Solve for n in PV=nRT
2.79*10^5(3.66)=n×8.314462175×(19.8+273.15)
to get
419 moles (3 sig. figures)
and similarly solve for P in
P(7.20)=419.235(8.314462175)(28.5+273.15)
to get 1.46*10^5 (3 sig. figures)
Your approach is correct, but cannot tell where you got wrong without seeing your calculations.
An ideal gas at 19.8 °C and a pressure of 2.79 x 105 Pa occupies a volume of 3.66 m3. (a) How many moles of gas are present? (b) If the volume is raised to 7.20 m3 and the temperature raised to 28.5 °C, what will be the pressure of the gas?
I got a) right with 419.46, but im stuck on part b) I replaced T with 301.65(converted to Kelvin) and V with 7.20 but I got 3689.3 which is wrong. Where did I go wrong ?
1 answer