Five moles of monatomic ideal gas have initial pressure 2.50 * 103 pa and initial volume 2.10 m3. while undergoing an adiabatic expansion, the gas does 1480 j of work. what is the final pressure of the gas after the expansion?

pressure of the gas after the expansion is 1795.238 Pa

Explanation:

adiabatic expansion W(+) -  ideal gas:

deriving (1):

⇒ PdV + VdP = RndT

⇒ PdV = RndT - VdP

being the T constant ⇒ dT = 0

⇒ PdV = - VdP(3)

(3) in (1):

⇒ W = ∫ (- VdP )

⇒ W = - V ∫dP

⇒ W = - V * ( P2 - P1 )

⇒ P2 = - ( W / V ) + P1

⇒ P2 = - ( 1480 J / 2,1 m³ ) + 2.5 E3 J /m³

⇒ P2 =  - 704.762 J/m³ + 2.5 E3 J/m³

⇒ P2 = 1795.238 Pa

answer: the primary difference between a hypothesis and a theory is that b hypothesis is falsifiable, but a theory has been proven to be correct. theory is an explanation of something that is happening but hypothesis is a guess of something that can happen

explanation:

the increase of protons   hope this