Finding the amount of heat required to double volume?

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To determine the heat required to double the volume of 1.35 mol of oxygen gas starting at 11.0°C, the relationship between heat (Q), molar specific heat (Cp), and temperature change (ΔT) is established using the equation Q=nCpΔT. The specific heat for constant pressure is given as Cp=7R/2, leading to the equation Q=1.35(7R/2)(Tf-11), where Tf is the final temperature. The challenge lies in linking the change in volume to heat, which requires using the ideal gas law and understanding pressure (P) in the context of the problem. The discussion suggests that conservation of mass and simultaneous equations may be necessary to find the solution. Overall, the key focus is on applying thermodynamic principles to solve for the heat needed to achieve the desired volume change.
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Homework Statement



In an experiment, 1.35 mol of oxygen (02) are heated at constant pressure starting at 11.0°C. How much heat must be added to the gas to double its volume? You may assume without proof, that the molar specific heats are cp=7R/2 and cv=5R/2.



Homework Equations





The Attempt at a Solution



My working so far...

Q=nCpΔT

Q=n(7R/2)ΔT

Q= 1.35(7R/2)(s-11) -----> where s= Tf

But I need some equation linking change in volume to this...

ie Q= -PΔV

But I don't Know what P is?

Perhaps I need something with ΔEint but I am not to sure.
I was thinking I will need to solve the first equation simultaneously with one with ΔV

I'm stuck as to where to go from here??

Please help any advice is greatly noted.
 
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Hint: Use the ideal gas law followed by a conservation of mass.
 

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