Question #089c7

1 Answer
May 10, 2017

Change in internal energy, Delta U = -143.56J

Explanation:

Using the first law of thermodynamics
Delta U → Delta Q + Delta W
where Delta U is the change in internal energy of a system
Delta Q is the energy supplied to the system
Delta W is the work done on or by the system

Delta W = pDeltaV
Delta W= 101.325 Pa (5.6xx10^-3m^3- 1.21xx10^-3m^3)
Delta W= 0.44 J

Since work is being done by the gas Delta W is negative
i.e. Delta W= -0.44 J

Since energy is being released by the gas, DeltaQ is negative
i.e. Delta Q= -124 J

Change in internal energy, Delta U= -124 + (-0.44) = -143.56J
So internal energy is decreasing.

*** I converted the L to m^3 and the atm to Pa