Potassium chlorate, KClO3, is widely used as an oxidising agent and to make O2(g).

1. (a)Define oxidising agent.[1]
2. (b)KClO3(s) decomposes when heated. MnO2(s) catalyses the exothermic decomposition reaction. Complete and label the diagram in Fig. 3.1 to show the effect of MnO2(s) on the decomposition of KClO3(s). [Figure 3.1][2]
3. (c)When KClO3 is heated without a catalyst, KClO4 and KCl form. 4KClO3 → 3KClO4 + KCl Explain why this reaction is described as a disproportionation reaction.[1]
4. (d)(i)Molten KClO3 reacts with glucose, C6H12O6. 4KClO3 + C6H12O6 → 6CO2 + 6H2O + 4KCl KClO3 melts at 630 K. At this temperature, both CO2 and H2O are gases. Use the ideal gas equation to calculate the volume, in m³, of one mole of gas at 630K and 1.00 x 105 Pa. Show your working. Give your answer to 3 significant figures.[1]
5. (d)(ii)5.00 g of C6H12O6 reacts completely with molten KClO3. Use your answer to (d)(i) to calculate the total volume of gas released at 630K and 1.00 x 105 Pa in this reaction. (If you were unable to answer (d)(i), use 0.0463m³ in this question. This is not the correct answer to (d)(i).)[2]
6. (e)(i)The structure of glucose, C6H12O6, is shown in Fig. 3.2. Complete Table 3.1 to identify the number of primary, secondary and tertiary alcohol groups present in the structure shown in Fig. 3.2. [Figure 3.2] [Table 3.1][1]
7. (e)(ii)Separate samples of aqueous glucose are tested with the reagents shown in Table 3.2. Complete Table 3.2 with the observation for each reaction. Write "no reaction" if applicable. [Table 3.2][3]
8. (e)(iii)There are many structural isomers of C6H12O6. Define structural isomers.[1]