The work done when a gas is compressed in a cylinder like that shown in Figure
6.5 is 351 J. During this process, there is a heat transfer of 269 J from the gas to
the surroundings. Calculate the energy change for this process.
Not sure how to do this please explain with correct answers.
To calculate the energy change for this process, we need to consider the energy transferred as work and heat.
Given:
Work done, W = 351 J
Heat transferred, Q = -269 J (negative sign indicates heat transfer from gas to surroundings)
The energy change, ΔE, can be calculated using the First Law of Thermodynamics:
ΔE = Q + W
Substituting the given values, we get:
ΔE = -269 J + 351 J
ΔE = 82 J
Therefore, the energy change for this process is 82 J.
To calculate the energy change for the process, we need to determine the change in the internal energy of the gas. The internal energy change can be calculated using the first law of thermodynamics, which states that the change in the internal energy of a system is equal to the heat added to the system minus the work done by the system:
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, the heat transfer (Q) is given as -269 J, indicating that heat is transferred from the gas to the surroundings. The negative sign indicates heat loss. The work done (W) is given as 351 J, which indicates work done on the gas. Since work is being done on the gas, it is considered positive.
Plugging in the given values into the equation:
ΔU = -269 J - 351 J
= -620 J
Therefore, the energy change for this process is -620 J.