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

2fe + 3h2so4 -> fe2(so4)3 + 3h2

it is necessary to balance equations in order to get the proper amount of reactants as well as products in order not to make a miscalculation.

you cannot change the subscripts as that would change the substance itself. for instance, diatomic elements such as h2 only have the subscript two when a gas. another example would be so4, if you were to change the subscript, the element would no longer be sulfate.

we change the coefficients instead as that only changes the number of molecules rather than the substance itself.

hope this !

the potential energy of the reactants is 200j.

from the energy diagram, the energy of the product formed is 350j; this means that, this reaction is an endothermic reaction, because it absorbs energy from its environment.