Acylinder and piston assembly (defined as the system) is warmed by an external flame. the contents of the cylinder expand, doing work on the surroundings by pushing the piston outward against the external pressure. if the system absorbs 533 j of heat and does 488 j of work during the expansion, what is the value of δe? express the energy change as an integer and include the appropriate units.

The energy change for the given system: ΔE  = 45 J

Explanation:

According to the First Law of thermodynamics, the energy can't be created or destroyed and can only be converted into other forms.

ΔE = Q - W                                 equation 1

Given: ΔE is the change in the internal energy

Q is the heat absorbed by the system

W is the work done by the system

Given: Q = = 533 J, W = 488 J, ΔE = ?

Using equation 1, to calculate the change is the internal energy (ΔE),

ΔE = Q - W = 533 J - 488 J = 45 J

Therefore, the energy change for the given system: ΔE  = 45 J

the reaction mixture contains some ammonia, plus a lot of unreacted nitrogen and hydrogen. the mixture is cooled and compressed, causing the ammonia gas to condense into a liquid. the liquefied ammonia is separated and removed. the unreacted nitrogen and hydrogen are then recycled back into the reactor .