Hydrogen fluoride, HF, can be made from the reaction

${\mathbf{H}}_{\mathbf{2}\left(g\right)}\mathbf{+}{\mathbf{F}}_{\mathbf{2}\left(g\right)}\mathbf{}\mathbf{}\mathbf{}\mathbf{\square }\mathbf{}\mathbf{}\mathbf{}\mathbf{2}{\mathbf{HF}}_{\left(g\right)}$

In one experiment, 0.10 mol of role="math" localid="1654926984654" ${\mathbf{H}}_{\mathbf{2}\mathbf{\left(}\mathbf{g}\mathbf{\right)}}$and 0.050 mol of ${\mathbf{F}}_{\mathbf{2}\left(g\right)}$are added to a 0.50-L f

lask. Write a reaction table for this process.

Thereaction table is a spreadsheet format that contains all numerical and algebraic data relevant to the problem and allows for the development of a consistent set of analytical and computational procedures inside a single calculational framework. We can use the approach to detect common ideas, evaluate issues, arrange computations, make logical conclusions, identify distracters, validate results, and move forward with confidence and precision to a solution.

Rewrite the reaction as follows:

${\mathrm{H}}_{2\left(\mathrm{g}\right)}+{\mathrm{F}}_{2(\mathrm{g})}\square 2{\mathrm{HF}}_{\left(\mathrm{g}\right)}$

The number of moles of ${\mathrm{H}}_2$is 0.10 mol and the number of moles of ${\mathrm{F}}_2$is 0.050 mol. The volume of the flask is 0.50L.

$$\begin{gathered} \left[{\mathrm{H}}_2\right]=\frac{0.010\mathrm{mol}}{50\mathrm{L}} \\ =0.20\mathrm{M} \\ \left[{\mathrm{F}}_2\right]=\frac{0.050\mathrm{mol}}{0.50\mathrm{L}} \\ =0.10\mathrm{M} \end{gathered}$$

Assume x (M) of and x (M) of dissociates and construct ICE table as follows.

Thus, the ICE table for the reaction is obtained.