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The second law of thermodynamics states ...

The second law of thermodynamics states that

A

all machines have an efficiency unity

B

energy can neither be created nor destroyed

C

all spontaneous processes are thermodynamically irreversible

D

heat can be completely converted into work without leaving changes in the system

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The correct Answer is:
C
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TARGET PUBLICATION-CHEMICAL THERMODYNAMICS AND ENERGETICS -EVALUATION TEST
  1. The second law of thermodynamics states that

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  2. The enthalpy change for a reaction does not depend upon:

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  3. The internal energy change when a system goes fromk state A to B is 40...

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  4. Following gases have equal masses at the same temperature, pressure an...

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  5. The standard enthalpy of formation (Delta(f)H^(@)) at 298K for methan...

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  6. (Delta H - Delta U) for the formation of carbon monoxide (CO) from its...

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  7. Identify the correct statement regarding a spontaneous process.

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  8. Standard entropy of X(2) , Y(2) and XY(3) are 60, 40 and 50JK^(-1)mol...

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  9. The heats of neutralisation of CH3 - COOH , H-COOH,HCN and H2 S are -1...

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  10. The bond dissociation energy of gaseous H(2), Cl(2) and HCl are 104, 5...

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  11. The difference between the heats of reaction at constant pressure and ...

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  12. Given standard enthalpy of formation of CO(-110 "KJ mol"^(-1)) and CO(...

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  13. H(2)(g)+1//2O(2)(g)=H(2)O(l) , Delta H(298 K)=-68.32 Kcal. Heat of vap...

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  14. The heat change at constant volume for the decomposition of silver (I)...

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  15. Which of the following value of DeltaH(f)^(@) represent that the produ...

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  16. The enthalpy change (DeltaH) for the process N2H(4(g)) to 2N((g)) + 4H...

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  17. For the two equations given below: H(2)(g)+1//2O(2)(g)toH(2)O(l)+x(1...

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  18. For an endothermic reaction, where Delta H represents the enthalpy of ...

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  19. The entropy chnge for a non-spontaneous reaction is 140 J/K.mole at 29...

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  20. The entropy change for a certain non-spontaneous reaction is 150 J/K.m...

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  21. C(2)H(4) +CI(2) rarr C(2)H(4)CI(2) DeltaH =- 270.6 kJ mol^(-1)K^(-1)...

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