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What is the experimental molar mass (that is, calculated from the data given and not taken from the periodic table) of magnesium if 0.0181 grams of magnesium generates 18.53 mL of hydrogen at 23.3 °C with a hydrogen partial pressure of 742.0 torr? Note that the partial pressure of water vapor has already been subtracted from the total pressure.     26.2 g/mol     23.8 g/mol     21.0 g/mol     24.3 g/mol     26.0 g/mol

What is the experimental molar mass (that is, calculated from the data given and not taken from the periodic table) of magnesium if 0.0181 grams of magnesium generates 18.53 mL of hydrogen at 23.3 °C with a hydrogen partial pressure of 742.0 torr? Note that the partial pressure of water vapor has already been subtracted from the total pressure.     26.2 g/mol     23.8 g/mol     21.0 g/mol     24.3 g/mol     26.0 g/mol

Chemistry
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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  1. What is the experimental molar mass (that is, calculated from the data given and not taken from the periodic table) of magnesium if 0.0181 grams of magnesium generates 18.53 mL of hydrogen at 23.3 °C with a hydrogen partial pressure of 742.0 torr? Note that the partial pressure of water vapor has already been subtracted from the total pressure.
       
    26.2 g/mol
       
    23.8 g/mol
       
    21.0 g/mol
       
    24.3 g/mol
       
    26.0 g/mol
Expert Solution
Step 1

Given :

Mass of Mg = 0.0181 g

Volume of hydrogen = 18.53 ml

Temperature = 23.3 °C

Partial pressure of hydrogen = 742 torr

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