CHE 169 Exp.## 8 MOLAR VOLUME OF A GAS LABORATORY REPORT Name Section Desk No. D

Question

CHE 169 Exp.## 8 MOLAR VOLUME OF A GAS LABORATORY REPORT Name Section Desk No. Date DATA RECORD ALL DATA IN INK using the correct number of significant figures and correct units 1. Mass of magnesium sample 2. Volume of hydrogen 3. Temperature of hydrogen 4. Temperature of water 5. Barometric pressure 6. Difference in water levels 7. Aqueous vapor pressure CALCULATIONS: SHOW COMPLETE "SET-UPS" (and the rounding off) FOR ALL CALCULATIONS on the back of this page or on a separate sheet. Report results to the correct number of significans figures and correct units. 2. Mercury equivalent of the difference of water levels 3. Partial pressure of dry hydrogen 4. Volume of dry hydrogen at STP 5. Moles of hydrogen 6. Molar volume at STP 7. Average molar volume at STP Average deviation 8, % Dev. of average STP molar V from ideal STP molar v

Explanation / Answer

                                            Trial 1                 Trial 2

2) mercury equivalent              7.35                   7.35

3) Partial pressure H2           761-7.35                761-7.35

                                          753.65                  753.65

4) Volume

TRial 1

V1 = P2V2/P1 = 753.65 X 94.15 / 760 = 93.36mL

Trial 2

V1 = P2V2/P1 = 753.65 X 93.10 / 760 = 92.32 mL

5) The mole ratio of hydrogen and magnesium are same

Trial 1

Moles of Mg = Mass / atomic mass = 0.0766g / 24 = 0.0032 = Moles of hydrogen

Trial 2

Moles of Mg = Mass / atomic mass = 0.0743g / 24 = 0.0031 = Moles of hydrogen

6) Molar volume at STP

Volume / mole = molar volume

Trial 1

Molar volume = 0.09415 / 0.0032 = 29.42 L /mole

Trial 2

Molar volume = 0.0931 / 0.0031 = 30.03 L /mole

7) average molar volume =29.42+ 30.03 / 2 = 29.73 L / mole

8) Deviation = 22.24 - 29.73 = 7.49

%deviation = 7.49 X 100 / 22.4 = 33.44 %

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