Question

4 2 O.021 3m L Mass of Me strip (e)O.O15 5pmL O.020 3mL almL 19ML 16ML 3ML 23mL 2 OmL 3mL 21eL 21mL Initial vol. of syringe (mL) 19mL Final vol. of syringe (mL) 18mL 14ML Volume of H: gas (mL) FiNGl Volume Barometric pressure, torr (given): 25.SC Ambient temperature, "C (given): as aoc Vapor pressure of water, torr (Table 6.1): Determine R from your data. 1. The amount (in moles) of H2 gas formed is equal to the amount of Mg that was consumed, as shown in the chemical reaction equation. Find the moles of Mg. Show work for at least one trial. 2 3 5 2. Determine the pressure of H2 gas. Use your data and Table 6.1 and rearrange Patmosphere = Prydrogen+ Pwater to find Pydrogen (How many torr 1 atm?) Show work for at least one trial. Pydrogen 3. Convert the ambient temperature from "C to Kelvin. Circle your answer.
Please answer #4

Answer 1

Determine P from 1.) The amount amine R from given Data formed is equalto amount amount of 1₂ gas( in moles of Mg that was consumed so, Molar mass of Mg = 24 g/mole fou trual ☺ maes of Mg struip > 0.015 g 19 mole = 0.015 mars Molar mass - = 0.000625 moles similarly, moles of 0.000833 moles 0.000625 0.000875 0.000667 0.000 75 : moles gos 1. 2.) Pressure of H₂ gas . 1 Patomosphera = Temberatwee = 25.5°C Patm = 765.8 torr Pho = 25.2 torri. PH₂ + Puzo - Patm - P420 765.9 - 25.2 = 74-0.640901 3.) 760 +0901 = 1 atm 50, 740.6 10:01 = 0.9745 atm PH2 = 0974-5 alm. temb foc) to Kelvin 0°C = 2.73.15 K So, 25.5 = 273.15+ 25.5 = 298.65K calculate or using PV=nRT Ro Py = Rue x Vez 0.9745 X Noall) next Mortex 298.65 - 4.) R= 0.9745x VH₂ | ML) MIX 298.65X 1000

for trial 0 o Volle Vol. - ryml 0.000625 , M, volk Ne 0.9 14.5 X 14 0 0.00062.5 X 29%.65 X1000 - = .013'1 " 0.013.1 od 2 Similarely - valeu 0.0% 2.2 0.013 | 0.067 10.0183 0,0 %10 Catmily hot к) 5.) Average for R = 0.0175 L atm/molk Standard deviation = Eln-52 we get standard deviation = D.DOSg. 1 ) b + || - 0 3 + 0:0 S + 95 + 211 ) 09