Use the theoretical number of moles of H2 from #1, the partial pressure of H2 from #2, the volume of H2 gas collected (in L), and the temperature (in K) to find the experimental value of the universal gas constant (R): Data TableMass of Mg Ribbon0.0447gEvidence of Chemical ChangeYou can see the hydrogen gas bubbling, creating the gas bubbles inthe tube.Barometric Pressure in Lab748.9mmHgTemperature of Water Bath23.7 CVolume of H2 Gas Collected46.50mL Table 1. Vapor Pressure of Water at Different TemperaturesTemperature, °CPH,0, mm HgTemperature, °CPH,0, mm Hg16 °C13.622 °C19.817 °C14.523 °C21.118 °C15.524 °C22.419 °C16.525 °C23.820 °C17.526 °C25.221 °C18.727 °C26.7

We have to find the value of Universal gas constant for given data, from ideal gas law

Answered: Use the theoretical number of moles of…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Use the theoretical number of moles of H₂ from #1, the partial pressure of H₂from #2, the volume of H₂ gas collected (in L), and the temperature (in K) to find the experimental value of the universal gas constant (R):

Data Table
Mass of Mg Ribbon
0.0447g
Evidence of Chemical Change
You can see the hydrogen gas bubbling, creating the gas bubbles in
the tube.
Barometric Pressure in Lab
748.9mmHg
Temperature of Water Bath
23.7 C
Volume of H2 Gas Collected
46.50mL

Table 1. Vapor Pressure of Water at Different Temperatures
Temperature, °C
PH,0, mm Hg
Temperature, °C
PH,0, mm Hg
16 °C
13.6
22 °C
19.8
17 °C
14.5
23 °C
21.1
18 °C
15.5
24 °C
22.4
19 °C
16.5
25 °C
23.8
20 °C
17.5
26 °C
25.2
21 °C
18.7
27 °C
26.7

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