Physics

A sample of helium behaves as an ideal gas as it is heated at constant pressure from 273 K to 373 K. If 15.0 J of work is done by the gas during this process, what is the mass of helium present?

I am not sure what equations to use for this problem....

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  1. PV=nRT
    p dV + V dp = n R dT
    p is constant here so
    p dV = n R dT
    work = integral p dV = nR dT
    p(V2-V1) = n R (T2-T1)

    so 15 = n R (T2-T1)

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  2. doesnt that give me an answer in moles? ...is there a way to convert moles to mg?

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  3. so i got the answer to be .01804 moles

    and i know one mole of helium is 4.03 g

    do i just multiply the two together? and then divide by 10000 to convert g to mg?

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  4. never mind. I made a silly error.

    i got .01804 moles...multiplied that times 4.03grams and then multiplied that times 1000 and got 72.7mg.

    got it! thanks so much!

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  5. what are we solving for in this equation?? 15 = n R (T2-T1)
    we know n, we know R, we know t1 and t2...so what do we solve for?

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