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Rutherford's Model

31 Calculate ...

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31 Calculate the standard free energy change for the reaction 4 NH3 (g) + 5O2 (g) 4NO (g) + 6 H2O (l) Given that the free energy change for the formation of NH3 (g), NO (g) and H2O (l) are -16.8, +86.7 and -273.2 kJ/mole respectively. Predict the feasibility of the reaction.

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Q. Calculate the standard free energy change for the reaction,

H_{2} (g) + I_{2} (g) ⟶ 2 H I (g)

Δ H^{⊖} = + 51.9 k J

Given that the standard entropies

(Δ S^{⊖})

H_{2}

I_{2}

H I

130.6

116.7

206.3 J K^{- 1} m o l^{- 1}

, respectively.

Predict whether the reaction is feasible at the standard state or not?

Q. Calculate the standard enthalpy change and standard internal energy change for the following reaction at 300K :

O F_{2} (g) + H_{2} O (g) \to O_{2} (g) + 2 H F (g)

Given that the standard enthalpy of formation of

O F_{2}

H_{2} O

H F

23 k j m o l^{- 1}

- 241.8 k j m o l^{- 1}

- 268.6 k j m o l^{- 1}

Q. Calculate the free energy change at

298 K

for the reaction :

B r_{2} (l) + C l_{2} (g) \to 2 B r C l (g)

. For the reaction

Δ H^{o} = 29.3 k J

& the entropies of

B r_{2} (l), C l_{2} (g)

& BrCl(g) at the

298 K

152.3, 223.0, 239.7

J m o l^{1} K^{1}

Q. The equilibrium constant for the reaction given below is

2.0 \times 10^{- 7}

at 300 K. Calculate the standard free energy change for the reaction.

P C l_{5} (g) ⇌ P C l_{3} (g) + C l_{2} (g)

Also, calculate the standard entropy change if,

Δ H^{\circ} = 28.40 k J m o l^{- 1}

Q. The standard free energy change for the following reaction is -210 kJ. What is the standard cell potential?

2 H_{2} O_{2} (a q) \to 2 H_{2} O (l) + O_{2} (g)

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