Answer:
No, ΔE does not always equal zero because it refers to the systems internal energy, which is affected by heat and work
Explanation:
According to the first law of thermodynamics, energy is neither created nor destroyed. This implies that the total energy of a system is always a constant.
So, according to the first law of thermodynamics we have that ΔE = q + w. This means that the value of ΔE depends on q (heat) and w(work). Hence ΔE is not always zero since it depends on the respective values of q and w.
Answer:
-1,300 kJ
I don't want to explain it brainly AAAAA
N₂ + 3H₂ ⇆ 2NH₃
↓ volume = ↑ pressure
The reaction shifts toward the product gas.
:)
