As a system increases in volume, it absorbs 59.0 J of energy in the form of heat from the surroundings. The piston is working against a pressure of 0.543 atm. The final volume of the system is 57.7 L. What was the initial volume of the system if the internal energy of the system decreased by 107.6 J? Volume = L

The initial volume of the system is 2.7 L

Explanation:

The change in internal energy is given by;

ΔU = Q - W

where;

Q is the heat absorb from the surrounding

W is the work done by the system

Given;

ΔU  = -107.6 J

Q = 59 J

W = ?

W = Q- ΔU

W = 59J - (-107.6)

W = 166.6 J

Work done is given by;

W = PΔV

W = P(V₂ - V₁)

101.325 Joules = 1 L.atm

166.6 Joules  = ?

= 1.644 L.atm

1.644 L.atm = 0.543 atm(57.7L - V₁)

57.7L - V₁ = (1.644 L.atm) / (0.543 atm)

57.7L - V₁ = 3.0 L

V₁ = 57.7L - 3.0 L

V₁ = 2.7 L

Therefore, the initial volume of the system is 2.7 L

i was thinking more like reflects green light, just not sure

= initial pressure

= final pressure = 2

= initial volume

= final volume = /4

= initial temperature = 20 c = 20 + 273 = 293 k

= final temperature = ?

using the equation