Calculate the oxidation number of $C$ in the following: $C_{2} H_{6}, C_{4} H_{10}, C O, C O_{2}$ and $H C O_{3}^{-}$

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Solution

For $C_{2} H_{6}, C_{4} H_{1} 0$
Oxidation state for covalent compounds have not the proper definition as Oxidation state basically relates with charge carried by that certain elements within the compound but since $C_{2} H_{6}$ is covalent compound hence $C$ has not definite oxidation state.
For $C O$ ,
Oxidation state for carbon in compound $C O$ is $+ 2$ as the oxygen has $- 2$ charge.
For $C O_{2}$
Oxidation state of carbon $= + 4$
For $H C O_{3}^{- 1}$
Oxidation state of carbon = $+ 4$ .

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Find the oxidation number of elements in each case :

C

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and

C O_{2}

Out of the following pairs of compounds, the unsaturated compounds are :
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Q. Calculate the heat of formation of

C O_{2}

by following data.
(

Δ

Hc)

C_{2} H_{6}

- 397.8

Kcal
(

Δ

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C_{2} H_{6}

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(

Δ

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- 94.1

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Q. Balance the following equations by oxidation number method.

C O + F e_{3} O_{4} \to F e O + C O_{2}

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Calculate the oxidation number of C in the following: C2H6,C4H10,CO,CO2 and HCO−3

Calculate the oxidation number of $C$ in the following: $C_{2} H_{6}, C_{4} H_{10}, C O, C O_{2}$ and $H C O_{3}^{-}$