2. Using the smallest whole number coefficients, balance the following reactions. Draw diagrams like those in Figure 4 for Equations a, b, and f. а, а. HgO → _ Hg + O2 b. Fe + O2 → _ Fe2O3 с. KC103 → КСІ + O2 d. Ca(OH)2 +_ H2SO4 → НОН + CaSO4 Cu + AGNO3 →_ Cu(NO3)2 + Ag е. f. - C2H6 +_O2 →_ CO2 +_H20

4. Balance the reactions in the following. H₂ + N₂ → NH3 CaCl2 + AgNO3 → Ca (NO3)2 + AgCl SnO₂ + H₂ →→→ H₂O + Sn Na2CO3 + HCl → NaCl + H₂O + CO2 Fe2(SO4)3 + KOH → K2SO4 + Fe (OH)3 C₂H6O2 + O2 CO2 + H2O Fe(OH)2 → Fe3O4+H₂ + H₂O Balanced equation lu comes from carbohydrates, which are broken down into

Classify the following reactions: a. CH4 + 2 O2 ⟶ CO2 + 2 H2Oi. Combustionii. Double replacementiii. Single replacementiv. Synthesis/combinationv. Decomposition b. N2 + 3 Cl2 ⟶ 2 NCl3i. Combustionii. Double replacementiii. Single replacementiv. Synthesis/combinationv. Decomposition c. 2 Al + 3 CuSO4 ⟶ Al2(SO4)3 + 3 Cui. Combustionii. Double replacementiii. Single replacementiv. Synthesis/combinationv. Decomposition

Complete the following table, making sure to include your units! Concentration of Concentration of acetic acid Water level on measuring cylinder before reaction 98 mL 91 mL 95 mL 0.5% 0.2% 0.1% ● sodium bicarbonate 0.5 M 0.5 M 0.5 M From the results above, which reactant do you consider to be the limiting reagent? Why? ● Water level on measuring cylinder after reaction 8 mL 49 mL 81 mL Consider the reaction where the concentration of acetic acid was 0.5% and the concentration of sodium bicarbonate was 0.5 M. Complete the table on page 5 to calculate the theoretical yield of CO2 with these concentrations. The following bullet points may help: You have already calculated the amount of sodium bicarbonate in 100 mL In a 100 mL solution of acetic acid at 0.1% there will be 0.1 mL of acetic acid. ● Volume of gas produced The density of acetic acid is 1.05 g/mL. You can use this value to calculate the mass of acetic acid used in the reaction.