(D) Statement-$I$ is incorrect because internal energy $(U)$ is a state function,but work $(w)$ is a path function,not a state function.Statement-$II$

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Statement-$I$ is not correct,but statement-$II$ is correct

(D) Statement-$I$ is incorrect because internal energy $(U)$ is a state function,but work $(w)$ is a path function,not a state function.Statement-$II$ is correct because during free expansion into a vacuum,the external pressure $(P_{ext})$ is $0$. Since $w = -P_{ext} \Delta V$,the work done $(w)$ is $0$.

Class 11 Chemistry Thermodynamics Mix Examples-Thermodynamics and Thermochemistry

Medium

Consider the following statements:
Statement-$I$: Both internal energy $(U)$ and work $(w)$ are state functions.
Statement-$II$: During the free expansion of an ideal gas into vacuum,the work done is zero.
The correct answer is:

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A
Both statement-$I$ and statement-$II$ are correct
B
Both statement-$I$ and statement-$II$ are not correct
C
Statement-$I$ is correct,but statement-$II$ is not correct
D
Statement-$I$ is not correct,but statement-$II$ is correct

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Mix Examples-Thermodynamics and Thermochemistry

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Match the conditions and the temperature for the 'fusion' process of $H_2O_{(s)}$ at $1 \ atm$ pressure.

Condition Temperature

$(1)$. Spontaneous $(p)$. $273 \ K$

$(2)$. At equilibrium $(q)$. $260 \ K$

$(3)$. Non-spontaneous $(r)$. $280 \ K$

Condition	Temperature
$(1)$. Spontaneous	$(p)$. $273 \ K$
$(2)$. At equilibrium	$(q)$. $260 \ K$
$(3)$. Non-spontaneous	$(r)$. $280 \ K$

Medium

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Two moles of an ideal monoatomic gas are allowed to expand adiabatically and reversibly from $300 \ K$ to $200 \ K$. The work done in the process will be $..... \ kJ$.

Medium

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Standard entropies of $X_2$,$Y_2$ and $XY_3$ are $60$,$40$ and $50 \ J \ K^{-1} \ mol^{-1}$ respectively. For the reaction $\frac{1}{2} X_2 + \frac{3}{2} Y_2 \rightarrow XY_3$,the enthalpy change is $\Delta H = -30 \ kJ \ mol^{-1}$. At what temperature will the reaction be at equilibrium (in $K$)?

MediumAP EAMCET 2021

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For the reaction $2H_{(g)} \to H_{2(g)}$,the signs of $\Delta H$ and $\Delta S$ are:

Easy

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Enthalpy of fusion and enthalpy of vaporization for water respectively are $6.01 \ kJ \ mol^{-1}$ and $45.07 \ kJ \ mol^{-1}$ at $0^{\circ}C$. What is enthalpy of sublimation at $0^{\circ}C$?

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Consider the following statements:Statement-$I$: Both internal energy $(U)$ and work $(w)$ are state functions.Statement-$II$: During the free expansion of an ideal gas into vacuum,the work done is zero.The correct answer is:

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Match the conditions and the temperature for the 'fusion' process of $H_2O_{(s)}$ at $1 \ atm$ pressure. Condition Temperature $(1)$. Spontaneous $(p)$. $273 \ K$ $(2)$. At equilibrium $(q)$. $260 \ K$ $(3)$. Non-spontaneous $(r)$. $280 \ K$

Two moles of an ideal monoatomic gas are allowed to expand adiabatically and reversibly from $300 \ K$ to $200 \ K$. The work done in the process will be $..... \ kJ$.

Standard entropies of $X_2$,$Y_2$ and $XY_3$ are $60$,$40$ and $50 \ J \ K^{-1} \ mol^{-1}$ respectively. For the reaction $\frac{1}{2} X_2 + \frac{3}{2} Y_2 \rightarrow XY_3$,the enthalpy change is $\Delta H = -30 \ kJ \ mol^{-1}$. At what temperature will the reaction be at equilibrium (in $K$)?

For the reaction $2H_{(g)} \to H_{2(g)}$,the signs of $\Delta H$ and $\Delta S$ are:

Enthalpy of fusion and enthalpy of vaporization for water respectively are $6.01 \ kJ \ mol^{-1}$ and $45.07 \ kJ \ mol^{-1}$ at $0^{\circ}C$. What is enthalpy of sublimation at $0^{\circ}C$?

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Consider the following statements:
Statement-$I$: Both internal energy $(U)$ and work $(w)$ are state functions.
Statement-$II$: During the free expansion of an ideal gas into vacuum,the work done is zero.
The correct answer is:

Match the conditions and the temperature for the 'fusion' process of $H_2O_{(s)}$ at $1 \ atm$ pressure.

Condition Temperature

$(1)$. Spontaneous $(p)$. $273 \ K$

$(2)$. At equilibrium $(q)$. $260 \ K$

$(3)$. Non-spontaneous $(r)$. $280 \ K$