Mass of the gelatin capsule was: 0.1134 g Mass of the capsule and the allow sample was: 0.3218 g Ambient Temperature was: 23°C Mass of empty beaker: 154.3 g Mass of beaker with water: 401.6 g Vapor pressure of water for this data: 21.1 mmHg Atmospheric Pressure: 732 mmHg Assume density of water to be 1.0000 g/mL What is the volume of the displaced water in Liters? Using PH2V= nH2RT, nH2=PH2V/RT how many moles of H2 were evolved? Determine the number of moles of H2 per gram of sample. Determine the %Al using NH2= (%AL/100 * 0.0556) + (100-%AL/100 * 0.0153)
Mass of the gelatin capsule was: 0.1134 g Mass of the capsule and the allow sample was: 0.3218 g Ambient Temperature was: 23°C Mass of empty beaker: 154.3 g Mass of beaker with water: 401.6 g Vapor pressure of water for this data: 21.1 mmHg Atmospheric Pressure: 732 mmHg Assume density of water to be 1.0000 g/mL What is the volume of the displaced water in Liters? Using PH2V= nH2RT, nH2=PH2V/RT how many moles of H2 were evolved? Determine the number of moles of H2 per gram of sample. Determine the %Al using NH2= (%AL/100 * 0.0556) + (100-%AL/100 * 0.0153)
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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Mass of the gelatin capsule was: 0.1134 g
Mass of the capsule and the allow sample was: 0.3218 g
Ambient Temperature was: 23°C
Mass of empty beaker: 154.3 g
Mass of beaker with water: 401.6 g
Vapor pressure of water for this data: 21.1 mmHg
Atmospheric Pressure: 732 mmHg
Assume density of water to be 1.0000 g/mL
What is the volume of the displaced water in Liters?
Using PH2V= nH2RT, nH2=PH2V/RT how many moles of H2 were evolved? Determine the number of moles of H2 per gram of sample. Determine the %Al using
NH2= (%AL/100 * 0.0556) + (100-%AL/100 * 0.0153)
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