For which of the following reactions- - H- E-2RT-

The correct option is D NH_4HS(s)→ NH_3(g)+H_2S(g) In the equation, #160; Δ H=Δ E+Δ n_gRT Δ n_g=2 for the required #160;reactionA) #160; ...

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Thermodynamic Processes

For which of ...

Question

For which of the following reactions, $Δ H = Δ E + 2 R T$ ?

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

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N_{2} (g) + O_{2} (g) \to 2 N O (g)

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N H_{4} H S (s) \to N H_{3} (g) + H_{2} S (g)

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

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C (s) + O_{2} (g) ⟶ C O_{2} (g)

Δ H = Δ U + R T

N_{2} (g) + 3 H_{2} (g) ⟶ 2 N H_{3} (g)

Δ H = Δ U

N H_{4} H S (s) ⟶ N H_{3} (g) + H_{2} S (g)

Δ H = Δ U - 2 R T

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

Δ H = Δ U + 2 R T

2 S O_{2} (g) + O_{2} (g) ⟶ 2 S O_{3} (g)

Δ H = Δ U - R T

C (s) + O_{2} (g) ⟶ C O_{2} (g)

Δ H = Δ U + R T

N_{2} (g) + 3 H_{2} (g) ⟶ 2 N H_{3} (g)

Δ H = Δ U

N H_{4} H S (s) ⟶ N H_{3} (g) + H_{2} S (g)

Δ H = Δ U - 2 R T

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

Δ H = Δ U + 2 R T

2 S O_{2} (g) + O_{2} (g) ⟶ 2 S O_{3} (g)

Δ H = Δ U - R T

N_{2} (g) + 3 H_{2} (g) ⇌ 2 N H_{3} (g)

N_{2} (g) + O_{2} (g) ⇌ 2 N O (g)

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

2 H I_{(g)} ⟶ H_{2 (g)} + I_{2 (g)}

2 N H_{3 (g)} ⟶ N_{2 (g)} + 3 H_{2 (g)}

2 N O_{(g)} ⟶ N_{2 (g)} + O_{2 (g)}

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

I . 2 H I_{(g)} ⇌ H_{2 (g)} + I_{2 (g)}

I I . 2 N H_{3 (g)} ⇌ N_{2 (g)} + 3 H_{2 (g)}

I I I . 2 N O_{(g)} ⇌ N_{2 (g)} + O_{2 (g)}

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

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