Advertisements
Advertisements
प्रश्न
Which of the following is not an example of redox reaction?
विकल्प
\[\ce{CuO + H2 -> Cu + H2O}\]
\[\ce{Fe2O3 + 3CO -> 2Fe + 3CO2}\]
\[\ce{2K + F2 -> 2KF}\]
\[\ce{BaCl2 + H2SO4 -> BaSO4 + 2HCl}\]
Advertisements
उत्तर
\[\ce{BaCl2 + H2SO4 -> BaSO4 + 2HCl}\]
Explanation:
Redox reaction is defined as the simultaneous oxidation and reduction of reacting species. Thus, change in oxidation state will decide whether a reaction is redox or not. Thus, assigning the oxidation states as:
(i) \[\ce{CuO + H2 -> Cu + H2O}\]
Here, oxidation of H and reduction of \[\ce{Cu}\] is taking place.
(ii) \[\ce{Fe2O3 + 3CO -> 2Fe + 3CO2}\]
Here, oxidation of \[\ce{C}\] and reduction of \[\ce{Fe}\] is taking place.
(iii) \[\ce{2K + F2 -> 2KF}\]
Here, the oxidation of \[\ce{K}\] and reduction of \[\ce{F}\] is taking place.
(iv) \[\ce{BaCl2 + H2SO4 -> BaSO4 + 2HCl}\]
This is not a redox reaction, but it is a double displacement reaction.
APPEARS IN
संबंधित प्रश्न
Justify that the following reaction is redox reaction:
\[\ce{4BCl3(g) + 3LiAlH4(s) → 2B2H6(g) + 3LiCl(s) + 3 AlCl3(s)}\]
Justify that the following reaction is redox reaction:
\[\ce{2K(s) + F2(g) → 2K+F– (s)}\]
Suggest a list of the substances where carbon can exhibit oxidation states from –4 to +4 and nitrogen from –3 to +5.
How do you count for the following observations?
When concentrated sulphuric acid is added to an inorganic mixture containing chloride, we get colourless pungent-smelling gas HCl, but if the mixture contains bromide then we get red vapour of bromine. Why?
Identify the substance oxidised, reduced, oxidising agent and reducing agent for the following reaction:
\[\ce{HCHO(l) + 2[Ag (NH3)2]+(aq) + 3OH–(aq) → 2Ag(s) + HCOO–(aq) + 4NH3(aq) + 2H2O(l)}\]
Identify the substance oxidised, reduced, oxidising agent and reducing agent for the following reaction:
\[\ce{Pb(s) + PbO2(s) + 2H2SO4(aq) → 2PbSO4(s) + 2H2O(l)}\]
Refer to the periodic table given in your book and now answer the following question:
Select three metals that can show disproportionation reaction.
Arrange the following metals in the order in which they displace each other from the solution of their salts.
Al, Cu, Fe, Mg and Zn.
Identify disproportionation reaction
Which of the following elements does not show disproportionation tendency?
Which of the following statement(s) is/are not true about the following decomposition reaction.
\[\ce{2KClO3 -> 2KCl + 3O2}\]
(i) Potassium is undergoing oxidation.
(ii) Chlorine is undergoing oxidation.
(iii) Oxygen is reduced.
(iv) None of the species are undergoing oxidation or reduction.
Identify the correct statements with reference to the given reaction.
\[\ce{P4 + 3OH- + 3H2O -> PH3 + 3H2PO^{-}2}\]
(i) Phosphorus is undergoing reduction only.
(ii) Phosphorus is undergoing oxidation only.
(iii) Phosphorus is undergoing oxidation as well as reduction.
(iv) Hydrogen is undergoing neither oxidation nor reduction.
Assertion (A): Redox couple is the combination of oxidised and reduced form of a substance involved in an oxidation or reduction half cell.
Reason (R): In the representation \[\ce{E^Θ_{Fe^{3+}/Fe^{2+}}}\] and \[\ce{E^Θ_{Cu^{2+}/Cu}, Fe^{3+}/Fe^{2+}}\] and \[\ce{Cu^{2+}/Cu}\] are redox couples.
Write redox couples involved in the reactions given.
\[\ce{Cu + Zn^{2+} ->Cu^{2+} + Zn}\]
Write redox couples involved in the reactions given.
\[\ce{Mg + Fe^{2+} -> Mg^{2+} + Fe}\]
Which of the following examples does not represent disproportionation?
Which of the following reactions is the metal displacement reaction? Choose the right option.
In an experiment O3 undergo decomposition as \[\ce{O3 -> O2 + O}\] by the radiations of wavelength 310 Å. The total energy falling on the O3 gas molecules is 2.4 × 1026 eV and quantum yield of the reaction is 0.2.
The volume strength of the H2O2 solution which is obtained from reaction of 1 l H2O and nascent oxygen [O] obtained from the above reactions is (Assuming no change in volume of H2O)
\[\ce{H2O + O -> H2O2}\]
[Given: Na (Avogadro's No.) = 6 × 1023]
