Check all the correct statements.

Note: Push yourself to understand why these statements are true or false. If false think about an example that contradicts the stalement, or think about how you would formulate the statement so it is correct. You will not see these exact questions in an exam, so it is important that you understand the concepts so you can answer a similar question that is formulated differently.

$U=q_v=n{C}_{v}T$ is always valid for any type of ideal gas. This expression even works, if the volume is not constant during the process.

The heat capacity of an ideal gas does not depend on whal molecules the gas is made of$.$

$U=0$ for any process that does not result in a change in temperature.

At constant temperature, the internal energy of a real gas changes with increasing pressure because molecules are brought closer together.

The internal energy of an ideal gas $($those that obey PV $=nRT)$ depends only on the temperature of the system.

A cyclic path $($initial stale $=$ final state $)$ always results in $U=0$

The intemal energy of any gas depends only on the temperature of the system.