Advertisements
Advertisements
Question
In which chemical reaction does carbon exhibit variation of oxidation state from - 4 to + 4? Write a balanced chemical reaction.
Advertisements
Solution
In the combustion of methane, carbon exhibits variation from – 4 to + 4. The reaction is as follows:
\[\ce{CH4 + 2O2->CO2 + 2H2O}\]
In CH4, the oxidation state of carbon is – 4 while in CO2, the oxidation state of carbon is + 4.
APPEARS IN
RELATED QUESTIONS
Choose the correct option.
Oxidation number of oxygen in superoxide is
Calculate the oxidation number of the underlined atom.
H2SO4
Calculate the oxidation number of the underlined atom.
H3PO3
Calculate the oxidation number of the underlined atom.
H2S4O6
Calculate the oxidation number of the underlined atom.
Cr2O72−
Justify that the following reaction is redox reaction; identify the species oxidized/reduced, which acts as an oxidant and which acts as a reductant.
\[\ce{I2_{(aq)} + 2S2O^{2-}_{3(aq)}->S4O^{2-}_{6(aq)} + 2I^-_{ (aq)}}\]
Justify that the following reaction is redox reaction; identify the species oxidized/reduced, which acts as an oxidant and which acts as a reductant.
\[\ce{HF_{(aq)} + {OH}^-_{ (aq)}->H2O_{(l)} + {F}^ -_{ (aq)}}\]
Provide the stock notation for the following compound:
Fe2O3
Provide the stock notation for the following compound:
MnO
Assign oxidation number atom in the following species.
\[\ce{Cr(OH)^Θ_4}\]
Assign oxidation number atom in the following species.
Na2S2O3
Assign oxidation number atom in the following species.
H3BO3
Which of the following redox couple is a stronger oxidizing agent?
Cl2 (E0 = 1.36 V) and Br2 (E0 = 1.09 V)
Which of the following redox couple is a stronger reducing agent?
Li (E0 = - 3.05 V) and Mg (E0 = - 2.36 V)
Which of the following is NOT an example of redox reaction?
In the complex [Co(en)3]Cl3, ____________.
In the following reaction, the oxidation number of Cr changes.
\[\ce{ClO^-_{( aq)} + Cr(OH)^-_{4(aq)} -> CrO^{2-}_{4(aq)} + Cl^-_{( aq)} (basic)}\]
The oxidation number of sulphur in S8 molecule is ______.
Match the following.
| Compound | Oxidation no. of underlined element |
| i. \[\ce{\underline{C}_4H4O^{2-}_6}\] | a. +2.5 |
| ii. \[\ce{\underline{N}_3H}\] | b. +1.5 |
| iii. \[\ce{Mg2\underline{P}_2O7}\] | c. +5 |
| iv. \[\ce{Na2\underline{S}_4O6}\] | d. `-1//3` |
In which of the following, oxidation number of oxygen is +2?
All of these are CORRECT for the complex K4[Mn(CN)6], EXCEPT:
In which among the following compounds, oxidation number of nitrogen is + 5?
When methane undergoes combustion in air, the oxidation number of C ____________.
The sum of oxidation states of all atoms in \[\ce{Cr2O^{2-}_7}\] ion is ______.
Which among the following pair of elements show highest oxidation state +7 in their different compounds?
Among group 16 elements, which one does not show −2 oxidation state?
Which of the following changes exhibit that nitrogen undergoes oxidation?
