This question is about oxides of nitrogen.
An investigation is carried out on the equilibrium system shown below:
2NO2(g)⇌N2O4(g)ΔH=−57.2 kJ mol−1 2\text{NO}_2(\text{g}) \rightleftharpoons \text{N}_2\text{O}_4(\text{g}) \quad \Delta H = -57.2\text{ kJ mol}^{-1} 2NO2(g)⇌N2O4(g)ΔH=−57.2 kJ mol−1A sealed flask containing 6.00 moles6.00\text{ moles}6.00 moles of NO2(g)\text{NO}_2(\text{g})NO2(g) is heated to a constant temperature and allowed to reach equilibrium.
The equilibrium mixture contains 4.50 mol of NO2(g)\text{NO}_2(\text{g})NO2(g), and the total pressure is 3.00 atm3.00\text{ atm}3.00 atm.
Determine the value of KpK_{\text{p}}Kp and give your answer to 3 significant figures.
Include an expression for KpK_{\text{p}}Kp and the units of KpK_{\text{p}}Kp in your answer.
Kp=…………………units………………… K_{\text{p}} = \dots\dots\dots\dots\dots\dots\dots \quad \text{units} \dots\dots\dots\dots\dots\dots\dots Kp=…………………units…………………The sealed flask in (a)(i) is then heated to a higher temperature at an increased pressure. The system is allowed to reach equilibrium again.
Explain why it is difficult to predict how these changes in reaction conditions affect the amount of N2O4(g)\text{N}_2\text{O}_4(\text{g})N2O4(g) formed at equilibrium.
Nitrogen dioxide, NO2\text{NO}_2NO2, can react fully with oxygen to form a different oxide of nitrogen, oxide Y, as the only product.
Oxide Y is collected and heated to 65.0∘C65.0^\circ\text{C}65.0∘C at a pressure of 98.0 kPa.
Under these conditions, oxide Y is a gas that occupies a volume of 125 cm3 and has a mass of 0.471 g.
Calculate the molar mass of oxide Y and suggest its molecular formula.
molar mass=………………… g mol−1 \text{molar mass} = \dots\dots\dots\dots\dots\dots\dots\text{ g mol}^{-1} molar mass=………………… g mol−1 molecular formula=………………… \text{molecular formula} = \dots\dots\dots\dots\dots\dots\dots molecular formula=…………………
