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If DeltaG for a reaction is negative, yo...

If `DeltaG` for a reaction is negative, you infer that the change is
(1)spontaneous
(2) non-spontaneous
(3) reversible
(4) irreversible
(5) equilibrium

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For a chemical reaction occurring at constant temperature and pressure show that DeltaG=-TDeltaS_("univ") , where DeltaG= change in free energy of the system and DeltaS_("univ") =change in entropy of the universe. Using this equation explain when a reaction at a constant temperature and pressure will be (i) spontaneous (ii) non-spontaneous (iii) at equilibrium.

It the free energy change for a reaction at 25^@C be 5.4 Kj Calculate the equilibrium constant for the reaction. State wheather the vaporisation of water at 110^@C in 1 atm pressure is a spontaneous or non spontaneous process.

At a given temperature and pressure, for a chemical reaction DeltaH gt0 and DeltaS lt 0 . The reaction is non-spontaneous at all temperature. But the reverse reaction is spontaneous at all temperature-give reason.

DeltaG of the system alone provides a criterion for the spontaneity of a process at constant temperature & pressure, DeltaG system lt 0 (spontaneous) DeltaG system = 0 (equilibrium) DeltaG system gt 0 {(non-spontaneous) Again DeltaG^@ is related to the equilibrium constant as follows : DeltaG^@ = 2.303 RT log K_e If both DeltaH and Delta S are negative, the reaction will be spontaneous

At 25^(@)C and 1 atm pressure, for the reaction 3O_(2)(g)to2O_(3)(g)," "DeltaH=286kJ and DeltaS=-137.2J*K^(-1) . Is this reaction spontaneous? Does the spontaneity of thir reaction depend on temperature? Is the reverse reaction spontaneous ? If so, then why? does the spontaneity of the reverse reaction depend on temperature?

At a certain temperature and pressure, DeltaH=0 for the reaction: X+X= X_(2) . Show that the reaction is non-spontaneous at this temperature and pressure.

Are the given statements correct? (1) if heat is absorbed in a chemical reaction, the reaction cannot be spontaneous. (2) the entropy of the system may decrease in a reaction, but the reaction can occur spontaneously.

Consider the reaction, Ato2B , if the free energy per mole of A is G_(A) and that of B is G_(B) then what will the relation be between G_(A) and G_(B) when the reaction (i) occurs spontaneously and (ii) is at equilibrium?

The given graph indicates the change in concentrations of A and B of a reversible reaction, A hArr nB at constant temperature. If the value of equilibrium constant of the reaction is 1.2 at that temperature, then find the value of n.

PATHFINDER-THERMODYNAMICS-QUESTION BANK
  1. Assuming enthalpy of combustion of hydrogen at 273K is -286 kJ/mol and...

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  2. A piston filled with 0.04mole of an ideal gas expa nds teversibly from...

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  3. If DeltaG for a reaction is negative, you infer that the change is (1...

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  4. In order to decompose 9g water 142.5 kJ heat is required. Hence, the e...

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  5. The enthalpy of combustion of C6H6(l) is -3250 kJ. When 0.39 g of benz...

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  6. The intensive property among these quantities is

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  7. Hess's law states that

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  8. A gas can expand from 100 mL to 250 mL. under a constant pressure of 2...

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  9. For a Process to be spontaneous

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  10. Assertion DeltaH and DeltaE are almost the same for the reaction, N2(g...

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  11. Assertion The increase in internal energy (DeltaE) for the vaporisatio...

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  12. Which of the following has DeltaS^@ greater than zero?

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  13. The heat of reaction for C(10)H8(s) + 12O2,(g) rarr10CO2,(g) + 4H2O(l...

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  14. Which law states entropy of all pure crystalline solids is zero at abs...

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  15. The enthalpies of formation of C2H2(g) and C6H6(g) at 298 K are 230 an...

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  16. For an ideal gas, the Joule Thomson coefficient is

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  17. The relation of DeltaH and DeltaE is represented as

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  18. Calculate the temperature at which DeltaG = -5.2 kJ mol^-1, DeltaH = 1...

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  19. When ice melts into water entropy

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  20. Which of the following Is not the extensive property?

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