Adiabatic free expansion of an ideal gas must | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(C) According to the first law of thermodynamics, $Q = \Delta U + W$. In an adiabatic process, $Q = 0$. In free expansion, the external pressure $P_{e

Vedclass · Accepted Answer

Isothermal

Vedclass · Answer

(C) According to the first law of thermodynamics, $Q = \Delta U + W$. In an adiabatic process, $Q = 0$. In free expansion, the external pressure $P_{ext} = 0$, so the work done $W = P_{ext} \Delta V = 0$. Substituting these values into the first law: $0 = \Delta U + 0$, which implies $\Delta U = 0$. For an ideal gas, internal energy $U$ is a function of temperature only $(U = f(T))$. Since $\Delta U = 0$, the change in temperature $\Delta T = 0$, meaning the temperature remains constant. Therefore, the process is isothermal.

Adiabatic free expansion of an ideal gas must be

Similar Questions

Exothermic reactions occur in which of the following processes?

An ideal gas expands isothermally from $10^{-3} \; m^{3}$ to $10^{-2} \; m^{3}$ at $300 \; K$ against a constant external pressure of $10^{5} \; Nm^{-2}$. The work done on the gas is:

If $\Delta H$ is the change in enthalpy,$\Delta U$ is the change in internal energy,$N_P$ is the number of moles of products,and $N_r$ is the number of moles of reactants,then which of the following is correct for a gaseous reaction?

For which of the following reactions is $\Delta E = \Delta H$?

Identify the intensive quantity from the following.

Vedclass Test Series

Exam Paper Generator

Online Exam Module