H₂ volume (ml) Moles Al Moles Mg Moles Zn 4.8x10^-8 1.3x10^-3 40 1.6x10^-3 1.5x10^-6 2.7x10^-3 2.6x10^-3 70 1.8x10^-3 4.

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H Volume Ml Moles Al Moles Mg Moles Zn 4 8x10 8 1 3x10 3 40 1 6x10 3 1 5x10 6 2 7x10 3 2 6x10 3 70 1 8x10 3 4 1 (19.15 KiB) Viewed 34 times

H₂ volume (ml) Moles Al Moles Mg Moles Zn 4.8x10^-8 1.3x10^-3 40 1.6x10^-3 1.5x10^-6 2.7x10^-3 2.6x10^-3 70 1.8x10^-3 4.1x10^-3 4.0x10^-3 100 1. The balanced chemical reaction between Al and HCI resulting the formation of hydrogen gas is given below: 2Al(s) + 6HCl(aq) → 2AlCl3 + 3H₂ (9) Write the balanced equation for the reactions between Zn and HCI and Mg and HCI. Zn(s) + HCI (ag) → ZnCl2 + H2(g) Mg(s) + 2 HCl(ag) --> MgCl2(aq) + H₂(g) 2. Using the stoichiometry of your balanced equations above, calculate the ratio of moles Zn to moles Al needed to produce the same volume of H₂ gas. Reference your table from question #8 above and calculate the same ratio using your experimental data. What is the relationship, if any, between the ratio you calculated from the reaction stoichiometry and the experimental data?