Answer: The pressure of the gas comes out to be [tex]1.45\times 10^2atm[/tex]
Explanation:
To calculate the pressure of the gas, we use the equation given by ideal gas equation, which is:
[tex]PV=nRT[/tex]
where,
P = Pressure of the gas = ? atm
V = Volume of the gas = 500 mL = 0.5 L (Conversion factor: 1 L = 1000 mL)
n = Number of moles of gas = 2.91 moles
R = Gas constant = [tex]0.0821\ttext{ L atm }mol^{-1}K^{-1}[/tex]
T = Temperature of the gas = [tex]31^oC=[273+31]K=304K[/tex]
Putting values in above equation, we get:
[tex]P\times 0.5L=2.91mol\times 0.0821\text{ L atm }mol^{-1}K^{-1}\times 304K\\\\P=145.2atm=1.45\times 10^2atm[/tex]
Hence, the pressure of the gas comes out to be [tex]1.45\times 10^2atm[/tex]
