In an adiabatic process, the temperature of an ideal gas decreases. What happens

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Question: In an adiabatic process, the temperature of an ideal gas decreases. What happens to its pressure?

Options:

Correct Answer: Decreases

Solution:

In an adiabatic process, as the temperature decreases, the pressure also decreases due to the ideal gas law.

In an adiabatic process, the temperature of an ideal gas decreases. What happens to its pressure?

In an adiabatic process, the temperature of an ideal gas decreases. What happens to its pressure?

Step 1: Understand what an adiabatic process is. It is a process where no heat is exchanged with the surroundings.
Step 2: Know that in an adiabatic process, if the temperature of an ideal gas decreases, it means the gas is losing energy.
Step 3: Recall the ideal gas law, which states that pressure (P), volume (V), and temperature (T) are related: PV = nRT, where n is the number of moles and R is the gas constant.
Step 4: If the temperature (T) decreases and the volume (V) remains constant, the pressure (P) must also decrease to keep the equation balanced.
Step 5: Therefore, in an adiabatic process, when the temperature of an ideal gas decreases, the pressure also decreases.

Adiabatic Process – An adiabatic process is one in which no heat is exchanged with the surroundings, leading to changes in temperature and pressure based on the work done on or by the gas.
Ideal Gas Law – The ideal gas law (PV=nRT) relates pressure (P), volume (V), temperature (T), and the number of moles (n) of an ideal gas.
Relationship Between Temperature and Pressure – In an adiabatic process for an ideal gas, a decrease in temperature typically leads to a decrease in pressure if the volume remains constant.