1. $N_2(g)$ $+$ $3H_2(g)$ $\rightarrow$ $2NH_3(g)$
2. $2H_2S(g)$ $+$ $3O_2(g)$ $\rightarrow$ $2H_2O(l)$ $+$
$2SO_2(g)$
3. $3BaCl_2(aq)$ $+$ $Al_2(SO_4)_3(aq)$ $\rightarrow$
$2AlCl_3(aq)$
$+$ $3BaSO_4(s)$
4. $2K(s)$ $+$ $2H_2O(l)$ $\rightarrow$ $2KOH(aq)$ $+$
$H_2(g)$ $+$ $Heat$
5. $Ca(OH)_2(aq)$ $+$ $CO_2(g)$ $\rightarrow$ $CaCO_3(s)$
$+$
$H_2O(l)$
6. $ZnCO_3(s)$ $\rightarrow$ $ZnO(s)$ $+$ $CO_2(g)$
7. $Mg(s)$ $+$ $2HCl(aq)$ $\rightarrow$ $MgCl_2(aq)$ $+$
$H_2(g)$
8. $Na_2SO_3(s)$ $+$ $2HCl(aq)$ $\rightarrow$ $2NaCl(aq)$
$+$ $H_2O(l)$
$+$ $SO_2(g)$
9. $2HNO_3$ $+$ $Ca(OH)_2$ $\rightarrow$ $Ca(NO_3)_2$ $+$
$2H_2O$
10. $2NaOH$ $+$ $H_2SO_4$ $\rightarrow$ $Na_2SO_4$ $+$
$2H_2O$
11. $NaCl$ $+$ $AgNO_3$ $\rightarrow$ $AgCl$ $+$ $NaNO_3$
(Already
balanced)
12. $BaCl_2$ $+$ $H_2SO_4$ $\rightarrow$ $BaSO_4$ $+$
$2HCl$
13. $2FeSO_4$ $\xrightarrow{\Delta}$ $Fe_2O_3$ $+$ $SO_2$
$+$ $SO_3$
14. $2Pb(NO_3)_2$ $\xrightarrow{\Delta}$ $2PbO$ $+$
$4NO_2$ $+$ $O_2$
15. $MnO_2$ $+$ $4HCl$ $\rightarrow$ $MnCl_2$ $+$ $2H_2O$
$+$ $Cl_2$
16. $C_6H_{12}O_6$ $+$ $6O_2$ $\rightarrow$ $6CO_2$ $+$
$6H_2O$ $+$
$Energy$
17. Combination Reaction: Reaction where
two or more reactants combine to form a single product. Ex: $CaO$ $+$ $H_2O$ $\rightarrow$ $Ca(OH)_2$ $+$
$Heat$.
18. Decomposition Reaction: Single
reactant breaks down into simpler products. It is opposite of combination. Ex: $CaCO_3$
$\xrightarrow{\Delta}$
$CaO$ $+$ $CO_2$.
19. Displacement Reaction: More reactive
element displaces less reactive element from its salt solution. $Fe$ $+$ $CuSO_4$ $\rightarrow$ $FeSO_4$ $+$
$Cu$. Iron
displaces Copper.
20. Double Displacement: Exchange of ions
between reactants. Precipitate: Insoluble solid formed during reaction.
21. Combination Reaction (Formation of Water).
22. Thermal Decomposition.
23. Displacement Reaction.
24. Double Displacement (Precipitation) Reaction.
25. Decomposition carried out by heating. $2Pb(NO_3)_2$
$\xrightarrow{\Delta}$ $2PbO$ $+$ $4NO_2$ $+$ $O_2$.
26. Decomposition by light energy. Used in Black & White
photography. $2AgCl$ $\xrightarrow{Sunlight}$ $2Ag$ $+$ $Cl_2$.
27. Decomposition by electricity. Electrolysis of water:
$2H_2O$ $\rightarrow$ $2H_2$ $+$ $O_2$.
28. Because energy is released during the process of
breaking down glucose.
29. Because heat is evolved due to microbial action
(Exothermic).
30. Exothermic: Heat released
(Respiration, Burning). Endothermic: Heat absorbed (Photosynthesis, Decomposition of
CaCO3).
31. Oxidation: Gain of Oxygen.
Reduction: Loss of Oxygen.
32. Oxidation: Loss of Hydrogen.
Reduction: Gain of Hydrogen.
33. Sodium (Na) is oxidized to $Na_2O$.
34. Oxidizing Agent: $CuO$ (gives oxygen).
35. Reducing Agent: $C$ (takes oxygen).
36. Reduced Substance: $MnO_2$ (loses oxygen to become
$MnCl_2$).
37. Oxidizing Agent: $Cl_2$ (removes hydrogen from H2S).
38. Reducing Agent: $C$ (Carbon).
39. Substance Oxidized: $Al$ (Aluminium).
40. Reaction where oxidation and reduction occur
simultaneously. Ex: $CuO + H_2 \rightarrow Cu + H_2O$.
41. No. Redox reactions always involve simultaneous
oxidation and reduction (electron transfer).
42. Combination / Oxidation / Redox. Mg is oxidized, O2 is
reduced.
43. Slow eating away of metal by atmospheric
gases/moisture. Rust: $Fe_2O_3 \cdot xH_2O$.
44. To preventing contact of iron surface with air and
moisture.
45. Oiling/Greasing, Galvanisation.
46. Coating iron with Zinc. Zinc is used.
47. Oxidation of fats/oils causing bad smell/taste. Chips,
fried foods.
48. Adding Antioxidants, Flushing with Nitrogen, Airtight
containers.
49. Nitrogen is an inert gas, prevents contact with
Oxygen.
50. Yes. Copper: Green ($CuCO_3 \cdot Cu(OH)_2$). Silver:
Black ($Ag_2S$).
51. Cleaned to remove oxide layer. Flame: Dazzling White.
Ash: White Powder (MgO).
52. Yellow Precipitate. Lead Iodide ($PbI_2$).
53. Hydrogen ($H_2$). Burns with a 'pop' sound.
54. Hot. Exothermic reaction (Slaking of lime).
55. Anode: Oxygen ($O_2$). Cathode: Hydrogen ($H_2$).
Ratio $H_2:O_2 = 2:1$.
56. Green crystals turn white (anhydrous), then brown
($Fe_2O_3$). Smell of burning sulphur ($SO_2, SO_3$).
57. Blue fades to Light Green ($FeSO_4$ formed).
Reddish-brown copper deposits on nail.
58. White Precipitate ($BaSO_4$). Double Displacement /
Precipitation.
59. Brown powder turns Black ($CuO$). $2Cu + O_2
\xrightarrow{\Delta} 2CuO$.
60. White turns Grey (Silver metal formed). $2AgCl
\xrightarrow{Sunlight} 2Ag + Cl_2$.
