For the reaction- 3N2Og-2NH3g- 4N2g-3H2Og- - Ho-879-6 kJIf - Hof-NH3g-45-9 kJ mol-1- - Hof-H2Og-241-8 kJ mol-1Then - Hof-N2Og- will be-

The correct option is B +82 kJ 3NO_2_(g)+2NH_3_(g)⟶4N_2_(g)+3H_2O_(g); Δ H^o= 879.6KJ Δ H^o=ΣΔ H^o_f(products) ΣΔ H^o_f(reactants) #160; # ...

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Heat of Formation

For the react...

Question

For the reaction,
$3 N_{2} O (g) + 2 N H_{3} (g) \to 4 N_{2} (g) + 3 H_{2} O (g)$ ; $Δ H^{o} = - 879.6$ kJ
If $Δ H_{f}^{o} [N H_{3} (g)] = - 45.9$ kJ $m o l^{- 1}$ ; $Δ H_{f}^{o} [H_{2} O (g)] = - 241.8$ kJ $m o l^{- 1}$
Then $Δ H_{f}^{o} [N_{2} O (g)]$ will be:

+ 246

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+ 82

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- 82

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- 246

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Δ H_{f}^{o}

C O_{2 (g)}

C O_{(g)}

H_{2} O_{(g)}

- 393.5

- 110.5

- 241.8

m o l^{- 1}

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

S - S

(i) C_{2} H_{5} - S - C_{2} H_{5} (g)

Δ H_{f}^{o} = - 147.2 k J / m o l

(i i) C_{2} H_{5} - S - S - C_{2} H_{5} (g)

Δ H_{f}^{o} = - 201.9 k J / m o l

(i i i) S (g)

Δ H_{f}^{o} = 222.8 k J / m o l

Δ H_{f}^{o}

\frac{1}{2} H_{2} (g) + \frac{1}{2} C l_{2} (g) \to H C l (g)

Δ H = - 92.4

H C l (g) + N H_{2} O

\to H^{+} (a q) + C l^{-} (a q)

Δ H = - 74.8

Δ H_{f}^{o} (H^{+} (a q)) = 0.0

N_{2} O

△_{f} H^{o} o f N_{2} O = 82 k J m o l^{- 1},

N \equiv N, 946 k J m o l^{- 1}; N = N, 418 k J m o l^{- 1};

O = O, 498 k J m o l^{- 1}; N = O, 607 k J m o l^{- 1}

N_{2} O

△_{f} H^{o} o f N_{2} O = 82 k J m o l^{- 1},

N \equiv N, 946 k J m o l^{- 1}; N = N, 418 k J m o l^{- 1};

O = O, 498 k J m o l^{- 1}; N = O, 607 k J m o l^{- 1}

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