A 161.8 L take of an ideal gas is stored at 7.6 °C and 19.0 atm. 1)How many mole

Question

A 161.8 L take of an ideal gas is stored at 7.6 °C and 19.0 atm.

1)How many moles of gas are in the tank?

2)If the gas is He (atomic weight 4), what is the mass of the gas (in kg)?

3)If 736.2 L of this gas are used at 77.4 °C, and 1 atm, how many moles are left in the tank.

4)If the tank springs a leak and the pressure drops. When the pressure is at equilibrium, how many moles remain int he tank?( hint:Assuming the tank is on the surface of the earth, what pressure would be in the tank at equilibrium?)

5)Finally, the tank cooling system fails, and the temperatures rises to 32.6 °C. How many moles of gas are left?

I need 4,5. I already know first 3.

Explanation / Answer

considering 4) and 5) to be independent questions

4) After leakage T2 remains same and the final pressure becomes P2= 1 atm

as V1=V2

Applying PV=nRT

101325* 161.8*0.001 = n* 8.314*(7.6+273)

or n = 7.03 moles

5) no. of moles inside the tank will remain same after rising the temperature if there is no leakage as pressure will also increase in the same proportion.

n=19* 7.03= 133.57 moles

otherwise be specific whether 3,4 and 5 are subsequent processes!

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