Table 1. Vapor Pressure of Water at Different lem Temperature, °C PH3Os mm Hg Temperature, C PHo, 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 A reaction of 0.028 g of magnesium with excess hydrochloric acid generated 31.0 mL of hydrogen gas was collected by water displacement in a 22 °C water bath. The barometric pressure gas. The in the lab that day was 746 mm Hg. 1. Use Dalton's law and the vapor pressure of water at 22 °C (Table 1) to calculate the partial pressure of hydrogen gas in the gas collecting tube. 2. Use the combined gas law to calculate the "corrected" volume of hydrogen at STP. Hint: Watch your units for temperature and pressure! 3. What is the theoretical number of moles of hydrogen that can be produced from 0.028 g of Mg? Hint: Refer to Equation I for the balanced equation for the reaction. 4. Divide the corrected volume of hydrogen by the theoretical number of moles of hydrogen to calculate the molar volume (in L/mol) of hydrogen at STP.
Table 1. Vapor Pressure of Water at Different lem Temperature, °C PH3Os mm Hg Temperature, C PHo, 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 A reaction of 0.028 g of magnesium with excess hydrochloric acid generated 31.0 mL of hydrogen gas was collected by water displacement in a 22 °C water bath. The barometric pressure gas. The in the lab that day was 746 mm Hg. 1. Use Dalton's law and the vapor pressure of water at 22 °C (Table 1) to calculate the partial pressure of hydrogen gas in the gas collecting tube. 2. Use the combined gas law to calculate the "corrected" volume of hydrogen at STP. Hint: Watch your units for temperature and pressure! 3. What is the theoretical number of moles of hydrogen that can be produced from 0.028 g of Mg? Hint: Refer to Equation I for the balanced equation for the reaction. 4. Divide the corrected volume of hydrogen by the theoretical number of moles of hydrogen to calculate the molar volume (in L/mol) of hydrogen at STP.
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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Please answer 1, 2 and 3 as we are allowed to ask 3 questions at once please and thank you!!
Transcribed Image Text:Table 1. Vapor Pressure of Water at Different Temperatures
Temperature, C
PH,0, mm Hg
Temperature, °C
PHo, 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
A reaction of 0.028 g of magnesium with excess hydrochloric acid generated 31.0 mL of hydrogen
gas. The gas was collected by water displacement in a 22 °C water bath. The barometric pressure
in the lab that day was 746 mm Hg.
1. Use Dalton's law and the vapor pressure of water at 22 °C (Table 1) to calculate the partial
pressure of hydrogen gas in the gas collecting tube.
2. Use the combined gas law to calculate the "corrected" volume of hydrogen at STP. Hint:
Watch your units for temperature and pressure!
3. What is the theoretical number of moles of hydrogen that can be produced from 0.028 g of
Mg? Hint: Refer to Equation 1 for the balanced equation for the reaction.
4. Divide the corrected volume of hydrogen by the theoretical number of moles of hydrogen to
calculate the molar volume (in L/mol) of hydrogen at STP.
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