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Statement-1: Under adiabatic free expans...

Statement-1: Under adiabatic free expansion, `((dU)/(dV))_(T)` is +ve when attractive forces are dominant between gas molecules [U,V,T respectively]
Statement-2: Internal energy is a state function.

A

Statement-1 is true, Statement-2, is true, Statement -2 is a correct explanation for statement-1

B

Statement-1 is true, Statement-2, is true, Statement -2 is not a correct explanation for statement-1

C

Statement-1 is true, Statement-2 is false

D

Statement-1 is false, Statement-2 is true

Text Solution

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The correct Answer is:
B
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Statement-1: The internal energy of a system does not change when there is not change in temperature Statement-2: The internal energy of a gaseous system is state function.

Statement-1: Adiabatic free expansion of any subatance in a cosed system will not cause any change in temperature of the substance. Statement-2: In adiabatic free expansion of any substance in a closed system, internal energy will remain constant.

Statement-1: Due to adiabatic free expansion temperature of real gas may increase. Statement-2 : In adiabatic free expansion, temperature is always constant irrespective of real or ideal gas

Statement-1: In kinetic theory of gases, we do not take into account the change in gravitational potential energy of the molecules. Statement-2: The internal energy of a gas depends on the interaction between gas molecules. This interaction is not affected by the change in gravitational potential energy of the molecules.

Identify the option which correctly represents set of true (T) false (F) statements: Statement :1 In an adiabatic free expansion, entropy of system remains constant. Statement-2: For every isothermal process, internal energy of the system remains contant. Statement-3: Molar enthalpy is an intensive parameter. Statement-4: For every reversible cyclic process, final state of surroundings is same as that of initial state of surroundings.

Statement-1 : When an ideal gas is freely expanded change in internal energy of gas is zero, where as when real gas is expanded freely it's internal energy decreases. Statement-2 : There is no intermolecular force of attraction in ideal gas.

Statement-1 : The amount of heat change during the isothermal free expansion of an ideal gas is zero. Statement-2: There are no intermolecular forces of attraction among the gas molecules, in case of real gas at given pressure.

Statement-1 : In an adiabatic process, change in internal energy of a gas is equal to work done on/by the gas in the process. Statement-2 : This is because temp.of gas remains constant in an adiabatic process.

NARAYNA-THERMODYNAMICS-Level -V
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  3. Statement-1: There is a natural asymmetry between work to heat and con...

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  4. Statement -1: Entropy change in reversible adiabatic expansion of an i...

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  5. Statement -1: The Standard free energy changes of all spontaneously oc...

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  6. Statement -1: Enthalpy and entropy of any elements substance in the st...

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  7. Statement-1: A reaction which is spontaneous and accompained by decrea...

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  8. Statement -1: Many endothermic reactions that are not spontaneous at r...

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  9. Statement-1: Decrease of free energy during the process under constant...

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  10. Statement-1: All combustion reactions are exothermic. Statement-2: E...

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  11. Statement-1: Due to adiabatic free expansion temperature of real gas m...

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  12. Statement-1: Under adiabatic free expansion, ((dU)/(dV))(T) is +ve whe...

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  13. Statement-1: At low temperatures, DH is the dominant factor for sponta...

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  14. Statement-1: A reaction which is spontaneous and accompained by decrea...

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  15. The temperature of 1 mole helium gas is increased by 1^@C. Find the in...

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  16. An ideal gas is taken through the cycle A rarr B rarr C rarr A As show...

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  17. If 2kcal heat is given to a system and 6 kcal work is done on the syst...

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  19. Molar enthalpy of vaporization of a liquid is 2.6 kJ. If boiling point...

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  20. The chemical reaction : A rarr P, Delta H^(@) = 2.8 kJ is spontaneous ...

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