Use Fig. 4.1 to determine the average rate of change of concentration of $\text{HCl(aq)}$ in this reaction between $0$-$100$ seconds and between $400$-$500$ seconds. Include units in your answers.
Use Fig. 4.1 to identify the limiting reagent. Justify your answer.
Explain why the rate of reaction changes with time.
The reaction between $\text{Na}_2\text{S}_2\text{O}_3\text{(aq)}$ and $\text{HCl(aq)}$ is repeated in a second experiment. In this second experiment, $25.0\,\text{cm}^3$ of $0.050\,\text{mol dm}^{-3}\,\text{Na}_2\text{S}_2\text{O}_3\text{(aq)}$ reacts with $0.0020\,\text{mol}$ of $\text{HCl(aq)}$. Calculate the number of sulfur atoms produced.
Explain why the rate of reaction cannot be monitored accurately by measuring the volume of $\text{SO}_2\text{(g)}$ produced in this reaction.
Fig. 4.2 shows one possible arrangement of outer-shell electrons in a single $\text{SO}_2$ molecule. Use Fig. 4.2 to predict the shape and bond angle of a molecule of $\text{SO}_2$.
Use Table 4.1 to predict the strength of the dipole moment of $\text{SO}_2$, if any, compared with that of $\text{H}_2\text{O}$. Explain your answer.
The reaction between $\text{Na}_2\text{S}_2\text{O}_3(aq)$ and $\text{HCl}(aq)$ is repeated in a second experiment. In this second experiment, $25.0\text{ cm}^3$ of $0.050\text{ mol dm}^{-3}$ $\text{Na}_2\text{S}_2\text{O}_3(aq)$ reacts with $0.0020\text{ mol}$ of $\text{HCl}(aq)$. Calculate the number of sulfur atoms produced.
Explain why the rate of reaction cannot be monitored accurately by measuring the volume of $\text{SO}_2(g)$ produced in this reaction.