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प्रश्न
In which chemical reaction does carbon exhibit variation of oxidation state from - 4 to + 4? Write a balanced chemical reaction.
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उत्तर
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.
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संबंधित प्रश्न
In which reaction does nitrogen exhibit variation of oxidation state from –3 to +5?
Calculate the oxidation number of the underlined atom.
H2SO4
Calculate the oxidation number of the underlined atom.
HNO3
Calculate the oxidation number of the underlined atom.
H2S4O6
Justify that the following reaction is redox reaction; identify the species oxidized/reduced, which acts as an oxidant and which acts as a reductant.
\[\ce{I2_{(aq)} + 2S2O^{2-}_{3(aq)}->S4O^{2-}_{6(aq)} + 2I^-_{ (aq)}}\]
Identify the following pair of species is in its oxidized state?
Cl2/Cl−
Provide the stock notation for the following compound:
HAuCl4
Provide the stock notation for the following compound:
Tl2O
Which of the following redox couple is a stronger oxidizing agent?
\[\ce{MnO^Θ_4}\](E0 = 1.51 V) and \[\ce{Cr2O^{2Θ}_7}\](E0 = 1.33 V)
Complete the following table:
Assign oxidation number to the underlined species and write Stock notation of compound
| Compound | Oxidation number | Stock notation |
| AuCl3 | ||
| SnCl2 | ||
| \[\ce{\underline{{V}}_2O^{4-}_{7}}\] | ||
| \[\ce{\underline{{Pt}}Cl^2-_6}\] | ||
| H3AsO3 |
Oxidation state of Xe in XeOF4 is ____________.
What is the oxidation number of As in H3AsO3?
Which of the following is CORRECT?
\[\ce{H3PO4_{(aq)} + 3KOH_{(aq)} -> K3PO4_{(aq)} + 3H2O_{(l)}}\]
In the following reaction, the oxidation number of Cr changes.
\[\ce{ClO^-_{( aq)} + Cr(OH)^-_{4(aq)} -> CrO^{2-}_{4(aq)} + Cl^-_{( aq)} (basic)}\]
Identify the strongest oxidising agent.
\[\ce{Na^+ + e^- -> Na}\]; E0 = −2.714 V
\[\ce{Pt^{2+} + 2e^- -> Pt}\]; E0 = +1.200 V
\[\ce{I2 + 2e^- -> 2I^-}\]; E0 = + 0.535 V
\[\ce{Co^{2+} + 2e^- -> Co}\]; 0 = −0.280 V
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 among the following compounds, oxidation number of nitrogen is + 5?
Stock notations are used to specify the oxidation numbers of ____________.
The sum of oxidation number of all atoms in \[\ce{SnO^{2-}_3}\] ion is _______.
Which among the following pair of elements show highest oxidation state +7 in their different compounds?
The oxidation number of phosphorous in Ba(H2PO2)2 is ______.
What is the oxidation number of Cr in K2Cr2O7?
The brown ring complex is formulated as [Fe(H2O)5NO]SO4. The oxidation number of iron is ______.
Which of the following explanation is correct about the given below reaction?
\[\ce{Cr2O^2-_7 + H2O -> 2CrO^2-_4 + 2H+}\]
Among group 16 elements, which one does not show −2 oxidation state?
