Question

4.39 moles of gas in a box has a pressure of 2.25 atm at temperature of 385K. What is the volume of the box?
Make sure to put P,V,and T in the right units)

(Unit=m^3)

Answer 1

Answer:

0.0619 m^3

Explanation

number of moles = n = 4.39 mol

pressure = P = 2.25 atm =2.25×1.01×10^5 Pa= 2.27×10^5 Pa

Molar gas constant =R = 8.31 J/(mol K)

Temperature T= 385K

volume of gas = V =?

BY GENERAL GAS LAW WE HAVE

PV = nRT

or V = nRT/P

or V = (4.39×8.31×385)/(2.27×10^5)

V = 0.0618728

V =  0.0619 m^3

Answer 2

Answer:

Volume of the container = 0.0618 m³

Explanation:

Assuming that the gas is ideal, we can apply ideal gas equation:

PV=nRT

where P = pressure of the gas

          V = volume occupied by the gas

          n =  number of moles of gas

          R = Universal gas constant = 8.314 J/mol-K

          T = Temperature of the gas

Here we have to find volume.

Given: P=2.25 atm T=385 K n=4.39 moles

Putting the above values in the ideal gas equation, we get:

$V=\frac{nRT}{P}=\frac{4.39\times8.314\times385}{2.25\times1.01\times10^{5}}=0.0618\ m^3$

Volume of the gas = volume of the container in which it is filled = 0.0618 m³