Each of these flasks contains the same number of gas molecules. In which would t
ID: 528795 • Letter: E
Question
Each of these flasks contains the same number of gas molecules. In which would the pressure be lowest? A. Flask 1 B. Flask 2 C. Flask 3 D. Flask 4 Neon gas has a volume of 2,000ml with an atm of 1.8 however the pressure decreased to 1.3atm what is now the volume of the neon gas? A. 2, 795mL, B. 2, 769mL, C. 3, 795mL, D. 3, 759mL, Each of these flasks is the same size and at the same temperature. Which one contains the most molecules? A. Flask 1 B. Flask 2 C. Flask 3 D. Flask 4 When a supply of hydrogen gas is held in a 4 liter container at 320 K it exerts a pressure of 800 torr. The supply is moved to a 2 liter container, and cooled to 160 K. What is the new pressure of the confined gas? A. 800 torr B. 1600 torr C. 200 torr D. 400 torr A small sample of helium gas occupies 6 mL at a temperature of 250 K. At what temperature does the volume expand to 9 mL? A. 125K B. 375K C. 500K. D. 2250KExplanation / Answer
14) Answer : Flask 4
P = nRT/V
Since, n & V are constant, P T ,
Therefore, higher the temperature higher the pressure.
15) At constant temperature; P1V1 = P2V2
P1 = 1.8 atm; V1 = 2000 mL; P2 = 1.3 atm and V2 = ?
P1V1 = P2V2
V2 = (1.8 atm x 2000 mL) / (1.3 atm) = 2769 mL
Answer : B
16) Each flask is same volume and temperature . The pressure is different.
So, according to ideal gas law; PV = nRT
Therefore, pressure P n;
So, more the pressure more the number of moles/more the molecules.
Therefore, Flask 4 contains more no. of molecules.
Answer: D
17) P1 = 800 torr; V1 = 4 L and T = 320 K
P2 = ? ; V2= 2L ; T = 160 K
P1V1/T1 = P2V2/T2
P2 = (800torr x 4L/320 K )(160 K /2L) = 800 torr
Answer : 800 torr
19) V1 = 6 mL ; T1 = 250 K
V2 = 9 mL ; T2 = ?
V1/T1 = V2/T2 (at constant pressure)
T2 = (V2/V1)T1 = (9 mL /6 mL) x 250 K = 375 K
Answer: B
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