Explanation:
According to first law of thermodynamics, total energy of a system and its surroundings remain constant.
Equation for first law of thermodynamics is as follows.
[tex]\Delta U = q + w[/tex]
where, [tex]\Delta U[/tex] = change in energy
q = heat released or absorbed
w = work done
As it is given that heat absorbed is 139 J (as heat is absorbed so it will be positive) and work done is -344 J (as work is done on the system).
Hence, we will calculate the energy change as follows.
[tex]\Delta U = q + w[/tex]
= 139 J + (-344 J)
= 205 J
Thus, we can conclude that change in energy of the gas is 205 J.
The change in energy of the gas is -2.05 × 10^-2 J.
According to the first law of thermodynamics, energy is neither created nor destroyed. From this law, the total energy of the system is given by;
ΔU = Q + W
Where;
ΔU = change in energy of the system
Q = heat absorbed or lost
W = work done
Recall that work done is negative when work is done on the surrounding and Q is negative when heat is lost to the surroundings.
Given that;
Q = 139 J
W = -344 J
ΔU = 139 J - 344 J
ΔU = -2.05 × 10^-2 J
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