Pleaese i need help!! Thanks Pleaese i need help!! Thanks 1 PnkI in all its poss
ID: 545939 • Letter: P
Question
Pleaese i need help!! ThanksPleaese i need help!! Thanks
1 PnkI in all its possible uses. Here are a few examples of the many possible A. A sample of Argon gas occupies a 1.5 L cylinder at a temperature of 22 °C. The cylinder has a pressure of 125 atm. How many moles of argon occupy the cylinder? B. A 5.0 L cylinder is filled with 34.0 moles of nitrogen gas at 293 °C, calculate the pressure in the cylinder in atm. C. High pressure chemistry is conducted in a vessel commonly called a "bomb". A 1.25 L bomb is pressurized to 1,500 psi and sealed room temperature (23 °C). If the temperature is raised to 450 oC, what is the final pressure in psi and atm. D. A gas filled balloon having a volume of 2.50 L at 1.2 atm and 25 °C is allowed to rise to the stratosphere (about 30 km above the surface of the Earth), where the temperature and pressure is -23 °C and 3.00 × 10-3 atm, respectively. Calculate the final volume of the balloon. E. If I have a sealed steal cylinder containing an inert gas and I increase the pressure what effect will this have?
Explanation / Answer
14.
A.
V = 1.5 L
T = 22 oC = 273 + 22 K = 295 K
P = 125 atm
R = 0.082 L atm mol-1 K-1
Now,
PV = nRT
n = PV/RT
= [ (125 atm) (1.5 L) ] / [ (0.082 L atm mol-1 K-1) (295 K) ]
= 7.75113683 mol
B.
V = 5.0 L
n = 34.0 mol
T = 293 oC = (273 + 293) K = 566 K
P = ?
R = 0.082 L atm mol-1 K-1
Now,
PV = nRT
P = nRT/V
= [ (34.0 mol) (0.082 L atm mol-1 K-1) (566 K) ] / (5.0 L)
= 315.60 atm
C.
PV = nRT
We know that, at constant volume
P1/T1 = P2/T2
P1 = 1500 psi
T1 = 23 oC = (273 + 23) K = 296 K
P2 = ?
T2 = 450 oC = (273 + 450) K = 723 K
Now,
P1/T1 = P2/T2
P2 = P1T2/T1
= [ (1500 psi) (723 K) ] / (296 K)
= 3664 psi
1 psi = 0.068046 atm
3664 psi = 3664 x 0.068046 atm
= 249 atm
D.
PV = nRT
We know that,
P1V1/T1 = P2V2/T2
P1 = 1.2 atm
V1 = 2.50 L
T1 = 25 oC = (273 + 25) K = 298 K
P2 = 3.00 x 10-3 atm = 0.003 atm
V2 = ?
T2 = - 23 oC = (273 - 23) K = 250 K
Now,
P1V1/T1 = P2V2/T2
[ (1.2 atm) (2.50 L) / (298 K) ] = [ (0.003 atm) V2 / (250 K) ]
0.0100671141 L = 0.000012 x V2
V2 = (0.0100671141 L) / (0.000012)
= 839 L
E.
PV = nRT
It’s a sealed tube, so V = constant
Now, in the equation,
PV = nRT
V, n and R are constant.
So, if we increase the pressure, the temperature will raise.