A 3.75 mol sample of a diatomic ideal gas ( ? = 1.4) expands slowly and adiabati

Question

A 3.75 mol sample of a diatomic ideal gas (? = 1.4) expands slowly and adiabatically from a pressure of 4.25 atm and a volume of 13.0 L to a final volume of 33.0 L.

A 3.75 mol sample of a diatomic ideal gas (? = 1.4) expands slowly and adiabatically from a pressure of 4.25 atm and a volume of 13.0 L to a final volume of 33.0 L. What is the final pressure of the gas? What is the initial temperature of the gas? What is the final temperature of the gas? Find the value for Q. Find the value for ?U. Find the value for W (work done by the gas). Use ?U = Q - W and the answers from the last two parts.

Explanation / Answer

here are the formulas you need to solve this problem: ----> put of this you can get the final pressure (P1V1)^ ? =(P2V2) ^? where p- pressure V-volume ?- 1.4 adiabatic exponent ------> out of this you can get the initial temperature & final temperatures pV=?RT ?- number of mols T-temperature ------> Q is always 0 in an adiabatic process -------> L=?U= ?*2.5*R*(T2-T1) -------->Eint= ?U R- the constant of ideal gases

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