Need help with these few questions... A sample of argon gas is at a pressure of 1.24...?

Question

1. A sample of argon gas is at a pressure of 1.24  104 kPa and a temperature of
24C in a rigid 25-L tank. How many moles of argon does this tank contain?
2. A 35.0-L tank contains 7.00 mol of compressed air. If the pressure inside the
tank is 500.0 kPa, what is the temperature of the compressed gas?
3. How many grams of helium does a 25.0-L balloon contain at 102.0 kPa and
24C?
4. Calculate the volume that 2.25 mol of O2(g) will occupy at STP.

Dr.A · Accepted Answer

1.24 x 10^4 kPa = 122.4 atm

122.4 atm x 25 L / 0.08206 x 297 K = 125 atm

500 kPa = 4.93 atm
T = 4.93 x 35.0 / 0.08206 x 7.00=300.6 K => 27.6 °C


102 kPa = 1.0 atm
moles He = 1.0 x 25.0/ 0.08206 x 297 K=1.0
mass He = 1.0 mol x 4.0 g/mol= 4.0 g

V = 2.25 x 22.4 =50.4 L

wedel · Answer

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Need help with these few questions... A sample of argon gas is at a pressure of 1.24...?

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