Explain what the term bond polarity means.
Suggest why the boiling point of HF is much higher than those of the other hydrogen halides.
Describe and explain the relative thermal stabilities of the hydrogen halides.
The equation for making hydrogen chloride using concentrated sulfuric acid is shown: $\text{H}_2\text{SO}_4 + \text{NaCl} \rightarrow \text{NaHSO}_4 + \text{HCl}$. Use the Brønsted-Lowry theory of acids and bases to identify the base and its conjugate acid in this reaction. Explain your answer.
Explain why the reaction of concentrated sulfuric acid and sodium iodide is not suitable for preparing hydrogen iodide.
Hydrogen chloride reacts reversibly with oxygen:\n\n$4\text{HCl(g)} + \text{O}_2\text{(g)} \rightleftharpoons 2\text{Cl}_2\text{(g)} + 2\text{H}_2\text{O(g)}$\n\nThe reaction is carried out at $400\,^\circ\text{C}$ in the presence of a copper(II) chloride catalyst.\n\nUse the data in the table to calculate the overall enthalpy change of reaction.\n\n$\Delta H_f^\circ(\text{HCl(g)}) = -92\,\text{kJ mol}^{-1}$\n\n$\Delta H_f^\circ(\text{H}_2\text{O(g)}) = -242\,\text{kJ mol}^{-1}$
State the type of catalyst used in this reaction. Explain how a catalyst can increase the rate of a chemical reaction.
The reaction exists in dynamic equilibrium. The reaction was repeated at $1000\,^\circ\text{C}$ and the same pressure.\n\nState and explain the effect on the composition of the equilibrium mixture of the change in temperature.
When $1.60\,\text{mol}$ of HCl are mixed in a sealed container with $0.500\,\text{mol}$ of $\text{O}_2$ at $400\,^\circ\text{C}$, $0.600\,\text{mol}$ of $\text{Cl}_2$ and $0.600\,\text{mol}$ of $\text{H}_2\text{O}$ are formed. The total pressure inside the container is $1.50 \times 10^5\,\text{Pa}$.\n\nCalculate the amounts, in mol, of HCl and $\text{O}_2$ in the equilibrium mixture.
Calculate the mole fraction of $\text{Cl}_2$ and then the partial pressure of $\text{Cl}_2$ in the equilibrium mixture.
In a separate experiment, an equilibrium reaction mixture was found to contain the four gases at the partial pressures listed below:\n\n$\text{HCl}: 4.8 \times 10^4\,\text{Pa}$, $\text{O}_2: 3.0 \times 10^4\,\text{Pa}$, $\text{Cl}_2: 3.6 \times 10^4\,\text{Pa}$, $\text{H}_2\text{O}: 3.6 \times 10^4\,\text{Pa}$.\n\n$K_p = \dfrac{(p_{\text{Cl}_2})^2 (p_{\text{H}_2\text{O}})^2}{(p_{\text{HCl}})^4 p_{\text{O}_2}}$\n\nUse this information together with the expression given for $K_p$ to calculate a value for $K_p$. State the units of $K_p$.
The reaction is repeated without a catalyst. State the effect of this on $K_p$.
Use this information together with the expression given for $K_p$ to calculate a value for $K_p$. State the units of $K_p$.\nThe expression for $K_p$ is $K_p = \dfrac{(p_{\text{Cl}_2})^2 \times (p_{\text{H}_2\text{O}})^2}{(p_{\text{HCl}})^4 \times p_{\text{O}_2}}$.
The reaction is repeated without a catalyst. State the effect of this on $K_p$.