For which reaction will ∆H - ∆E = 0 ? Assume tha

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 Multiple Choice QuestionsMultiple Choice Questions

331.

Which thermodynamic parameter is not a state function?

  • q at constant pressure

  • q at constant volume

  • W at adiabatic

  • W at isothermal


332.

Assertion: For an isolated system, q is zero.

Reason : In an isolated system, change in U and V is zero.

  • If both assertion and reason are true and reason is the correct explanation of assertion.

  • If both assertion and reason are true but reason is not the correct explanation of assertion.

  • If assertion is true but reason is false.

  • If both assertion and reason are false.


333.

Assertion : Entropy of system increases for a spontaneous reaction.

Reason : Enthalpy of reaction always decreases for spontaneous reaction.

  • If both assertion and reason are true and reason is the correct explanation of assertion.

  • If both assertion and reason are true but reason is not the correct explanation of assertion.

  • If assertion is true but reason is false.

  • If both assertion and reason are false.


334.

Assertion : Catalyst changes Gibbs free energy of system.

Reason : Catalyst changes pre-exponential factor of a chemical reaction.

  • If both assertion and reason are true and reason is the correct explanation of assertion.

  • If both assertion and reason are true but reason is not the correct explanation of assertion.

  • If assertion is true but reason is false.

  • If both assertion and reason are false.


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335.

Assertion : A process is called adiabatic if the system does not exchange heat with the surroundings.

Reason : It does not not involve increase or decrease in temperature of the system.

  • If both assertion and reason are true and reason is the correct explanation of assertion

  • If both assertion and reason are true but reason is not the correct explanation of assertion.

  • If assertion is true but reason is false.

  • If both assertion and reason are false.


336.

Heat of combustion of C and CO are -394 and -285 kJ respectively , so heat of formation of CO in kJ/mol is :

  • - 218

  • - 109

  • + 109

  • + 218


337.

For endothermic reaction :

  • Ea > Ea'

  • Ea = Ea'

  • Ea < Ea'

  • None of these


338.

The enthalpy of formation of CO(g), CO2(g), N2O(g), and N2O4(g) is -110, -393, +811 and 10 kJ/mol respectively. For the reaction, N2O4 + 3CO(g) N2O(g)+ 3CO2(g)Hr (kJ/mol) is

  • -212

  • +212

  • +48

  • -48


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339.

The difference between heat of reaction at constant pressure and constant volume of the reaction :

2C6H6 (l) + 15O2 (g)  12CO2 + 6H2O (l)

at 25°C (in kJ) is :

  • - 7.43

  • 3.72

  • - 3.72

  • 7.43


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340.

For which reaction will H - E = 0 ? Assume that each reaction is carried out in an open container .

  • 2CO2 (g) + O2 (g)  2CO2 (g)

  • PCl5 (g)  PCl3 (g) + Cl2 (g)

  • H2 (g) + Br2 (g)  2HBr (g)

  • C (s) + 2H2O (g)  2H2 (g) + CO2 (g)


C.

H2 (g) + Br2 (g)  2HBr (g)

H = E + ngRT

For reaction H2 (g) + Br2 (g)  2HBr (g)

ng = 0 , while for other ng  0

Thus , H = E + 0 x RT

H - E = 0


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