What is the change in oxidation number of carbon in the following reaction?
$N_{2} O_{4} (g) + 3 C O (g) \to N_{2} O (g) + 3 C O_{2} (g)$

+2 to +4

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0 to +4

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0 to +2

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+4 to –4

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Solution

The correct option is A +2 to +4
$C O_{2} \Rightarrow x + 2 (- 2) = 0$
$x = + 4$
$C O \Rightarrow x + 1 (- 2) = 0$
$x = + 2$
$_{2} O_{4} (g) + 3 + 2 C O (g) \to_{2} O (g) + 3 + 4 C O_{2} (g)$

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Similar questions

Q. What is the change in oxidation number of nitrogen in the following reaction?

N_{2} (g) + \frac{1}{2} O_{2} (g) \to N_{2} O (g)

Q. What is the change in oxidation number of carbon in the following reaction?

C H_{4} (g) + 4 C l_{2} (g) \to C C l_{4} (l) + 4 H C l (g)

Q. Enthalpies of formation of CO(g),

C O_{2} (g)

N_{2} O (g)

and

N_{2} O_{4} (g)

are

- 110, - 393.81

and

9.7 k J

m o l^{- 1}

respectively. Find the value of

△_{r} H

for the reaction :

N_{2} O_{4} (g) + 3 C O (g) \to N_{2} O (g) + 3 C O_{2} (g)

Enthalpies of formation of $C O_{(g)}, C O_{2 (g)}, N_{2} O_{(g)}$ and $N_{2} O_{4 (g)} a r e - 110 k J m o l^{- 1}, - 393 k J m o l^{- 1}, 81 k J m o l^{- 1}$ and $9.7 k J m o l^{- 1}$ respectively. Find the value of $Δ_{r} H$ for the reaction:
$N_{2} O_{4 (g)} + 3 C O_{(g)} \to N_{2} O_{(g)} + 3 C O_{2 (g)}$

Enthalpies of formation of CO₍_g_),CO₂₍_g_),N₂O₍_g₎and N₂O₄₍_g₎are –110 kJ mol^–1, – 393 kJ mol^–1, 81 kJ mol^–1 and 9.7 kJ mol^–1 respectively. Find the value of Δ_rH for the reaction:

N₂O₄₍_g₎ + 3CO₍_g₎ N₂O₍_g₎ + 3CO₂₍_g₎

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What is the change in oxidation number of carbon in the following reaction? N2O4(g)+3CO(g)→N2O(g)+3CO2(g)

The correct option is A +2 to +4CO2⇒x+2(−2)=0 x=+4 CO⇒x+1(−2)=0 x=+2 +4N2O4(g)+3+2CO(g)→+1N2O(g)+3+4CO2(g)

What is the change in oxidation number of carbon in the following reaction?
$N_{2} O_{4} (g) + 3 C O (g) \to N_{2} O (g) + 3 C O_{2} (g)$

The correct option is A +2 to +4
$C O_{2} \Rightarrow x + 2 (- 2) = 0$
$x = + 4$
$C O \Rightarrow x + 1 (- 2) = 0$
$x = + 2$
$_{2} O_{4} (g) + 3 + 2 C O (g) \to_{2} O (g) + 3 + 4 C O_{2} (g)$