(B) is the incorrect statement because the specific heat capacity of a liquid is generally higher than that of its gaseous state.$A$,$C$,and $D$ are c

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The specific heat capacity of a substance is greater in the gaseous state than in the liquid state

(B) is the incorrect statement because the specific heat capacity of a liquid is generally higher than that of its gaseous state.$A$,$C$,and $D$ are correct statements.

Class 11 Chemistry Thermodynamics Mix Examples-Thermodynamics and Thermochemistry

Medium

Which of the following statements is incorrect?

A
The specific heat capacity of a substance is greater in the solid state than in the liquid state
B
The specific heat capacity of a substance is greater in the gaseous state than in the liquid state
C
The latent heat of vaporization of a substance is greater than that of fusion
D
The internal energy of an ideal gas is a function of its temperature

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Class 11 Questions

Class 11

Chemistry Questions

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Thermodynamics

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Mix Examples-Thermodynamics and Thermochemistry

Which among the following are true for an irreversible isothermal expansion of an ideal gas?
$(i)$ $W = -Q$
$(ii)$ $\Delta U = 0$
$(iii)$ $\Delta H \neq 0$
$(iv)$ $\Delta T = 0$

EasyAP EAMCET 2021

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$\Delta H_f^o$ of water is $-285.5\, kJ\, mol^{-1}$. If enthalpy of neutralisation of monoacidic strong base is $-57.3\, kJ\, mol^{-1}$,$\Delta H_f^o$ of $OH^{-}$ ion will be $.....\, kJ\, mol^{-1}$.

Medium

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The heat of combustion of naphthalene $(C_{10}H_8(s))$ at constant volume is $-5133 \, kJ \, mol^{-1}$. The value of enthalpy change is .... $J$ $(R = 8.314 \, J \, K^{-1} \, mol^{-1}, T = 298 \, K)$.

Difficult

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Which of the following relations are correct?
$(A)$ $\Delta U = q + p \Delta V$
$(B)$ $\Delta G = \Delta H - T \Delta S$
$(C)$ $\Delta S = \frac{q_{rev}}{T}$
$(D)$ $\Delta H = \Delta U - \Delta nRT$
Choose the most appropriate answer from the options given below:

MediumJEE MAIN 2023

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For the combustion of one mole of acetic acid,the work done at $298 \ K$ is (in $J$)

DifficultMHT CET 2022

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Which of the following statements is incorrect?

Similar Questions

Which among the following are true for an irreversible isothermal expansion of an ideal gas?$(i)$ $W = -Q$$(ii)$ $\Delta U = 0$$(iii)$ $\Delta H \neq 0$$(iv)$ $\Delta T = 0$

$\Delta H_f^o$ of water is $-285.5\, kJ\, mol^{-1}$. If enthalpy of neutralisation of monoacidic strong base is $-57.3\, kJ\, mol^{-1}$,$\Delta H_f^o$ of $OH^{-}$ ion will be $.....\, kJ\, mol^{-1}$.

The heat of combustion of naphthalene $(C_{10}H_8(s))$ at constant volume is $-5133 \, kJ \, mol^{-1}$. The value of enthalpy change is .... $J$ $(R = 8.314 \, J \, K^{-1} \, mol^{-1}, T = 298 \, K)$.

Which of the following relations are correct?$(A)$ $\Delta U = q + p \Delta V$$(B)$ $\Delta G = \Delta H - T \Delta S$$(C)$ $\Delta S = \frac{q_{rev}}{T}$$(D)$ $\Delta H = \Delta U - \Delta nRT$Choose the most appropriate answer from the options given below:

For the combustion of one mole of acetic acid,the work done at $298 \ K$ is (in $J$)

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Which among the following are true for an irreversible isothermal expansion of an ideal gas?
$(i)$ $W = -Q$
$(ii)$ $\Delta U = 0$
$(iii)$ $\Delta H \neq 0$
$(iv)$ $\Delta T = 0$

Which of the following relations are correct?
$(A)$ $\Delta U = q + p \Delta V$
$(B)$ $\Delta G = \Delta H - T \Delta S$
$(C)$ $\Delta S = \frac{q_{rev}}{T}$
$(D)$ $\Delta H = \Delta U - \Delta nRT$
Choose the most appropriate answer from the options given below: