Thermodynamic Process

Heat absorbed by a system in going through a cyclic process shown in figure is :

A closed container contains a homogeneous mixture of two moles of an ideal monatomic gas $\left(\gamma =\frac{5}{3}\right)$ and one mole of an ideal diatomic gas $\left(\gamma =\frac{7}{5}\right)$. Here, $\gamma$ is the ratio of the specific heats at constant pressure and constant volume of an ideal gas. The gas mixture does a work of $66$ Joule when heated at constant pressure. The change in its internal energy is _____ Joule.

A thermodynamic system is taken through cyclic process. The total work done in the process is :

A gas is compressed adiabatically, which one of the following statement is NOT true?

An ideal gas is compressed such that its pressure $P$ and volume $V$ are related as $PV{ }^2$= constant. During this process, the temperature of gas

In which of the following process, the internal energy of gas remains constant?

 The final volume (in $L$) of one mole of an ideal gas initially at $27°\mathrm{C}$ and $8.21$ $\mathrm{atm}$ pressure, if it absorbs $420 \mathrm{cal}$ of heat during a reversible isothermal expansion, is

The work done by gas is equal to heat supplied. An ideal gas has initial volume $V$ and pressure $P.$ To triple its volume the minimum work done, will be

 

 Following graph shows a single stage expansion process, then work done by the system is ?

  Select the correct option regarding adiabatic expansion of an ideal gas.

A monoatomic gas does $100 \mathrm{J}$ of work when it is expanded isobarically. How much of heat is given to the gas in the process

A gas is expanded from an initial state to a final state along a path on a $P-V$ diagram. The path consists of (i) an isothermal expansion of work $50 \mathrm{J}$, (ii) an adiabatic expansion and (iii) an isothermal expansion of work $20 \mathrm{J}$. If the internal energy of gas is changed by $-30 \mathrm{J}$, then the work done by gas during adiabatic expansion is

A process in which the amount of heat supplied to the system goes fully to change its internal energy and temperature is

Calculate the amount of work done when one mole of an ideal gas contained in a bulb of $2 \mathrm{L}$ capacity at $1\mathrm{atm}$ is allowed to enter in evacuated bulb of $10 \mathrm{L}$ capacity and in another case it is allowed to expand from $1 \mathrm{L}$ to $5 \mathrm{L}$ against a pressure of $1\mathrm{atm}$.

In the given $P-V$ diagram, a monoatomic gas $\left(\gamma =\frac{5}{3}\right)$ is first compressed adiabatically from state $A$ state $B$. Then it expands isothermally from state $B$ to state $C$. [Given : ${\left(\frac{1}{3}\right)}^{0.6}=0.5,\ln 2\approx 0.7$].

Which of the following statement(s) is(are) correct?

State $1 \rightleftarrows$ State $2 \rightleftarrows$ State 3

$\left(\begin{array}{c}T=300 \mathrm{K}\\ P=15 \mathrm{bar}\\ \text{1 mole }\end{array}\right) \left(\begin{array}{c}T=300 \mathrm{K}\\ P=10 \mathrm{bar}\\ \text{ 1 mole }\end{array}\right)\left(\begin{array}{c}T=300 \mathrm{K}\\ P=5 \mathrm{bar}\\ \text{1 mole }\end{array}\right)$

Above shows a cyclic process. Calculate the total work done during one complete cycle.

(Assume a single step to reach the next state).

Find the heat energy required to raise the temperature of $n$ moles of a gas from $T_0$ to $2T_0$ if its molar heat capacity varies as shown in the diagram. The equation of the curve is ${\mathrm{CT}}^x=$ constant

Which of the following statements is correct, in case of adiabatic expansion?

The relation between internal energy $U$, pressure $P$ and volume $V$ of a gas in an adiabatic process is $U=a+bPV$ where $a$ and $b$ are positive constants.

The value of ratio of molar specific heats $\left(\gamma \right)$ is 

A thermodynamic system containing one mole of an ideal gas was supplied with $3\mathrm{kJ}$ of heat. All the heat was utilized in increasing the internal energy of the system. No work is done in the process through volume change.
$\left[C_v=\frac{3R}{2}\right]$
Choose correct statements from the following: