What is an isothermal process, adiabatic process, and isobaric process? Write the first law of thermodynamics for an ideal gas.
(N/A) $1$. Isothermal Process: $A$ process in which the temperature of the system remains constant $(T = \text{constant})$. For an ideal gas, the internal energy remains constant $(dU = 0)$.
$2$. Adiabatic Process: $A$ process in which there is no exchange of heat between the system and its surroundings $(dQ = 0)$.
$3$. Isobaric Process: $A$ process in which the pressure of the system remains constant $(P = \text{constant})$.
$4$. First Law of Thermodynamics: For an ideal gas, the first law is given by $dQ = dU + dW$, where $dQ$ is the heat supplied to the system, $dU$ is the change in internal energy, and $dW$ is the work done by the system.
$2$. Adiabatic Process: $A$ process in which there is no exchange of heat between the system and its surroundings $(dQ = 0)$.
$3$. Isobaric Process: $A$ process in which the pressure of the system remains constant $(P = \text{constant})$.
$4$. First Law of Thermodynamics: For an ideal gas, the first law is given by $dQ = dU + dW$, where $dQ$ is the heat supplied to the system, $dU$ is the change in internal energy, and $dW$ is the work done by the system.
Explore More
Similar Questions
$A$ gas expands such that its initial and final temperatures are equal. Also,the process followed by the gas traces a straight line on the $P-V$ diagram:
An ideal monoatomic gas is carried around the cycle $ABCDA$ as shown in the figure. The efficiency of the gas cycle is
Consider the thermodynamic cycle shown on the $PV$ diagram. The process $A \rightarrow B$ is isobaric,$B \rightarrow C$ is isochoric,and $C \rightarrow A$ is a straight-line process. The following internal energy change and heat are given: $\Delta U_{A \rightarrow B} = + 400 \text{ kJ}$ and $Q_{B \rightarrow C} = - 500 \text{ kJ}$. The heat flow in the process $Q_{C \rightarrow A}$ is ...... $\text{kJ}$.
Difficult
View SolutionThe internal energy of an ideal diatomic gas corresponding to volume $V$ and pressure $P$ is $2.5 PV$. The gas expands from $1 \text{ litre}$ to $2 \text{ litre}$ at a constant pressure of $10^5 \text{ N/m}^2$. The heat supplied to the gas is: (in $\text{ J}$)
One mole of an ideal monoatomic gas undergoes the following four reversible processes:
Step $1$: It is first compressed adiabatically from volume $8.0 \, m^{3}$ to $1.0 \, m^{3}$.
Step $2$: Then expanded isothermally at temperature $T_{1}$ to volume $10.0 \, m^{3}$.
Step $3$: Then expanded adiabatically to volume $80.0 \, m^{3}$.
Step $4$: Then compressed isothermally at temperature $T_{2}$ to volume $8.0 \, m^{3}$.
Then,$T_{1} / T_{2}$ is:
Step $1$: It is first compressed adiabatically from volume $8.0 \, m^{3}$ to $1.0 \, m^{3}$.
Step $2$: Then expanded isothermally at temperature $T_{1}$ to volume $10.0 \, m^{3}$.
Step $3$: Then expanded adiabatically to volume $80.0 \, m^{3}$.
Step $4$: Then compressed isothermally at temperature $T_{2}$ to volume $8.0 \, m^{3}$.
Then,$T_{1} / T_{2}$ is:
DifficultKVPY 2017
View SolutionVedclass Products
For Students
Vedclass Test Series
Mock tests in real JEE/NEET style with performance analysis. 5-day free trial.
Start Free TrialFor Teachers
Exam Paper Generator
Generate Set A/B/C/D exam papers from 7.5L+ questions in 2 minutes. 3 chapters free.
Try FreeFor Institutes
Online Exam Module
Live online exams with unlimited students, 360° analytics & white-label branding.
See Demo