Displacement reaction: A more reactive element displaces a less reactive element from its compound. For example, zinc displaces copper from copper sulphate solution.

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7. Displacement reaction: A more reactive element displaces a less reactive element from its compound. For example, zinc displaces copper from copper sulphate solution. $Zn(s) + CuSO_4(aq) \rightarrow ZnSO_4(aq) + Cu(s)$ Double Displacement reaction: Two compounds react by an exchange of ions to form two new compounds. This often results in the formation of a precipitate, a gas, or water. For example, the reaction between sodium sulphate and barium chloride. $Na_2SO_4(aq) + BaCl_2(aq) \rightarrow BaSO_4(s) + 2NaCl(aq)$

8. When calcium carbonate ($\text{CaCO}_3$) is heated, it undergoes thermal decomposition to form calcium oxide ($\text{CaO}$) and carbon dioxide ($\text{CO}_2$) gas. $CaCO_3(s) \xrightarrow{heat} CaO(s) + CO_2(g)$ The presence of $\text{CO}_2$ gas can be confirmed by passing it through limewater (calcium hydroxide solution), which turns milky due to the formation of insoluble calcium carbonate.

9. When lead nitrate ($\text{Pb(NO}_3)_2$) is heated, it decomposes to produce lead(II) oxide ($\text{PbO}$), brown fumes of nitrogen dioxide ($\text{NO}_2$) gas, and oxygen ($\text{O}_2$) gas. $2Pb(NO_3)_2(s) \xrightarrow{heat} 2PbO(s) + 4NO_2(g) + O_2(g)$

10. • When ferrous sulphate ($\text{FeSO}_4$) crystals are heated, they lose water of crystallization and then decompose to form ferric oxide ($\text{Fe}_2O_3$), sulfur dioxide ($\text{SO}_2$), and sulfur trioxide ($\text{SO}_3$). The green color of the crystals changes to reddish-brown. $2FeSO_4(s) \xrightarrow{heat} Fe_2O_3(s) + SO_2(g) + SO_3(g)$ • When potassium chlorate ($\text{KClO}_3$) is heated, it decomposes to form potassium chloride ($\text{KCl}$) and oxygen gas ($\text{O}_2$). This reaction is faster in the presence of a catalyst like manganese dioxide ($\text{MnO}_2$). $2KClO_3(s) \xrightarrow{heat} 2KCl(s) + 3O_2(g)$

11. A combination reaction is a reaction in which two or more reactants combine to form a single product. Example: $\text{C(s)} + O_2(g) \rightarrow CO_2\text{(g)}$ A decomposition reaction is a reaction in which a single reactant breaks down into two or more simpler products. Example: $\text{CaCO}_3(s) \xrightarrow{heat} CaO(s) + CO_2\text{(g)}$ They are opposite because combination reactions involve substances joining to form one product, while decomposition reactions involve one substance breaking apart into multiple products.

12. When electricity is passed through water (electrolysis), water decomposes into hydrogen gas ($\text{H}_2$) and oxygen gas ($\text{O}_2$). $2H_2O(l) \xrightarrow{electricity} 2H_2(g) + O_2(g)$

13. When silver chloride ($\text{AgCl}$) and silver bromide ($\text{AgBr}$) are exposed to sunlight, they undergo photodecomposition. They break down to form silver metal and chlorine gas or bromine gas, respectively. This reaction is used in black and white photography. $2AgCl(s) \xrightarrow{sunlight} 2Ag(s) + Cl_2(g)$ $2AgBr(s) \xrightarrow{sunlight} 2Ag(s) + Br_2(g)$

14. a) The substance 'x' used for white washing is calcium oxide. Its formula is $\boxed{CaO}$. b) The reaction of substance 'x' (calcium oxide) with $\text{H}_2\text{O}$ is: $CaO(s) + H_2O(l) \rightarrow Ca(OH)_2(aq)$ This forms calcium hydroxide, also known as slaked lime, which is the solution used for whitewashing.

15. OR: During the electrolysis of water, hydrogen gas ($\text{H}_2$) is collected at the cathode, and oxygen gas ($\text{O}_2$) is collected at the anode. The chemical formula of water is $\text{H}_2\text{O}$, indicating that for every one molecule of oxygen, there are two molecules of hydrogen. Therefore, the volume of hydrogen gas collected is double the amount of oxygen gas.

16. a) $\text{Zn} + CuSO_4 \rightarrow ZnSO_4 + \text{Cu}$ This reaction occurs because zinc is more reactive than copper and displaces copper from copper sulphate solution. b) $\text{Cu} + ZnSO_4 \rightarrow \text{NO reaction}$ This reaction does not occur because copper is less reactive than zinc and cannot displace zinc from zinc sulphate solution.

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