Class 11

Physics

Heat & Thermodynamics

Thermodynamics

5 mole of an ideal gas expand isothermally and irreversibly from a pressure of 10 atm to 1 atm against a constant external pressure of 1 atm. $w_{irr}$ at 300 K is :

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On compressing a gas suddenly, its temperature

Curve in the figure shows an adiabatic compression of an ideal gas from $15m_{3}$ to $12m_{3},$ followed by an isothermal compression to a final volume of $3.0m_{3}.$ There are $2.0$ moles of the gas. Total heat supplied to the gas is equal to: $(ln2=0.693)$

The heat capacity at constant volume of a sample of a monoatomic gas is $31.867J/K$. Find the internal energy at $300_{∘}C$.

Refer to figure. Let $ΔU_{1}$ and $ΔU_{2}$ be the changes in internal energy of the system in the processes A andB. Then

In thermodynamic process, $200$ joules of heat is given to a gas and $100$ joules of work is also done on it . The chnage in internal energy of the gas is

The first law of thermodynamics can be written as $ΔU=ΔQ+ΔW$ for and ideal gas. Which of the following statements is correct?

Two moles of helium gas undergo a cyclic process as shown in figure. Assuming the gs to be ideal, calculate the following quantities in this process. The net change in internal energy.

Two cylinders A and B of equal capacity are connected to each other via a stopcock. A contains a gas at standard temperature and pressure. B is completely evacuated. The entire system is thermally insulated. The stopcock is now opened. Answer the following :(a) What is the final pressure of the gas in A and B ?(b) What is the change in internal energy of the gas?(c) What is the change in the temperature of the gas?(d) Do the intermediate states of the system (before settling to the final equilibrium state) lie on its P-V-T surface ?