For which of the following change - H - E-

The correct option is D H_2(g)+3H_2(g)→ 2NH_3(g) Δ H_(g)=Δ E_(g)+Δ n_(g)RT . And for A, B and C; Δ n_(g) = 0 so Δ H_(g)=Δ E_(g) but nbsp; ...

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For which of ...

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For which of the following change $Δ H \neq Δ E ?$

H_{2} (g) + I_{2} (g) \to 2 H I (g)

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H C l (a q) + N a O H (a q) \to N a C l (a q) + H_{2} O (l)

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

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H_{2} (g) + 3 H_{2} (g) \to 2 N H_{3} (g)

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Δ H \neq Δ U

6 C (s) + 3 H_{2} (g) ⟶ C_{6} H_{6} (l), Δ H = 49.0 k J

H_{2} (g) + 1 / 2 O_{2} (g) ⟶ H_{2} O (l), Δ H = - 285.8 k J

C (s) + O_{2} (g) ⟶ C O_{2} (g), Δ H = - 389.3 k J

6 C (s) + 3 H_{2} (g) \to C_{6} H_{6} (l); Δ H = + 45.9 k J

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

C (s) + O_{2} (g) \to C O_{2} (g); Δ H = - 393.5 k J

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)

C (s) + O_{2} (g) ⟶ C O_{2} (g)

Δ H = - 94 K c a l

H_{2} (g) + I / 2 O_{2} (g) ⟶ H_{2} O (l)

Δ H = - 68 K c a l

C_{2} H_{5} O H (l) + 3 O_{2} (g) ⟶ 2 C O_{2} (g) + 3 H_{2} O (l)

Δ H = - 327 K c a l

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