Internal Energy

Internal energy and pressure of a gas per unit volume are related as:

According to law of equipartition of energy, the average energy associated with each degree of freedom is:

The process in which the value of $∆\mathrm{U} = 0$ is:

A thermally insulated rigid container of $1 \mathrm{L}$ volume contains a diatomic ideal gas at room temperature. A small paddle installed inside the container is rotated from the outside, such that the pressure rises by ${10}^5 \mathrm{Pa}$. The change in internal energy is close to

Which factors affect the internal energy ?

One mole of an ideal gas at $300 \mathrm{K}$ is expanded isothermally from an initial volume of $1$ $\mathrm{Litres}$ to $10$ $\mathrm{litres}$. The $∆\mathrm{U}$ for this process is ($\mathrm{R}=$$2$ $\mathrm{cal} {\mathrm{mol}}^{-1} {\mathrm{K}}^{-1}$)

In the reaction, ${\mathrm{H}}_2\left(\mathrm{g}\right)+{\mathrm{Cl}}_2\left(\mathrm{g}\right)⟶2\mathrm{HCl}\left(\mathrm{g}\right)$ $\mathrm{\Delta H}=-184\mathrm{kJ}$ if $2$ moles of ${\mathrm{H}}_2$ react with $2$ moles of ${\mathrm{Cl}}_2$, then $∆\mathrm{U}$ is equal to

A gas does $0.320 \mathrm{kJ}$ of work on its surroundings and absorbs $120 \mathrm{J}$ of heat from the surroundings. Hence, $∆\mathrm{U}$ is 

When a sample of an ideal gas is allowed to expand at constant temperature against an atmospheric pressure,

For the isothermal reversible expansion of an ideal gas

Out of boiling point (I), internal energy (II), Molar specific heat (III) and density (IV) intensive properties are:

One mole of an ideal gas at $300 \mathrm{K}$ is expanded isothermally from an initial volume of $1$ litre to $10$ litre. $∆\mathrm{U}$ for this process is: 

$\left(\mathrm{R}=2\mathrm{ }\mathrm{cal}\mathrm{ }{\mathrm{mol}}^{-1}\mathrm{ }{\mathrm{K}}^{-1}\right)$

The internal energy change when a system goes from state A to B is 40 kJ/mole. If the system goes from A to B by a reversible path and returns to state A by an irreversible path what would be the net change in internal energy?

Which of the following is correct for an ideal gas?

One mole of a non-ideal gas undergoes a change of state (2.0 atm, 3, 0 L,95(K) $\to$ (4.0 atm, 5.0 L, 245 K) with a change in internal energy, $∆\mathrm{U}=30.0\mathrm{ }\mathrm{L}$ atm is

Assertion: The internal energy of an isothermal process does not change.

Reason: The internal energy of a system depends only on pressure of the system

The internal energy when a system goes from state A to B is 40 kJ/mol. If the system goes from A to B by a reversible path and returns to state A by an irreversible path. What would be the net change in internal energy?

A stationary mass of gas is compressed without friction from an initial state of $0.3\mathrm{ }{\mathrm{m}}^3$ and $0.105\mathrm{ }\mathrm{M}\mathrm{ }\mathrm{P}\mathrm{a}$ to a final state of $0.15\mathrm{ }{\mathrm{m}}^3$ and $0.105\mathrm{ }\mathrm{M}\mathrm{ }\mathrm{P}\mathrm{a}$. The pressure remaining constant. During the process there is transfer of $37.6\mathrm{ }\mathrm{k}\mathrm{J}$ of heat from the system. During the process the amount of internal energy change is-

Select the correct statement -

The total internal energy change for a reversible isothermal cycles is