The free energy change for the following reactions are given below C 2 H 2 g - 5 - 2 O 2 g - 2 CO 2 g - H 2 O l - G 0 -1234kJ C s - O 2 g - CO 2 g - G 0 -394kJ H 2 g - 1 - 2 O 2 g - H 2 O l - G 0 -237kJWhat is the standard free energy change for the reaction- H 2 g -2C s - C 2 H 2 g

The correct option is D 209 kJRequired equation H_2(g)+2C(s)⟶ C_2H_2 (g) #160; #160; G Reverse equation 1 Multiply equation 2 with ...

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Entropy

The free ener...

Question

The free energy change for the following reactions are given below
$C_{2} H_{2} (g) + \frac{5}{2} O_{2} (g) ⟶ 2 {C O}_{2} (g) + H_{2} O (l); △ G^{0} = 1234 k J$
$C (s) + O_{2} (g) ⟶ {C O}_{2} (g); △ G^{0} = - 394 k J$
$H_{2} (g) + \frac{1}{2} O_{2} (g) ⟶ H_{2} O (l); △ G^{0} = - 237 k J$
What is the standard free energy change for the reaction,
$H_{2} (g) + 2 C (s) \to C_{2} H_{2} (g)$

-209 kJ

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-2259 kJ

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+2259 kJ

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209 kJ

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2 C (s) + 2 O_{2} (g) \to 2 C O_{2} (g)

Δ H = - 787

H_{2} (g) + 1_{/ 2} O_{2} (g) \to H_{2} O (l)

Δ

= - 286

C_{2} H_{2} (g) + \frac{5}{2} O_{2} (g) \to 2 C O_{2} (g) + H_{2} O (l)

Δ

= - 1310

H_{2} (g) + \frac{1}{2} O_{2} (g) ⟶ H_{2} O (l) + x_{1}

k J

H_{2} (g) + \frac{1}{2} O_{2} (g) ⟶ H_{2} O (g) + x_{2}

k J

2 C (s) + 2 O_{2} (g) ⟶ 2 C O_{2} (g); Δ H = - 787 k J . . . (i)

H_{2} (g) + \frac{1}{2} O_{2} (g) ⟶ H_{2} O (l); Δ H = - 286 k J . . . (i i)

C_{2} H_{2} (g) + \frac{5}{2} O_{2} (g) ⟶ 2 C O_{2} (g) + 3 H_{2} O (l) . . . . (i i i)

Δ H = - 1301 k J

H_{(a q)}^{+} + O H_{(a q)}^{-} = H_{2} O_{(l)}, Δ H = - X_{1}

m o l^{- 1}

H_{2 (g)} + \frac{1}{2} O_{2 (g)} = H_{2} O_{(l)}, Δ H = X_{2}

m o l^{- 1}

C O_{2 (g)} + H_{2 (g)} = C O_{(g)} + H_{2} O_{(l)} - X_{3}

m o l^{- 1}

C_{2} H_{2 (g)} + \frac{5}{2} O_{2 (g)} = 2 C O_{2 (g)} + H_{2} O_{(l)} + X_{4}

m o l^{- 1}

H_{2} O_{(l)}

C_{2} H_{2}

C_{2} H_{4}

H_{2} (g) + \frac{1}{2} O_{2} (g) ⟶ H_{2} O (l); Δ H = - 68.32 k c a l

C_{2} H_{2} (g) + \frac{1}{2} O_{2} (g) ⟶ 2 C O_{2} (g) + H_{2} O (l); Δ H = - 310.61 k c a l

C_{2} H_{4} (g) + 3 O_{2} (g) ⟶ 2 C O_{2} (g) + H_{2} O (l); Δ H = - 337.32 k c a l

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