A reaction of 0.028 g of magnesium with excess hydrochloric acid generated 31.0 mL of gas. The gas was collected by water displacement in a 22°C water bath. The barometric pressure in the lab that day was 746 mmHg. A. Using Dalton's Law and the vapor pressure of water at the given temperature to calculate the partial pressure of hydrogen gas in the collection tube. 7 B. Use the combined gas law to calculate the corrected volume of hydrogen at STP. C. What is the theoretical number of moles of hydrogen that cạn be produced from 0.028 g of magnesium reacting with excess hydrochloric acid?
A reaction of 0.028 g of magnesium with excess hydrochloric acid generated 31.0 mL of gas. The gas was collected by water displacement in a 22°C water bath. The barometric pressure in the lab that day was 746 mmHg. A. Using Dalton's Law and the vapor pressure of water at the given temperature to calculate the partial pressure of hydrogen gas in the collection tube. 7 B. Use the combined gas law to calculate the corrected volume of hydrogen at STP. C. What is the theoretical number of moles of hydrogen that cạn be produced from 0.028 g of magnesium reacting with excess hydrochloric acid?
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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