Question

3.27 moles of an ideal gas has a pressure of 125000 Pa at 15.0 ° C What is the volume of the gas?

Answer 1

15.96 m³ (corrected to 2 d.p.)

Step-by-step explanation:

Using idea gas law:

pV = nRT

pressure p = 125000 Pa

volume V = unknown

no. of moles n= 3.27 moles

ideal gas constant R = 8.3145 J K−1 mol−1

Temperature t (in Kelvins) = 15 + 273.15 = 288.15K

125000 x v = 3.27 x 8.3145 x 288.15

v = 15.96 m³ (corrected to 2 d.p.)

Answer 2

0.0626 m^3

Step-by-step explanation:

First, we know that the equation to calculate the behavior of gases is:

PV=nRT

Looking at the problem, we understand that we are needing to solve for V, which means we need to isolate V to solve for it.

The new equation will look something like this:

V=nRT/P

The last step is to simply plug in the remaining variables:

n=3.27

R=8.31 (that is not given but is a standard number that you will always use for "R"/ the ideal gas constant-it helps to right it down somewhere to reference it if you ever need it!)

P=125000

T=288 (the temp needs to be in degrees K, so take 15.0 degrees c and + 273)

Finally, when you input all of those, you will have something that looks like this:

V=(3.27*8.31*288)/125000

V=0.02608205 m^3

V= 0.0626 m^3 (rounded to 3 sig. figs)

I hope this was helpful and easy to understand!