Question

Simulating a Job’s plot. Consider the reaction $\mathbf{A}\mathbf{+}\mathbf{2}\mathbf{B}\mathbf{\rightleftharpoons }{\mathbf{AB}}_{\mathbf{2}}\mathbf{,}\mathbf{forwhich}\mathbf{}\mathbf{K}\mathbf{=}\mathbf{\left[}{\mathbf{AB}}_{\mathbf{2}}\mathbf{\right]}\mathbf{/}\mathbf{\left[}\mathbf{A}\mathbf{\right]}\mathbf{[}\mathbf{B}{\mathbf{]}}^{\mathbf{2}}$. Suppose that the following mixtures of A and B at a fixed total concentration of

10^-4 M are prepared:

(b)Prepare a graph by the method of continuous variation in which you plot$\left[{\mathrm{AB}}_2\right]$versus mole fraction offor each equilibrium constant. Explain the shapes of the curves.

Short answer

It is the ratio of number of mole of one component to the total number of moles in given mixture.

Step-by-step solution

Define mole fraction.

It is the ratio of number of mole of one component to the total number of moles in given mixture.

 Calculate mole fraction.

We will calculate mole fraction by=$\frac{\left[\mathrm{A}\right]}{\left[\mathrm{A}\right]+\left[\mathrm{B}\right]}$

Draw spreadsheet of mole fraction.

Draw graph.

With that, we conclude that stoichmetry is$1:2\left({\mathrm{AB}}_2\right),$ so the maximum mole fraction will be 0.33. The higher the equilibrium constant, the steeper the curve and this will results in hig extent of reaction.