For the reaction H 2 g -1-2 O 2 g - H 2 O l - - H -285-8 kJ mol -1- S -0-163 kJ mol -1 K -1- What is the value of free energychange 27- C for the reaction-A- -236-9 kJmol -1B- -281-4 kJmol -1C- -334-7 kJmol -1D- -334-7 kJmol -1

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Mass Energy Equivalence

For the react...

Question

For the reaction $H_{2} (g) + \frac{1}{2} O_{2} (g) \to H_{2} O (l), Δ H = - 285.8 k J m o l^{- 1} Δ S = - 0.163 k J m o l^{- 1} K^{- 1}$ . What is the value of free energy change $27^{\circ} C$ for the reaction.

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2 A l (s) + 1 \frac{1}{2} O_{2} (g) ⟶ A l_{2} O_{3} (s), Δ H = - 166.78 k J

H_{2} (g) + \frac{1}{2} O_{2} (g) ⟶ H_{2} O (l), Δ H = - 285.9 k J

Δ H

A l_{2} O_{3} (s) ⟶ 2 A l (s) + 1 \frac{1}{2} O_{2} (g)

Consider the following reactions:

(a) $H^{+} (a q) + O H^{-} (a q) \to H_{2} O (l) Δ H = - x_{1} k J m o l^{- 1}$

(b) $H_{2} (g) + \frac{1}{2} O_{2} (g) \to H_{2} O (l) Δ H = - x_{2} k J m o l^{- 1}$

(d) $C_{2} H_{2} (g) + \frac{5}{2} O_{2} (g) \to 2 C O_{2} (g) + H_{2} O (l) Δ H = x_{4} k J m o l^{- 1}$

Enthalpy of formation of $H_{2} O (l)$ is

H^{+} (a q) + O H^{-} (a q) = H_{2} O (l); Δ H = - X_{1} k J . m o l^{- 1}

H_{2} (g) + \frac{1}{2} O_{2} (g) = H_{2} O (l); Δ H = - X_{2} k J . m o l^{- 1}

C O_{2} (g) + H_{2} (g) = C O (g) + H_{2} O (l); Δ H = + X_{3} k J . m o l^{- 1}

C_{2} H_{2} (g) + \frac{5}{2} O_{2} (g) = 2 C O (g) + H_{2} O (l); Δ H = + X_{4} k J . m o l^{- 1}

H_{2} O (l)

C_{2} H_{2} (g) + \frac{5}{2} O_{2} (g) ⟶ 2 {C O}_{2} (g) + H_{2} O (l); △ G^{0} = 1234 k J

C (s) + O_{2} (g) ⟶ {C O}_{2} (g); △ G^{0} = - 394 k J

H_{2} (g) + \frac{1}{2} O_{2} (g) ⟶ H_{2} O (l); △ G^{0} = - 237 k J

H_{2} (g) + 2 C (s) \to C_{2} H_{2} (g)

H_{2} O (g) ⇌ H_{2} (g) + \frac{1}{2} O_{2} (g), Δ H^{\circ} = 200 k J m o l^{- 1} Δ S^{\circ} = 40 J m o l^{- 1}

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