Data Analysis

Determine the volume of hydrogen gas formed during the reaction.

Using Equation $6,$ calculate the partial pressure of the hydrogen gas $(P_{H2}),$ in atmosphere, that was formed. $($Recall $1$atm$=760mmHg)$

Using the ideal gas law $($Equation $5),$ calculate the number of moles of hydrogen gas formed.

Our calibration curve was calculated using a $50\mathrm{.}00mgZ\frac{n}{A}l$ mixture. Since the moles of $H_2$ gas formed during the reaction are proportional to the amount of reactants, the mass of the unknown mixture must be $50\mathrm{.}0mg$ to be able to use the calibration curve to calculate the $\%$ mass Al$.$ If the experimental mass of the unknown is not $50\mathrm{.}00mg,$ the moles of $H_2$ gas formed during the experiment must be scaled using the following equation:

$50\mathrm{.}00mg$ mixture $\frac{\text{e}\text{x}\text{p}\text{e}\text{r}\text{i}\text{e}\text{m}\text{n}\text{t}\text{a}\text{l}\text{m}\text{o}\text{l}of\text{h}\text{y}\text{d}\text{r}\text{o}\text{g}\text{e}\text{n}}{\text{e}\text{x}\text{p}\text{e}\text{r}\text{i}\text{m}\text{e}\text{n}\text{t}\text{a}\text{l}\text{m}\text{a}\text{s}\text{s}of\text{m}\text{i}\text{x}\text{t}\text{u}\text{r}\text{e}}$

Equation $720\%$

Use Equation $7$ to determine the number of moles of hydrogen gas that would be generated if the mass of the mixture is $50\mathrm{.}00mg.$

$50.00mg$ mix turex

Use the trendline from the plot you created in part A to determine the percent Al in the sample. Show your work here.