Solution: we can solve the problem by using the ideal gas law, which states: [tex]pV=nRT[/tex] where p is the gas pressure V its volume n the number of moles R the gas constant T the absolute temperature
Before using this equation, we have to convert the temperature in Kelvin: [tex]T=32^{\circ}C+273 = 305 K[/tex] and the volume in [tex]m^3[/tex]: [tex]V=2.92 L= 2.92 dm^3 = 2.92 \cdot 10^{-3} m^3[/tex]
So now we can re-arrange the ideal gas equation to find the pressure exerted by the gas, p: [tex]p= \frac{nRT}{V}= \frac{(2.50 mol)(8.31 J/mol K)(305 K)}{2.92 \cdot 10^{-3} m^3}= 2.17 \cdot 10^7 Pa[/tex]
