AIEEE 2003 | Thermodynamics Question 204 | Chemistry

If at 298 K the bond energies of C - H, C - C, C = C and H - H bonds are respectively 414, 347, 615 and 435 kJ/mol, the value of enthalpy change for the reaction
H₂C = CH₂(g) + H₂(g) $$\to$$ H₃C - CH₃(g) at 298 K will be :

- 250 kJ

+ 125 kJ

- 125 kJ

+ 250 kJ

AIEEE 2003

MCQ (Single Correct Answer)

-1

The correct relationship between free energy change in a reaction and the corresponding equilibrium constant K_c is :

- $$\Delta G$$ = RT ln K_c

$$\Delta G^o$$ = RT ln K_c

- $$\Delta G^o$$ = RT ln K_c

$$\Delta G$$ = RT ln K_c

AIEEE 2003

MCQ (Single Correct Answer)

-1

In an irreversible process taking place at constant T and P and in which only pressure-volume work is being done, the change in Gibbs free energy (dG) and change in entropy (dS), satisfy the criteria :

(dS)_{V, E} > 0, (dG)_{T, P} < 0

(dS)_{V, E} = 0, (dG)_{T, P} = 0

(dS)_{V, E} = 0, (dG)_{T, P} > 0

(dS)_{V, E} < 0, (dG)_{T, P} < 0

AIEEE 2003

MCQ (Single Correct Answer)

-1

The enthalpy change for a reaction does not depend upon :

use of different reactants for the same product

the nature of intermediate reaction steps

the differences in initial or final temperature of involved substances

the physical states of reactants and products