Suppose you do 100j of work in compressing a gas, if 80j of heat escapes in the process, what is the change in internal energy of the gas?
To determine the change in internal energy of the gas, we need to use 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.
Given:
Work done (W) = 100 joules
Heat escaped (Q) = 80 joules
By applying the First Law of Thermodynamics, we can find the change in internal energy (ΔU) using the formula:
ΔU = Q - W
Plugging in the values:
ΔU = 80 J - 100 J
Simplifying the equation, we find:
ΔU = -20 J
Therefore, the change in internal energy of the gas is -20 joules.
To determine the change in internal energy of the gas, we need to use the equation:
ΔU = Q - W
Where:
ΔU represents the change in internal energy
Q represents the heat transferred to or from the gas
W represents the work done on or by the gas
In this case, we are given that 100j of work (W) is done on the gas and 80j of heat (Q) escapes. We can substitute these values into the equation and calculate the change in internal energy (ΔU):
ΔU = Q - W
ΔU = 80j - 100j
ΔU = -20j
The change in internal energy (ΔU) of the gas is -20j. The negative sign indicates that the internal energy of the gas has decreased.
100 - 80= 20 J.
Any work done on the gas that does not escape as heat becomes internal energy.
Qin = Wout + delta U
In this case both Wout and Qin are negative