Dr. Swartling places 270 mL of liquid nitrogen at its boiling temp into a 1.000

Question

Dr. Swartling places 270 mL of liquid nitrogen at its boiling temp into a 1.000 Liter plastic Coke bottle and caps the bottle. If all the liquid were able to convert to gas and warm to 20.0 degrees Celsius without the bottle exploding, what would be the pressure of the gas in atm, assuming ideality? (You may neglect the air that was originally in the bottle.)

To what temperature in Celsius must a sample of ammonia gas be cooled from 20.00 degrees Celsius to reduce its volume from 4.00 L to 200 mL? (assume ideality)

Explanation / Answer

Let initial of Ammonia be p1 atm, V1 = 4000 mL, T1 = 273+20=293 K

Also, p2 atm, V2 = 200 mL, T2=?

Assuming ideal behaviour, we have

p1v1/ n1RT1 = p2v2/n2RT2

Now,

V1/T1 = V2/T2

Therefore,

T2 = 200*293/4000 = 14.65 K.

Answer 1.

Now,

Let initial of Liquid Nitrogen be p1 = 1 atm, V1 = 270 mL, T1 = 77.2 K

Also, p2 = ? atm, V2 = 1000 mL, T2= 293

Assuming ideal behaviour, we have

p1v1/ n1RT1 = p2v2/n2RT2

Hence, p2 = 1*270*293/1000*77

Therefore,

p2 = 1.027 atm.

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