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1. In an electrolysis cell similar to the one employed in this experiment, a student observed that his unknown metal anode lost 0.233 g while a total volume of 94.50 mL of H2 was being produced. The temperature in the laboratory was 25 °C, and the barometric pressure was 740 mm Hg. At 25 °C, the vapor pressure of water is 23.8 mm Hg. To find the equivalent mass of his metal, the student filled in the blanks below: P hydrogen gas = P bar - VP mm Hg = atm water V hydrogen gas mL T = K n hydrogen gas moles

1. In an electrolysis cell similar to the one employed in this experiment, a student observed that his unknown metal anode lost 0.233 g while a total volume of 94.50 mL of H2 was being produced. The temperature in the laboratory was 25 °C, and the barometric pressure was 740 mm Hg. At 25 °C, the vapor pressure of water is 23.8 mm Hg. To find the equivalent mass of his metal, the student filled in the blanks below: P hydrogen gas = P bar - VP mm Hg = atm water V hydrogen gas mL T = K n hydrogen gas moles

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. In an electrolysis cell similar to the one employed in this experiment, a student observed that his unknown metal anode lost 0.233 g while a total volume of 94.50 mL of H2 was being produced. The temperature in the laboratory was 25 °C, and the barometric pressure was 740 mm Hg. At 25 °C, the vapor pressure of water is 23.8 mm Hg. To find the equivalent mass of his metal, the student filled in the blanks below: P hydrogen gas =P bar - VP water mm Hg = atm %3D %3D V hydrogen gas mL = L T = K n hydrogen gas moles
Transcribed Image Text:1. In an electrolysis cell similar to the one employed in this experiment, a student observed that his unknown metal anode lost 0.233 g while a total volume of 94.50 mL of H2 was being produced. The temperature in the laboratory was 25 °C, and the barometric pressure was 740 mm Hg. At 25 °C, the vapor pressure of water is 23.8 mm Hg. To find the equivalent mass of his metal, the student filled in the blanks below: P hydrogen gas =P bar - VP water mm Hg = atm %3D %3D V hydrogen gas mL = L T = K n hydrogen gas moles
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