Define the term oxidising agent.
$\text{KClO}_3$(s) decomposes on heating. $\text{MnO}_2$(s) catalyses the exothermic decomposition reaction. Complete and label the diagram in Fig. 3.1 to show how $\text{MnO}_2$(s) affects the decomposition of $\text{KClO}_3$(s).
If $\text{KClO}_3$ is heated without a catalyst, $\text{KClO}_4$ and $\text{KCl}$ are produced. $4\text{KClO}_3 \rightarrow 3\text{KClO}_4 + \text{KCl}$. Explain why this reaction is called a disproportionation reaction.
Molten $\text{KClO}_3$ reacts with glucose, $\text{C}_6\text{H}_{12}\text{O}_6$. $4\text{KClO}_3 + \text{C}_6\text{H}_{12}\text{O}_6 \rightarrow 6\text{CO}_2 + 6\text{H}_2\text{O} + 4\text{KCl}$. $\text{KClO}_3$ melts at $630\,\text{K}$. At this temperature, both $\text{CO}_2$ and $\text{H}_2\text{O}$ are gases. Use the ideal gas equation to calculate the volume, in $\text{m}^3$, of one mole of gas at $630\,\text{K}$ and $1.00 \times 10^5\,\text{Pa}$. Show your working. Give your answer to 3 significant figures.
$5.00\,\text{g}$ of $\text{C}_6\text{H}_{12}\text{O}_6$ reacts fully with molten $\text{KClO}_3$. Use your answer to (d)(i) to calculate the total volume of gas produced at $630\,\text{K}$ and $1.00 \times 10^5\,\text{Pa}$ in this reaction.
Fig. 3.2 shows the structure of glucose, $\text{C}_6\text{H}_{12}\text{O}_6$. Complete Table 3.1 by identifying how many primary, secondary and tertiary alcohol groups are present in the structure shown in Fig. 3.2.
Different samples of aqueous glucose are tested with the reagents listed in Table 3.2. Complete Table 3.2 by giving the observation for each reaction. Write "no reaction" where relevant.
Many structural isomers exist for $\text{C}_6\text{H}_{12}\text{O}_6$. Define structural isomers.