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CBSE - Class 11 > Chemistry > Redox Reactions Worksheets

Free CBSE - Class 11 Chemistry - Redox Reactions worksheets

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1.
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
2.
Depict the galvanic cell in which the reaction $Zn(s) + 2Ag^+(aq) \rightarrow Zn^{2+}(aq) + 2Ag(s)$ takes place, Further show: (iii) individual reaction at each electrode.
3.
Arrange the following metals in the order in which they displace each other from the solution of their salts. $Al$, $Cu$, $Fe$, $Mg$ and $Zn$.
4.
Given the standard electrode potentials, $K^+/K = -2.93V$, $Ag^+/Ag = 0.80V$, $Hg^{2+}/Hg = 0.79V$ $Mg^{2+}/Mg = -2.37V$. $Cr^{3+}/Cr = -0.74V$ arrange these metals in their increasing order of reducing power.
5.
Depict the galvanic cell in which the reaction $Zn(s) + 2Ag^+(aq) \rightarrow Zn^{2+}(aq) + 2Ag(s)$ takes place, Further show: (i) which of the electrode is negatively charged,
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.
Using the standard electrode potentials given in the Table 8.1, predict if the reaction between the following is feasible: (e) $Br_2(aq)$ and $Fe^{2+}(aq)$.
9.
Predict the products of electrolysis in each of the following: (i) An aqueous solution of $AgNO_3$ with silver electrodes
10.
Predict the products of electrolysis in each of the following: (ii) An aqueous solution $AgNO_3$ with platinum electrodes
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Chapters in CBSE - Class 11 Chemistry

Chemical Bonding and Molecular Structure Worksheet Classification of Elements and Periodicity in Properties Worksheet Equilibrium Worksheet Hydrocarbons Worksheet Organic Chemistry – Some Basic Principles and Techniques Worksheet Some Basic Concepts of Chemistry Worksheet Structure of Atom Worksheet Thermodynamics Worksheet

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The Exchange Game of Electrons and Reactions

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