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One mole of an ideal monatomic gas, initially at 1 atm pressure, is surrounded by adiabatic walls in a container of volume 0.01 m3 . The gas is compressed until the volume is 1/8 of the original volume. Calculate the final pressure and temperature.
^^ I'm having problems following this question. Its only a short answer, but I'm confused none the less!
A: pV^5/3 = constant.
pf = pi(Vi/Vf )^5/3 = 1(8)^5/3 = 25 = 32 atm.
Tf = pfVf /nR = 32 × (0.01/8)101325/8.314 = 487.5 K
I understand the last line in normal ideal gas equation, but the first two lines, which reference the equation: pV^5/3 = constant has thrown me, i don't know how the second line follows (where does pf=pi*(vi/vf)^5/3 come from? i see its similar to the constant equation
^^ I'm having problems following this question. Its only a short answer, but I'm confused none the less!
A: pV^5/3 = constant.
pf = pi(Vi/Vf )^5/3 = 1(8)^5/3 = 25 = 32 atm.
Tf = pfVf /nR = 32 × (0.01/8)101325/8.314 = 487.5 K
I understand the last line in normal ideal gas equation, but the first two lines, which reference the equation: pV^5/3 = constant has thrown me, i don't know how the second line follows (where does pf=pi*(vi/vf)^5/3 come from? i see its similar to the constant equation