2. A cylinder with a moveable piston was a volume of 12.6 L when 30 moles of oxy
ID: 998124 • Letter: 2
Question
2. A cylinder with a moveable piston was a volume of 12.6 L when 30 moles of oxygen gas is added at a pressure of 5.83 atm. Over time the cylinder develops a small leak and the volume of the gas deceases to 12.1 L at the same pressure a. How many moles of oxygen were lost due to the leak? measures the pressure above the atmospheric that exists in the ball The ball is then used outside (not by the Patriots) at a temperature of - 7°C and feels 3. A ball is inflated inside at 25°C to a pressure of 8.0 psi using a pressure gauge The gauge (Note: atmospheric pressure 14.7 psi) flat What is the gauge pressure measured? What is the actual pressure inside the ball outside? a. b. A piece of dry ice (CO2 (s) with a mass of 22.50 g is placed into an evacuated 2.50 L container and sealed shut. (Note: freezing point of dry ice is -109.3°F) 4. a. What is the pressure inside the flask at a temperature of -4°C? 5. Complete the following table for dinitrogen tetroxide gas: Volume Temp A 1.77 atm 4.98L 43.1°C 912°C Temp Moles 0.783 0.166 Pressure 673 mmm Hg | 488 ml 6.25 C 0.899 bar 0899 bar-15L 39E 1.15 39°FExplanation / Answer
Post multiple questions to get the remaining answers
Q2)
Using ideal gas equation, PV = nRT
Since the pressure and temperature remains constant, hence we get
V1/n1 = V2/n2
12.6/3 = 12.1/n2
n2 = 2.8809 moles
Moles of oxygen leaked = 3 - 2.8809 = 0.1190 moles
3)
a) Using ideal gas equation PV = nRT
P1/T1 = P2/T2
8/(273+25) = P2/(273-7)
P2 = 7.248 psi
b) Actual Pressure inside the ball = atmospheric pressure + P2
=> 14.7 + 7.248
=> 21.948 psi
4)
Using ideal gas equation
PV = nRT
molar mass of CO2 = 12 + 2*16 = 44 gm/mol
Number of moles of CO2 = 22.5/44 = 0.51136 moles
P(2.50) = 0.51136 * 0.0821 * (273-4)
P = 4.517 atm
Related Questions
Navigate
Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.