The initial rate of this reaction was measured at a range of starting concentrations for the three reactants, and the outcomes are shown in the table. Use the data to work out the order with respect to each reactant: order with respect to $[\text{CH}_3\text{CHO}]$, order with respect to $[\text{CH}_3\text{OH}]$, and order with respect to $[\text{H}^+]$.
Use the results from part (i) to state the rate equation for the reaction.
State the units for the rate constant in the rate equation.
Calculate the relative rate for a mixture whose starting concentrations of all three reactants are $0.20\;\text{mol dm}^{-3}$.
Complete the second row of the table in terms of $x$, the concentration of acetal A at equilibrium. You may find it useful to look at the chemical equation opposite.
Using the given value of $[\text{acetal A}]$, $0.025\ \text{mol dm}^{-3}$, calculate the equilibrium concentrations of the other reactants and products and record them in the third row of the table.
Write the equilibrium constant expression for this reaction, $K_c$, and give its units.
Use the values in the third row of the table to work out $K_c$.