One hundred (100.) joules of work is required to compress a gas. At the same time, the gas releases 65 J of heat.
Internal energy change
The internal energy change can be determined using the First Law of Thermodynamics, which states that the change in internal energy of a system is equal to the heat added to the system minus the work done by the system.
In this case, the work done on the gas is 100 J and the heat released by the gas is 65 J. Therefore, we can calculate the internal energy change as follows:
Internal energy change = Heat added - Work done
Internal energy change = 65 J - 100 J
Internal energy change = -35 J
The negative sign indicates that the internal energy of the gas has decreased by 35 J.
To calculate the change in internal energy of the gas, we need to consider both the work done on the gas and the heat released by the gas.
The change in internal energy (ΔU) is given by the equation:
ΔU = Q - W
Here, Q represents the heat released by the gas, and W represents the work done on the gas.
Given:
Q = 65 J (heat released)
W = 100 J (work done)
Substituting these values into the equation, we get:
ΔU = 65 J - 100 J
Now, we can calculate the change in internal energy:
ΔU = -35 J
The negative sign indicates that the internal energy of the gas has decreased by 35 joules.
dE = dH + work
dH is 65
work is 100
Get th signs right on dH and work.
+ means "on the system"
- means "by the system"