A tank of compressed O2 gas is 6.00 ft high and has a diameter of 8.00 in. The t

Question

A tank of compressed O2 gas is 6.00 ft high and has a diameter of 8.00 in. The tank is filled with O2 to a pressure of 175 atm at 25 C.

a)How many moles of O2 does the tank hold, and what volume would the gas occupy at 1.00 atm and 25 C? (assume that the ideal gas law holds)

b)If it were assumed that the van der Waals equation held at 175 atm instead of the ideal gas law, how many moles does the tank hold, and what volume would the gas occupy at 1.00 atm and 25 C?

I got the answer to part (a) n= 424.22 mol O2 and V= 1.04 x 10^4
But how would you solve for part b? can someone please help me how to get the answer??

Thank you.

Explanation / Answer

The first part of this problem is straight forward, the only tricky part is finding out the volume of the tank using the information given: The volume of a cylinder is V = pr^2h I like to convert to units I am familiar with, so 6 ft is 182.88 centimeters, 8 in is 20.32 cm V = pr^2h V= p(10.16)^2(182.88) V= 59306.67 cm^3 V= 59306.67 mL Use the ideal gas law to determine the value of n: P=175 atm T= 298.15 K R=82.05746 cm^3? atm ?K^-1?mol^-1 V= 59306.67 cm^3 PV=nRT n=PV/RT n= 424.2176 mol O2 Use that value of n to solve for the second part of the question: PV=nRT V=nRT/P V= 1.037866 x 10^7 mL V= 1.037866 x 10^4 L

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