Chemistry is concerned with different types of matter and the transformation of one type of matter into another. The various types of reactions result in the conversion of matter from one type to another. Redox Reactions are an important type of such reaction. Redox reactions are involved in a variety of physical and biological phenomena.
CBSE Class 11 Chemistry Chapter 8 Redox Reactions – Set 1
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Q-1: Which of the following statements about redox reactions is correct?
a) A nonmetal with a higher reduction potential is a more potent reducing agent.
b) A metal with a lower oxidation potential is a more potent oxidising agent.
c) The oxygen oxidation state in O3 is -1.
d) All of the above
Q-2: Which of the following can behave as a strong reducing agent?
a) HClO4
b) SnCl2
c) SO2
d) All of the above
Q-3: The pair of compounds in which both metals are in the highest oxidation state is
a) FeSO4, CuS2
b) CrO2Cl2, MnO4–
c) TiO2, MnO2
d) [Co(CN)6]3-, MnO3
Q-4: The number of electrons involved when 1 mole of H2O2 decomposes as
H2O2 → H2O + O2
a) 1
b) 6
c) 8
d) 4
Q-5: Zinc iodide is formed during the reaction of zinc and iodine. Which of these is being oxidised?
a) Zinc ions
b) Zinc atom
c) Iodide ions
d) Iodine
Q-6: Can a solution of 1M copper sulphate be stored in a vessel made of nickel metal?
Given that Eo(Ni2+/Ni) = -0.25 volt and Eo(Cu2+/Cu) = +0.34 volt.
Q-7: Using the electronic concept, identify the oxidant and reductant in the following redox reactions.
i) Zn + 2H+ → Zn2+ + H2
ii) BrO3– + F2 + 2OH– → BrO4– + 2F– + H2O
Q-8: How does the oxidation number of carbon change when ethane is burned in excess of oxygen?
Q-9: Iron produces H2 gas when it reacts with dilute H2SO4, but Ag does not. Why?
Q-10:
a) Write a fluorine-alkali reaction.
b) Why does fluorine behave differently with alkali than other halogens?
Q-11: Define the term “oxidation number.” Write down the general rules for allocating oxidation numbers to different atoms in ions and molecules.
Q-12: Which of the two, ClO2– or ClO4–, exhibits the disproportionation reaction, and why?
Q-13: Balance the redox reaction by half-reaction method.
Br2 + H2O2 → BrO3– + H2O (in acidic medium)
Q-14: Balance the reaction below using the oxidation number method.
Mg + HNO3 → Mg(NO3)2 + N2O + H2O
Q-15: Using Stock notation, represent the following compounds: Hg2Cl2, FeCl3, Fe2O3, MnO2, SnO2, Cu2S and Cu2O.
Q-16: Classify the following redox reactions.
i) N2 + O2 → 2NO
ii) NaH + H2O → NaOH + H2
iii) 2Pb(NO3)2 → 2PbO + 2NO2 + ½ O2
iv) V2O5 + 5Ca → 2V + 5CaO
v) P4 + 3OH– + 3H2O → PH3 + 3H2PO2–
Q-17: Arrange the following reactions in the increasing order of their rate of evolution of hydrogen gas.
i) Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g)
ii) Mg(s) + 2HCl (aq) → MgCl2(aq) + H2(g)
iii) Fe(s) + 2HCl(aq) → FeCl2(aq) + H2(g)
Q-18: For each of the following redox reactions, write half reactions.
i) Zn(s) + PbCl2(aq) →Pb(s) + ZnCl2(aq)
ii) 2Fe3+(aq) + 2I–(aq) → I2(aq) + 2Fe2+(aq)
Q-19: How many grams of K2Cr2O7 is required to oxidise 17.2 g of FeSO4 in an acidic medium?
Q-20: The half cell reactions with reduction potentials are
Pb(s) → Pb2+ (aq) ; Eored = -0.13 V
Ag(s) → Ag+ (aq) ; Eored = 0.80 V
Calculate its emf.
Download the PDF to access answers to the Chemistry Worksheet for Class 11 Chemistry Chapter 8 Redox Reactions Set -1
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