140cal of energy are added to a container of air from an outside source. The air also has 30cal of work done to it. By how how much did the internal energy of the air inside the container change?
The change in internal energy of the air inside the container can be calculated using the first law of thermodynamics, which states that the change in internal energy (ΔU) of a system is equal to the amount of heat added (Q) minus the work done (W) on the system.
In this case, the heat added to the air is 140 cal, and the work done on the air is 30 cal. Therefore, the change in internal energy of the air inside the container is:
ΔU = Q - W
= 140 cal - 30 cal
= 110 cal
So, the internal energy of the air inside the container changed by 110 calories.
To find the change in internal energy of the air inside the container, we need to consider both the energy added from an outside source and the work done on the air.
The change in internal energy (ΔU) can be calculated using the first law of thermodynamics:
ΔU = Q - W
Where:
ΔU is the change in internal energy
Q is the heat added to the system
W is the work done on the system
Given that 140 cal of energy are added (Q = 140 cal) and 30 cal of work is done (W = 30 cal), we can substitute these values into the equation:
ΔU = 140 cal - 30 cal
ΔU = 110 cal
Therefore, the internal energy of the air inside the container changed by 110 cal.