A system does 3.7 × 104 J of work, and 8.5 × 104 J of heat flows into the system during the process. Find the change in the internal energy of the system.
Well, this sounds like quite the energetic situation! To find the change in the internal energy of the system, we can use the first law of thermodynamics: ΔU = Q - W.
Given that the work done on the system is 3.7 × 10^4 J and the heat flow into the system is 8.5 × 10^4 J, we can plug these values into the formula:
ΔU = (8.5 × 10^4 J) - (3.7 × 10^4 J)
Now, let's do the calculations. *cue circus music*
ΔU = 4.8 × 10^4 J
Ta-da! The change in internal energy of the system is 4.8 × 10^4 J. Keep that energy flowing, my friend!
The change in the internal energy of a system is given by the first law of thermodynamics, which states that:
ΔU = Q - W
where ΔU is the change in internal energy, Q is the heat added to the system, and W is the work done by the system.
In this case, Q = 8.5 × 10^4 J (heat flows into the system) and W = 3.7 × 10^4 J (work done by the system).
Therefore, the change in the internal energy of the system is:
ΔU = 8.5 × 10^4 J - 3.7 × 10^4 J
Calculating this expression:
ΔU = 4.8 × 10^4 J
So, the change in the internal energy of the system is 4.8 × 10^4 J.
To find the change in the internal energy of the system, we can use the first law of thermodynamics, which states that the change in the internal energy of a system is equal to the net heat added to the system minus the work done by the system.
Mathematically, this can be expressed as:
ΔU = Q - W
Where:
ΔU is the change in internal energy of the system,
Q is the heat added to the system, and
W is the work done by the system.
In this case, the given information is as follows:
Q = 8.5 × 10^4 J (heat added to the system)
W = 3.7 × 10^4 J (work done by the system)
Now, we can substitute these values into the equation to find the change in internal energy:
ΔU = 8.5 × 10^4 J - 3.7 × 10^4 J
Calculating this, we get:
ΔU = 4.8 × 10^4 J
Therefore, the change in internal energy of the system is 4.8 × 10^4 J.