Lab 5 MW

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Dec 6, 2023

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Molar Volume of an Ideal Gas 1. Write the balanced equation for the reaction between solid zinc and aqueous hydrochloric acid. Be sure to include physical states. 2. Record and calculate the following for all three trials. Trial 1 Trial 2 Trial 3 a Mass of zinc used (g) 0.250g 0.500g 1.00g b Volume of 6.00 M HCl used (mL) 10mL 10mL 10mL c Molar mass of zinc (g/mol) 65.39g/mol 65.39g/mol 65.39g/mol d Moles of zinc reactant 0.0038mols 0.0076mol 0.0153mol e Moles of HCl reactant (Calculate from M and V ) 0.06mols 0.06mols 0.06mols f Identity of Limiting Reactant Zn Zn Zn g Moles of hydrogen produced calculated using stoichiometry from limiting reactant (mol) 0.0038mols 0.0076mols 0.0153mols h Volume of gas produced at initial room temperature of 21.5°C (mL) 92.2mL 184.5mL 368.9mL i Calculated Molar Volume of the ideal hydrogen gas at room temperature (Volume/moles), expressed in units of L/mol (use unrounded value of moles H 2 for calculation) – Calculated from your experimental data 24.263L/mol 24.276L/mol 24.269L/mol j Under what conditions of temperature and pressure is this molar volume value valid? Include units. 21.5 C/1atm 21.5 C/1atm 21.5 C/1atm 𝑍𝑛(𝑠) + 2𝐻𝐶𝑙(𝑎𝑞) → 𝑍𝑛𝐶𝑙 ଶ (𝑎𝑞) + 𝐻 ଶ (𝑔)
3. Compare the molar volumes obtained in your best two trials. (a) Did you expect these results using different amounts of zinc metal in each trial? (b) Did your Trial 3 have any results that were unexpected? (a) I did not expect the values to differ. (b) No. The top did pop off the syringe though. 4. Calculate the theoretical value of the molar volume of an ideal gas at 21.5 °C using the ideal gas law equation: PV = nRT where R = 0.08206 L · atm/(K · mol), under the same conditions of pressure used in your experiment. To solve for molar volume, rearrange the ideal gas law equation so you’re solving for V/n with an answer with units of L/mol. Show calculation. 5. Calculate the average experimental value for the molar volume at 21.5 °C, and compare this value with the theoretical “ideal” value at the same temperature. Average Molar Volume from Trials 1 and 2 (L/mol). This is your experimental value. 24.2695L/mol Ideal molar volume from #4 (L/mol). This is your theoretical value. 24.1667L/mol Explain any differences between these two values for molar volume. If there is no difference, explain why you should expect a difference. Hydrogen is not an ideal gas. An ideal gas has zero intermolecular forces and zero molecular volume. 𝑉 𝑛 = 𝑅𝑇 𝑃 = ൬ 0.08206(𝐿 ∗ 𝑎𝑡𝑚) 𝐾 ∗ 𝑚𝑜𝑙 ൰ (294.5𝐾) 1.00𝑎𝑡𝑚 = 24.16667𝐿/𝑚𝑜𝑙
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