Explain what is understood by dynamic equilibrium.
Describe one difference between the reaction mixture at the start and the mixture once equilibrium has been reached.
Write an expression for $K_p$ for the reaction in equation 1.
At equilibrium, the partial pressure of $\text{HI(g)}$ equals $86.4\,\text{kPa}$. Calculate how many moles of $\text{HI(g)}$ are present in the equilibrium mixture. Show your working.
Use equation 1 and the bond energy values in Table 3.1 to calculate the enthalpy change, $\Delta H$, for the thermal decomposition of $1$ mole of $\text{HI(g)}$. Show your working.
Describe how increasing pressure affects the value of $K_p$ for the decomposition of $\text{HI(g)}$.
Identify the kind of reaction that takes place when $\text{NaI(s)}$ reacts with concentrated $\text{H}_2\text{SO}_4$ to form $\text{HI(g)}$.
Write an equation for how $\text{HI(g)}$ reacts with concentrated $\text{H}_2\text{SO}_4$.
Explain why $\text{HI(g)}$ reacts with concentrated $\text{H}_2\text{SO}_4$ but $\text{HCl}$ does not.