(D) The internal energy of an ideal gas is given by $U = \frac{f}{2} nRT$,where $f$ is the degrees of freedom. For a monoatomic gas,$f=3$,so $U \propt

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(D) The internal energy of an ideal gas is given by $U = \frac{f}{2} nRT$,where $f$ is the degrees of freedom. For a monoatomic gas,$f=3$,so $U \propto T$.From the graph:State $A$: $T_A = T$State $B$: $T_B = 2T$State $C$: $T_C = 2T$State $D$: $T_D = T$Comparing internal energies:$U_A = U_D$ (since $T_A = T_D$),so $U_A - U_D = 0$. (True)$U_B = U_C$ (since $T_B = T_C$),so $U_B - U_C = 0$. (True)$U_C > U_D$ (since $T_C > T_D$),so $U_C - U_D > 0$. (True)$U_B > U_A$ (since $T_B > T_A$),so $U_B - U_A > 0$. Therefore,$U_B - U_A < 0$ is false.

Class 11 Physics Thermodynamics Heat, Work done and Internal Energy from Graph

Medium

An ideal monoatomic gas is taken through the thermodynamic states $A \to B \to C \to D$ via the paths shown in the figure. If $U_A, U_B, U_C$ and $U_D$ represent the internal energy of the gas in states $A, B, C$ and $D$ respectively,then which of the following is not true?

A
$U_A - U_D = 0$
B
$U_B - U_C = 0$
C
$U_C - U_D > 0$
D
$U_B - U_A < 0$

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Class 11

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Thermodynamics

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Heat, Work done and Internal Energy from Graph

An enclosed ideal gas is taken through a cycle as shown in the figure. Then

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$A$ thermodynamic system is taken from an original state to an intermediate state by the linear process shown in the figure. Its volume is then reduced to the original value from $E$ to $F$ by an isobaric process. Calculate the total work done (in $J$) by the gas from $D$ to $E$ to $F$.

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The $P-V$ diagram of $2\,g$ of helium gas for a certain process $A \to B$ is shown in the figure. What is the heat given to the gas during the process $A \to B$ (in $,P_0V_0$)?

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An ideal gas has undergone a cyclic process as shown in the figure. The work done by the gas in the entire cycle is . . . . . . $\times 10^{-1} \ J$. (Take $\pi = 3.14$)

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An ideal gas is made to undergo the cyclic process shown in the figure below. Let $\Delta W$ depict the work done,$\Delta U$ be the change in internal energy of the gas,and $Q$ be the heat added to the gas. The signs of each of these three quantities for the whole cycle will be ($0$ refers to no change):

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An ideal monoatomic gas is taken through the thermodynamic states $A \to B \to C \to D$ via the paths shown in the figure. If $U_A, U_B, U_C$ and $U_D$ represent the internal energy of the gas in states $A, B, C$ and $D$ respectively,then which of the following is not true?

Similar Questions

An enclosed ideal gas is taken through a cycle as shown in the figure. Then

$A$ thermodynamic system is taken from an original state to an intermediate state by the linear process shown in the figure. Its volume is then reduced to the original value from $E$ to $F$ by an isobaric process. Calculate the total work done (in $J$) by the gas from $D$ to $E$ to $F$.

The $P-V$ diagram of $2\,g$ of helium gas for a certain process $A \to B$ is shown in the figure. What is the heat given to the gas during the process $A \to B$ (in $,P_0V_0$)?

An ideal gas has undergone a cyclic process as shown in the figure. The work done by the gas in the entire cycle is . . . . . . $\times 10^{-1} \ J$. (Take $\pi = 3.14$)

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