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Valency and Oxidation State

In which of t...

Question

In which of the following compounds is the oxidation state of carbon is zero?

C H_{4}

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C H_{3} O H

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H C O O H

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C_{6} H_{12} O_{6}

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Solution

The correct option is C $C_{6} H_{12} O_{6}$
Let $x$ be the oxidation state of carbon.
Since, the overall charge on the complex is $0$ , the sum of oxidation states of all elements in it should be equal to $0$ .
a. $C H_{4} : x + 4 = 0 \to x = - 4$
b. $C H_{3} O H : x + 4 - 2 = 0 \Rightarrow x = - 2$
c. $H C O O H : x + 2 - 4 = 0 \Rightarrow x = 2$
d. $C_{6} H_{12} O_{6} : 6 x + 12 - 12 = 0 \Rightarrow x = 0$
Hence, the oxidation state of carbon is zero in $C_{6} H_{12} O_{6}$ .

Suggest Corrections

Similar questions

{Δ H}_{f}^{o}

C_{6} H_{12} O_{6} (s)

Δ H_{c o m b .}

C_{6} H_{12} O_{6} (s) = - 2816 k J {m o l}^{- 1}

{Δ H}_{f}^{o}

{C O}_{2} (g) = - 393.5 J {m o l}^{- 1}

{Δ H}_{f (H_{2} O)}^{o} = - 285.9 k J {m o l}^{- 1}

Δ H_{f}^{o}

C_{6} H_{12} O_{6} (s)

Δ H_{c o m b} [C_{6} H_{12} O_{6} (s)] = - 2816 k J / m o l

Δ H_{f}^{o}

{C O}_{2} (g) = - 393.5 k J / m o l

Δ H_{f}^{o}

H_{2} O (l) = - 285.9 k J / m o l

C_{6} H_{12} O_{6}

C_{12} H_{22} O_{11} + H_{2} O I n v e r t a s e - ----- \to C_{6} H_{12} O_{6} A + C_{6} H_{12} O_{6} B

C_{6} H_{12} O_{6} z y m a s e - --- \to 2 C_{2} H_{5} O H + 2 {C O}_{2}

A

B

(C_{6} H_{6})

(C_{6} H_{12} O_{6})

(C_{2} H_{2})

(H_{2} O_{2})

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