CBSE - Class 11 Chemistry Redox Reactions Worksheet
1.
Consider the elements : $Cs$, $Ne$, $I$ and $F$. (d) Identify the element which exhibits neither the negative nor does the positive oxidation state.
2.
Using the standard electrode potentials given in the Table 8.1, predict if the reaction between the following is feasible: (b) $Ag^+(aq)$ and $Cu(s)$
3.
Consider the reactions: (a) $H_3PO_2(aq) + 4AgNO_3(aq) + 2H_2O(l) \rightarrow H_3PO_4(aq) + 4Ag(s) + 4HNO_3(aq)$ (b) $H_3PO_2(aq) + 2CuSO_4(aq) + 2H_2O(l) \rightarrow H_3PO_4(aq) + 2Cu(s) + H_2SO_4(aq)$ (c) $C_6H_5CHO(l) + 2[Ag(NH_3)_2]^+(aq) + 3OH^-(aq) \rightarrow C_6H_5COO^-(aq) + 2Ag(s) + 4NH_3(aq) + 2H_2O(l)$ (d) $C_6H_5CHO(l) + 2Cu^{2+}(aq) + 5OH^-(aq) \rightarrow$ No change observed. What inference do you draw about the behaviour of $Ag^+$ and $Cu^{2+}$ from these reactions ?
4.
Write formulas for the following compounds: (a) Mercury(II) chloride
5.
Assign oxidation number to the underlined elements in each of the following species: (b) $NaHSO_4$
6.
Predict the products of electrolysis in each of the following: (iii) A dilute solution of $H_2SO_4$ with platinum electrodes
7.
Predict the products of electrolysis in each of the following: (iv) An aqueous solution of $CuCl_2$ with platinum electrodes.
8.
Assign oxidation number to the underlined elements in each of the following species: (d) $K_2MnO_4$
9.
Consider the reactions : $2S_2O_3^{2-}(aq) + I_2(s) \rightarrow S_4O_6^{2-}(aq) + 2I^-(aq)$ $S_2O_3^{2-}(aq) + 2Br_2(l) + 5H_2O(l) \rightarrow 2SO_4^{2-}(aq) + 4Br^-(aq) + 10H^+(aq)$. Why does the same reductant, thiosulphate react differently with iodine and bromine ?
10.
Justify that the following reactions are redox reactions: (a) $CuO(s) + H_2(g) \rightarrow Cu(s) + H_2O(g)$
11.
Assign oxidation number to the underlined elements in each of the following species: (c) $H_4P_2O_7$
12.
Justify that the following reactions are redox reactions: (b) $Fe_2O_3(s) + 3CO(g) \rightarrow 2Fe(s) + 3CO_2(g)$
13.
Identify the substance oxidised reduced, oxidising agent and reducing agent for each of the following reactions: (e) $Pb(s) + PbO_2(s) + 2H_2SO_4(aq) \rightarrow 2PbSO_4(s) + 2H_2O(l)$
14.
What sorts of informations can you draw from the following reaction ? $(CN)_2(g) + 2OH^-(aq) \rightarrow CN^-(aq) + CNO^-(aq) + H_2O(l)$
15.
Predict the products of electrolysis in each of the following: (ii) An aqueous solution $AgNO_3$ with platinum electrodes
16.
Chlorine is used to purify drinking water. Excess of chlorine is harmful. The excess of chlorine is removed by treating with sulphur dioxide. Present a balanced equation for this redox change taking place in water.
17.
Depict the galvanic cell in which the reaction $Zn(s) + 2Ag^+(aq) \rightarrow Zn^{2+}(aq) + 2Ag(s)$ takes place, Further show: (ii) the carriers of the current in the cell, and
18.
Justify that the following reactions are redox reactions: (c) $4BCl_3(g) + 3LiAlH_4(s) \rightarrow 2B_2H_6(g) + 3LiCl(s) + 3AlCl_3(s)$
19.
Balance the following redox reactions by ion – electron method : (c) $H_2O_2(aq) + Fe^{2+}(aq) \rightarrow Fe^{3+}(aq) + H_2O(l)$ (in acidic solution)
20.
Refer to the periodic table given in your book and now answer the following questions: (a) Select the possible non metals that can show disproportionation reaction.
