Advertisements
Advertisements
Question
Which of the following is not an example of redox reaction?
Options
\[\ce{CuO + H2 -> Cu + H2O}\]
\[\ce{Fe2O3 + 3CO -> 2Fe + 3CO2}\]
\[\ce{2K + F2 -> 2KF}\]
\[\ce{BaCl2 + H2SO4 -> BaSO4 + 2HCl}\]
Advertisements
Solution
\[\ce{BaCl2 + H2SO4 -> BaSO4 + 2HCl}\]
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
RELATED QUESTIONS
Justify that the following reaction is redox reaction:
\[\ce{2K(s) + F2(g) → 2K+F– (s)}\]
Fluorine reacts with ice and results in the change: \[\ce{H2O(s) + F2(g) → HF(g) + HOF(g)}\]
Justify that this reaction is a redox reaction.
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:
\[\ce{2AgBr (s) + C6H6O2(aq) → 2Ag(s) + 2HBr (aq) + C6H4O2(aq)}\]
Identify the substance oxidised, reduced, oxidising agent and reducing agent for the following reaction:
\[\ce{Pb(s) + PbO2(s) + 2H2SO4(aq) → 2PbSO4(s) + 2H2O(l)}\]
Consider the reactions:
- \[\ce{H3PO2(aq) + 4 AgNO3(aq) + 2 H2O(l) → H3PO4(aq) + 4Ag(s) + 4HNO3(aq)}\]
- \[\ce{H3PO2(aq) + 2CuSO4(aq) + 2 H2O(l) → H3PO4(aq) + 2Cu(s) + H2SO4(aq)}\]
- \[\ce{C6H5CHO(l) + 2[Ag (NH3)2]+(aq) + 3OH–(aq) → C6H5COO–(aq) + 2Ag(s) + 4NH3 (aq) + 2 H2O(l)}\]
- \[\ce{C6H5CHO(l) + 2Cu^{2+}(aq) + 5OH–(aq) → No change observed}\]
What inference do you draw about the behaviour of Ag+ and Cu2+ from these reactions?
Identify disproportionation reaction
Assertion (A): The decomposition of hydrogen peroxide to form water and oxygen is an example of disproportionation reaction.
Reason (R): The oxygen of peroxide is in –1 oxidation state and it is converted to zero oxidation state in \[\ce{O2}\] and –2 oxidation state in \[\ce{H2O}\].
Write redox couples involved in the reactions given.
\[\ce{Mg + Fe^{2+} -> Mg^{2+} + Fe}\]
Write redox couples involved in the reactions given.
\[\ce{Br2 + 2Cl- -> Cl2 + 2Br-}\]
Write redox couples involved in the reactions given.
\[\ce{Fe + Cd^{2+} -> Cd + Fe^{2+}}\]
Which of the following examples does not represent disproportionation?
Which of the following reactions is the metal displacement reaction? Choose the right option.
The reaction of sulphur in alkaline medium is given below:
\[\ce{S8(s) + {a} OH^-(aq) -> {b} S^{2-}(aq) + {c} S2O^{2-}3(aq) + {d} H2O(l)}\]
The values of 'a' are ______. (Integer answer)
The species given below that does NOT show a disproportionation reaction is ______.
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]
