Isothermal Reversible Process

The video tutorial explores thermodynamic processes, focusing on isothermal processes. It explains the first law of thermodynamics, highlighting that in isothermal processes, the change in internal energy (delta U) is zero. The tutorial demonstrates how to calculate work and heat using the ideal gas law, emphasizing that work is the negative of heat. It also discusses enthalpy changes, showing that for isothermal processes, enthalpy change (delta H) is zero. The video concludes by noting that isothermal processes are simpler to handle compared to other processes like isobaric ones.

Which of the following processes involves no change in temperature?

• Isochoric

• Adiabatic

• Isobaric

• Isothermal

In an isothermal process, what is the value of delta U, the change in internal energy?

• It is zero

• It is equal to the work done

• It is equal to the heat added

• It is equal to the change in enthalpy

For an isothermal process involving an ideal gas, how is work calculated?

• By integrating pressure with respect to volume

• By integrating volume with respect to pressure

• By multiplying pressure and volume

• By using the change in temperature

What is the relationship between work and heat in an isothermal process?

• Work is equal to heat

• Work is half of the heat

• Work is the negative of heat

• Work is double the heat

In an isothermal process, what is the value of enthalpy change (delta H) for an ideal gas?

• It is zero

• It is equal to the heat added

• It is equal to the change in internal energy

• It is equal to the work done

Why are isothermal processes considered easier to analyze compared to isobaric processes?

• Because pressure remains constant

• Because they involve no work

• Because temperature remains constant

• Because volume remains constant

What is the first step in analyzing an isothermal process?

• Calculate the heat added

• Calculate the change in enthalpy

• Calculate the change in internal energy

• Calculate the work done