1.)To prevent tank rupture during deep-space travel, an engineering team is stud
ID: 919726 • Letter: 1
Question
1.)To prevent tank rupture during deep-space travel, an engineering team is studying the effect of temperature on gases confined to small volumes. What is the pressure of 4.00 mol of gas D measured at 251 C in a 1.75-L container assuming real behavior?
2.) A 1.15 g sample of dry ice is added to a 750 mL flask containing nitrogen gas at a temperature of 25.0 C and a pressure of 735 mmHg . The dry ice is allowed to sublime (convert from solid to gas) and the mixture is allowed to return to 25.0 C.What is the total pressure in the flask?
Explanation / Answer
P = [(RT)/(Vm - b)] - [a/(Vm)^2]
Vm = is the molar volume = V/n
R gas constant = 0.0821 L atm/ K mol
T = 251 C = (251 + 273) K = 524 K
Vm = 1.75 L / 4 mol = 0.4375 mol/L
a and b are given , a = 1.46(L2.atm/mol2) , b = 0.0373 (L/mol)
So the pressure is
P = [(RT)/(Vm - b)] - [a/(Vm)^2] ,
P = [(0.0821 x 524 )/ (0.4375 - 0.0373)] - [1.46 /0.1914]
P = 99.87 atm
Pressure = 99.87 atm
2)
P = 735 mmHg = 0.967 atm
V = 0.75 L
T = 25 + 273 = 298 K
P V = n RT
0.967 x 0.75 = n x 0.0821 x 298
n = 0.0296
moles of CO2 = mass / molar mass of CO2
= 1.15 / 44
= 0.0261
total moles CO2 = 0.0296 + 0.0261
= 0.0557 mol
Now use the ideal gas equation agian to determine the pressure the new number of moles of CO2 will result in.
P V = n RT
P x 0.75 = 0.0557 x 0.0821 x 298
P = 1.817 atm
total pressure = 1381 mmHg
Related Questions
Navigate
Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.