Answer:
<h2>
ΔE = -1,382,800Joules</h2>
Explanation:
The internal energy of the system according to the thermodynamics law is the difference between the heat released by the system and work done to the system. Mathematically;
ΔE = q - W where;
ΔE is the change in internal energy of the syatem
q is the heat released by the system
W is the work done to the system
Given W = 4.50×10² kcal and q = 5.00×10² kJ
Since 1cal = 4.184Joules
4.50×10² kcal = (4.50×10²×10³)×4.184
W = 4.50×10² kcal = 1,882,800 Joules
q = 5.00×10² kJ = 5.00×10⁵Joules
q = 500,000Joules
Since ΔE = q - W
ΔE = 500,000 J - 1,882,800 J
ΔE = -1,382,800Joules
Hence, the change in the internal energy of the system is -1,382,800Joules