Calculate the amount, in mol, of $\text{S}_2\text{O}_3^{2-}$ that is used up in the titration.
Use the result from (a)(i) to determine the amount, in mol, of $\text{I}_2$ in $1.00\,\text{dm}^3$ of solution A.
In experiment 2, $0.100\,\text{mol}$ of $\text{H}_2(g)$, $0.200\,\text{mol}$ of $\text{I}_2(g)$ and $0.300\,\text{mol}$ of $\text{HI}(g)$ are mixed. At equilibrium, $0.154\,\text{mol}$ of $\text{I}_2$ remains. Calculate the amounts, in mol, of $\text{H}_2$ and $\text{HI}$ in the equilibrium mixture formed in experiment 2.
In experiment 3, $0.0772\,\text{mol}$ of $\text{H}_2$ and $0.0986\,\text{mol}$ of $\text{I}_2$ are present in an equilibrium mixture at $298\,\text{K}$. Given $K_c = 7.94 \times 10^2$ for the reaction $\text{H}_2(g) + \text{I}_2(g) \rightleftharpoons 2\text{HI}(g)$, calculate the amount, in mol, of $\text{HI}$ present in the equilibrium mixture in experiment 3.
Define a covalent bond.
Describe and explain the relative thermal stabilities of hydrogen halides $\text{HCl}$ and $\text{HI}$.
Use the data from (c) and (d) to suggest a value for the equilibrium constant for the dissociation of $\text{HBr}(g)$ at $298\,\text{K}$.