Calculating Final Volume of Ideal Gas with Isobaric and Adiabatic Expansion

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The discussion revolves around calculating the final volume of an ideal gas after it undergoes isobaric and adiabatic expansions. The initial conditions include 0.310 mol of gas at a volume of 7500 cm³ and a temperature of 29 degrees Celsius. The gas first expands isobarically, doubling its volume, followed by an adiabatic expansion that returns the temperature to its initial value. The user initially struggled with finding the temperature after the isobaric expansion but later confirmed they solved the problem. The key equations used include PV = nRT and the relationships governing temperature and volume changes during the expansions.
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Homework Statement



A balloon has 0.310 mol of polyatomics gas, Initial volume 7500cm³ and temp 29 degrees C, gas first expands isobarically until volume double. Then expands adiabatiacally until temp returns to initial value, assume gas is ideal gas, C_p = 33.26 J/mol*K, gamma = 4/3.

What is the final volume V?


Homework Equations



I think I have to use
PV = nRT
T_1V_1^(gamma-1) = T_2V_2^(gamma-1)

The Attempt at a Solution



I've tried to find the temperature after it expands isobarically and use that as the T1 value, I think this is the only trouble I'm facing here, after that I can find V_2 and add all volumes together, please guide me on how to find T after the isobaric expansion.
 
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satanic said:

Homework Statement



A balloon has 0.310 mol of polyatomics gas, Initial volume 7500cm³ and temp 29 degrees C, gas first expands isobarically until volume double. Then expands adiabatiacally until temp returns to initial value, assume gas is ideal gas, C_p = 33.26 J/mol*K, gamma = 4/3.

What is the final volume V?


Homework Equations



I think I have to use
PV = nRT
T_1V_1^(gamma-1) = T_2V_2^(gamma-1)

The Attempt at a Solution



I've tried to find the temperature after it expands isobarically and use that as the T1 value, I think this is the only trouble I'm facing here, after that I can find V_2 and add all volumes together, please guide me on how to find T after the isobaric expansion.
I will assume this is an ideal gas. So PV=nRT which means that T = PV/nR. If P is constant ΔT = ΔV(P/nR). Remember T is in Kelvins so the initial temperature 29C is what in Kelvin?

AM
 
I've actually solved it, thank you anyway
 

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