For the adiabetic expansion of an ideal gas a) does the gas do work? B) doesd the internal energy of the gas increase, decrease or remain constant? C) what happens to the temperature?
Please check my answers
A) yes the gas does work because it is expanding
B) internal energy is zero because q=0
C) the temperature remains constant because q=0
A is right.
C is right.
I don't agree with B.
If dE = q + w and q is zero as you answered in C and work is done as you answered in A, how can dE be zero as you answered in B.
A) Your answer is correct. In an adiabatic expansion, the gas is doing work because it is expanding against an external pressure. The gas is able to transfer energy to its surroundings in the form of work.
B) However, your answer is not accurate. The internal energy of the gas does not necessarily have to be zero. In an adiabatic process, there may or may not be a change in internal energy, depending on several factors. To determine if the internal energy increases, decreases, or remains constant, we need to consider the specific conditions of the process, such as the initial and final volumes and pressures.
C) Your answer is partly correct. In an adiabatic process, there is no heat transfer occurring between the gas and its surroundings (q=0). As a result, the change in temperature of the gas is related to the change in internal energy. If the internal energy increases, the temperature of the gas will also increase. On the other hand, if the internal energy decreases, the temperature will decrease. Therefore, the temperature can either increase or decrease during the adiabatic expansion, depending on the specific conditions of the process.
To determine the change in internal energy, work, and temperature during an adiabatic expansion, you would need to know the specific values of the initial and final volumes, pressures, and the heat capacity ratio of the gas (ratio of specific heat capacities). These values can be used in the adiabatic expansion equations to calculate the changes.