree celsius to kelvin is:

the sample of water at is converted to kelvin temperature by using the above formula as:

on comparing the two samples of water at or we can say that at and at respectively. the difference between the temperatures of two samples of water is:

hence, one can say that the sample of water at is greater than the sample of water at by .