Fig. 2.1 illustrates how the rate of the forward reaction varies with time. At the start, the reverse reaction rate is zero. Finish Fig. 2.1 by drawing the way the reverse reaction rate changes over time.
State how the equilibrium position changes, if it changes at all, when the reaction is carried out at $100^\circ\text{C}$. Explain your answer. Assume the pressure stays constant.
Table 2.1 gives the composition of an equilibrium mixture of NO(g), NO$_2$(g) and N$_2$O$_3$(g) at $101\,\text{kPa}$. Calculate $K_p$, the equilibrium constant in terms of partial pressures. Deduce the units of $K_p$.
Identify one natural process and one human-made process that lead to the formation of atmospheric NO and NO$_2$.
NO$_2$ is a free radical. Define the term free radical.
NO$_2$ has a catalytic role in the oxidation of atmospheric sulfur dioxide. Write equations to show how NO$_2$ acts catalytically in this oxidation.
State one environmental consequence of atmospheric sulfur dioxide being oxidised.
Identify one base the student could use.
The student evaporates the water to obtain solid magnesium nitrate. When this solid is heated, it decomposes. Write an equation for the decomposition of magnesium nitrate.
State the way in which the thermal stability of Group 2 nitrates changes down the group.