State one natural source and one man-made source of oxides of nitrogen.
At high pressure and in the presence of a catalyst, nitrogen monoxide, $\text{NO}$, is converted into the two other oxides of nitrogen, dinitrogen monoxide, $\text{N}_2\text{O}$, and dinitrogen trioxide, $\text{N}_2\text{O}_3$. $\ldots\, \text{NO(g)} \rightarrow \ldots\, \text{N}_2\text{O(g)} + \ldots\, \text{N}_2\text{O}_3\text{(g)}$ $\Delta H^{\circ} = -195.2\,\text{kJ mol}^{-1}$ $\Delta G^{\circ} = -102.8\,\text{kJ mol}^{-1}$
Balance the equation above for the production of $\text{N}_2\text{O}$ and $\text{N}_2\text{O}_3$ from $\text{NO}$.
State how the oxidation number of nitrogen changes during this reaction. $\text{NO} \rightarrow \text{N}_2\text{O}$ from ................. to ................. $\text{NO} \rightarrow \text{N}_2\text{O}_3$ from ................. to .................
Calculate the entropy change for the reaction at $298\,\text{K}$. Include the units in your answer. $\Delta S^{\circ} = \ldots\ldots\ldots\ldots\ldots$ units = .................
State whether the sign of $\Delta S^{\circ}$ calculated in (iii) agrees with the sign predicted from your balanced equation in (i). Explain your answer.
At room temperature, $\text{N}_2\text{O}_3$ dissociates into a mixture. $\text{N}_2\text{O}_3\text{(g)} \rightleftharpoons \text{NO(g)} + \text{NO}_2\text{(g)}$
Write the expression for $K_p$ for this equilibrium. Include the units in your answer. $K_p = \ldots\ldots\ldots$ units = .................
A $1.00\,\text{dm}^3$ flask at $25^{\circ}\text{C}$ is charged with pure $\text{N}_2\text{O}_3\text{(g)}$ at an initial pressure of $0.60\,\text{atm}$. At equilibrium, the partial pressure of $\text{NO}_2\text{(g)}$ is $0.48\,\text{atm}$. Calculate the partial pressures of $\text{NO(g)}$ and $\text{N}_2\text{O}_3\text{(g)}$ at equilibrium. Hence calculate the value of $K_p$ at $25^{\circ}\text{C}$. $p(\text{NO(g)}) = .................$ $p(\text{N}_2\text{O}_3\text{(g)}) = .................$ $K_p = .................$
$\text{NO}$ reacts readily with oxygen. $2\text{NO(g)} + \text{O}_2\text{(g)} \rightarrow 2\text{NO}_2\text{(g)}$ The table shows how the initial rate of this reaction at $25^{\circ}\text{C}$ depends on the initial concentrations of the reactants.
Deduce the order of reaction with respect to each reactant. Explain your reasoning. order with respect to $[\text{NO(g)}]$ ................. order with respect to $[\text{O}_2\text{(g)}]$ .................
State the rate equation for this reaction. Use the rate equation to calculate the rate constant. Include the units for the rate constant in your answer. rate = ................. rate constant, $k = .................$ units of $k = .................
State what is meant by the term coordination number.
Describe how the coordination number of the iron changes during this reaction, from \_ to \_.
Only one stereoisomer of $\text{Fe(CO)}_2\text{(NO)}_2$ exists. Use this information to suggest the geometry of the complex.
The complex $\text{Ru(NO)L}_2\text{Cl}_3$ occurs in three isomeric forms. L represents the monodentate ligand $\text{C}_6\text{H}_5\text{P(CH}_3)_2$. Complete the three-dimensional diagrams to show the three isomers of $\text{Ru(NO)L}_2\text{Cl}_3$.
Suggest the type of isomerism shown.