In: Chemistry
Which of these gases, if any, is behaving ideally?
Gas I. A 0.357-mol sample takes up 10.2 L at STP.
Gas II. Under 85.5 mmHg of pressure and at 258 K, a full 23.0 L
container holds 0.140 moles of gas.
Gas III. At 50.0 °C, a 75.0 L container holds 6.70 moles of gas
under 240. kPa of pressure.
Gas I only |
Gas II only |
Gas III only |
None of these gases are behaving ideally. |
gas 1) Using ideal gas equation ,PV=nRT
n/V=P/RT
n=mol of gas=0.357 mol
Volume=V=10.2L
R=universal gas constant=0.0821L atm/Kmol
standard T=273K
std P=1atm
So for ideal gas( P/RT)ideal=1atm/(0.0821Latm/K.mol)*273K=0.0446 mol/L
for given gas ,n/V=0.357mol/10.2L=0.035 mol/L=P/RT is not equal to (P/RT)ideal.So it is not ideal
gas ll
P1=85.5 mmhg=85.5mmhg/760mmhg/atm=0.112 atm
V1=23.0L
T1=258K
at STP,
P2=1 atm
T2=273K
V2=22.4L
P1V1/T1=0.112 atm*23L/258K=0.01 atmL/K=nR
for ideal gas,p2V2/T2=1atm*22.4L/273K=0.0821 atm/LK
As P1V1/T1 is not equal to P2V2/T2 ,gas 2 is not ideal
gas lll) At 50.0 °C, a 75.0 L container holds 6.70 moles of gas under 240. kPa of pressure.
T1=50+273=323K
P1=240KPa*(1 atm/101.325 kpa)=2.369 atm
V1=75L
n=6.7mol
R=PV/nT=2.369atm*75L/6.7mol*323K=0.0821 Latm/K.mol
R(ideal)=1atm*22.4L/1mol*273K=0.0821Latm/K.mol
Rgas=R(ideal) so this gas is behaving ideally
Answer:gas lll is behaving ideally