Advertisements
Advertisements
प्रश्न
Justify that the following reaction is redox reaction; identify the species oxidized/reduced, which acts as an oxidant and which acts as a reductant.
\[\ce{HF_{(aq)} + {OH}^-_{ (aq)}->H2O_{(l)} + {F}^ -_{ (aq)}}\]
Advertisements
उत्तर
\[\ce{HF_{(aq)} + {OH}^-_{ (aq)}->H2O_{(l)} + {F}^ -_{ (aq)}}\]
- Write oxidation number of all the atoms of reactants and products
- Since the oxidation numbers of all the species remain the same, this is NOT a redox reaction.
Result:
The given reaction is NOT a redox reaction.
APPEARS IN
संबंधित प्रश्न
Choose the correct option.
Oxidation number of oxygen in superoxide is
Choose the correct option.
The process \[\ce{SO2->S2Cl2}\] is
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.
NaH2PO4
Justify that the following reaction is redox reaction; identify the species oxidized/reduced, which acts as an oxidant and which acts as a reductant.
\[\ce{I2_{(aq)} + 2S2O^{2-}_{3(aq)}->S4O^{2-}_{6(aq)} + 2I^-_{ (aq)}}\]
What is oxidation?
Identify the following pair of species is in its oxidized state?
Cl2/Cl−
Provide the stock notation for the following compound:
Tl2O
Provide the stock notation for the following compound:
MnO
Assign oxidation number atom in the following species.
H3BO3
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)
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 redox couple is a stronger reducing agent?
Zn (E0 = - 0.76 V) and Fe (E0 = - 0.44 V)
The oxidation number of oxygen in peroxides is ____________.
What is the oxidation number of As in H3AsO3?
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?
When methane undergoes combustion in air, the oxidation number of C ____________.
Which of the following is INCORRECT?
The sum of oxidation states of all atoms in \[\ce{Cr2O^{2-}_7}\] ion is ______.
What is the oxidation number of Carbon in K2C2O4?
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?
What is the oxidation number of Cr in K2Cr2O7?
The oxidation number of oxygen in oxygen difluoride (OF2) and dioxygen difluoride (O2F2) respectively is ______.
