Oxygen Tank: Question about gas laws

[electricblue7]

Homework Statement

A cylinder of compressed Oxygen is carried on a spacecraft headed for Mars. The compressed gas cylinder has a volume of 17000 L and is filled to a pressure of 248 atm at 231 K. The maximum pressure the cylinder can hold is 1000 atm.The contents of the cylinder are then entirely transferred to a partially filled holding tank of volume 10,000 L, originally at pressure 22 atm and 300 K. What is the new pressure in the holding tank at 300 K?

Homework Equations

PV = nRT

The Attempt at a Solution

Since we are given the initial pressure, I think we can can calculate the number of moles of gas in the tank before the transfer using PV = n RT.

I did: (248 atm)(17,000 L) = n (0.0821) (231 K)
n = 222,303.0725 moles

Then I used this number and plugged it into the ideal gas law equation once more to come up with the new pressure.

(P) (10,000 L) = (222,303.0725 moles)(0.0821) (300 K)

P = 547.5324675 atm

It says this is wrong, and I'm not sure why.

 

[LowlyPion]

Welcome to PF.

How many moles were initially in the Final 10K liter tank?

Don't you need to consider the total number of moles in the final tank?

 

[electricblue7]

I think so, but this is all the information the problem gives...

 

[rl.bhat]

You are transferring 17000 L of oxygen into partially filled cylinder containing 10000 L of gas. So first of all find the total mass of the gas in mole. The volume remains constant.