Question

A cylinder 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.

Answer 1

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

Step-by-step 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