This question is about methanoic acid and oxides of nitrogen.
An investigation is carried out on the equilibrium system shown below:
2HCOOH(g)⇌(HCOOH)2(g)ΔH=−60.1 kJ mol−1 2\text{HCOOH}(\text{g}) \rightleftharpoons (\text{HCOOH})_2(\text{g}) \quad \Delta H = -60.1\text{ kJ mol}^{-1} 2HCOOH(g)⇌(HCOOH)2(g)ΔH=−60.1 kJ mol−1A sealed flask containing 6.00 moles6.00\text{ moles}6.00 moles of HCOOH(g)\text{HCOOH}(\text{g})HCOOH(g) is heated to a constant temperature and allowed to reach equilibrium.
The equilibrium mixture contains 4.80 mol of HCOOH(g)\text{HCOOH}(\text{g})HCOOH(g), and the total pressure is 3.00 bar3.00\text{ bar}3.00 bar.
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 (HCOOH)2(g)(\text{HCOOH})_2(\text{g})(HCOOH)2(g) formed at equilibrium.
In an experiment, nitrogen monoxide, NO\text{NO}NO, reacts fully with oxygen to form a different oxide of nitrogen, oxide Y, as the only product.
Oxide Y is collected and heated to 60.0∘C60.0^\circ\text{C}60.0∘C at a pressure of 105 kPa.
Under these conditions, oxide Y is a gas that occupies a volume of 150 cm3 and has a mass of 0.262 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=…………………
