This question can be answered using Boyle's Law. Notice that initially the oxygen gas and the helium gas have the same temperature, and when they are both pumped into a tank, they remain at the same temperature. So, the temperature remains constant throughout the process, and Boyle's Law can be...

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This question can be answered using Boyle's Law. Notice that initially the oxygen gas and the helium gas have the same temperature, and when they are both pumped into a tank, they remain at the same temperature. So, the temperature remains constant throughout the process, and Boyle's Law can be applied.

As oxygen is pumped into a tank with the given volume, according to the Boyle's Law, the product of the pressure and the volume remains constant:

From here, the final pressure of oxygen is

`P_f = (P_iV_i)/(V_f) =(1.3*27.4)/5.81 = 6.13 atm `

(I am assuming that the volume of the tank is also given in liters.)

The new partial pressure of oxygen is 6.13 atm.