Question:
Which of the following is incorrect regarding the first law of thermodynamics?
It is a restatement of the principle of conservation of energy
It is not applicable to any cyclic process
It does not introduces the concept of the entropy
It introduces the concept of the internal energy
Question of from chapter.
JEE Main Previous Year 2005
Correct Option: 3
Solution:
Related Questions
A gas can be taken from $A$ to $B$ via two different processes ACB and ADB.
When path $A C B$ is used $60 \mathrm{~J}$ of heat flows into the system and $30 \mathrm{~J}$ of work is done by the system. If path ADB is used work done by the system is $10 \mathrm{~J}$. The heat Flow into the system in path ADB is :
$200 \mathrm{~g}$ water is heated from $40^{\circ} \mathrm{C}$ to $60^{\circ} \mathrm{C}$. Ignoring the slight expansion of water, the change in its internal energy is close to (Given specific heat of water $=4184 \mathrm{~J} / \mathrm{kgK}$ ):
A gas is compressed from a volume of $2 \mathrm{~m}^{3}$ to a volume of $1 \mathrm{~m}^{3}$ at a constant pressure of $100 \mathrm{~N} / \mathrm{m}^{2}$. Then it is heated at constant volume by supplying $150 \mathrm{~J}$ of energy. As a result, the internal energy of the gas:
An insulated container of gas has two chambers separated by an insulating partition. One of the chambers has volume $V_{1}$ and contains ideal gas at pressure $P_{1}$ and temperature $T_{1}$. The other chamber has volume $V_{2}$ and contains ideal gas at pressure $P_{2}$ and temperature $T_{2}$. If the partition is removed without doing any work on the gas, the final equilibrium temperature of the gas in the container will be
When a system is taken from state i to state $f$ along the path iaf, it is found that $Q=50$ cal and $W=20$ cal. Along the path ibf $Q=36$ cal. $W$ along the path ibf is
A system goes from $A$ to $B$ via two processes I and II as shown in figure. If $\Delta U_{1}$ and $\Delta U_{2}$ are the changes in internal energies in the processes I and II respectively, then
Three different processes that can occur in an ideal monoatomic gas are shown in the P vs V diagram. The paths are lebelled as $A \rightarrow B, A \rightarrow C$ and $A \rightarrow D$. The changein internal energies during these process are taken as $E_{A B}$, $\mathrm{E}_{\mathrm{AC}}$ and $\mathrm{E}_{\mathrm{AD}}$ and the workdone as $\mathrm{W}_{\mathrm{AB}}, \mathrm{W}_{\mathrm{AC}}$ and $\mathrm{W}_{\mathrm{AD}}$. The correct relation between these parameters are :
In an adiabatic process, the density of a diatomic gas becomes 32 times its initial value. The final pressure of the gas is found to be $n$ times the initial pressure. The value of $n$ is:
Match the thermodynamic processes taking place in a system with the correct conditions. In the table : $\Delta Q$ is the heat supplied, $\Delta W$ is the work done and $\Delta U$ is change in internal energy of the system.
A balloon filled with helium $\left(32^{\circ} \mathrm{C}\right.$ and $\left.1.7 \mathrm{~atm} .\right)$ bursts. Immediately afterwards the expansion of helium can be considered as :
