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Determine the number of grams of nitrogen gas present in a 5.00-L cylinder at 4.00 x 103 mm Hg and 23.0°C. 15.2 g 30.3 g O 389 g 2.30 × 104 g O 75.0 g

Determine the number of grams of nitrogen gas present in a 5.00-L cylinder at 4.00 x 103 mm Hg and 23.0°C. 15.2 g 30.3 g O 389 g 2.30 × 104 g O 75.0 g

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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**Determining the Number of Grams of Nitrogen Gas** **Problem Statement:** Calculate the number of grams of nitrogen gas present in a 5.00-liter (L) cylinder at a pressure of 4.00 × 10³ millimeters of mercury (mm Hg) and a temperature of 23.0°C. **Answer Choices:** 1. 15.2 grams 2. 30.3 grams 3. 389 grams 4. 2.30 × 10⁴ grams 5. 75.0 grams Students will use the Ideal Gas Law equation (PV = nRT) to determine the number of moles (n) of nitrogen gas, and subsequently convert the number of moles to grams given the molar mass of nitrogen (N₂). **Conditions Provided:** - Volume (V) = 5.00 L - Pressure (P) = 4.00 × 10³ mm Hg - Temperature (T) = 23.0°C or 296.15 K (23.0 + 273.15) - Gas constant (R) depending on pressure units. Note: The Ideal Gas Constant (R) is 0.0821 L·atm/mol·K when pressure is in atmospheres (atm). Convert pressure to atm if mm Hg is provided (1 atm = 760 mm Hg).
Transcribed Image Text:**Determining the Number of Grams of Nitrogen Gas** **Problem Statement:** Calculate the number of grams of nitrogen gas present in a 5.00-liter (L) cylinder at a pressure of 4.00 × 10³ millimeters of mercury (mm Hg) and a temperature of 23.0°C. **Answer Choices:** 1. 15.2 grams 2. 30.3 grams 3. 389 grams 4. 2.30 × 10⁴ grams 5. 75.0 grams Students will use the Ideal Gas Law equation (PV = nRT) to determine the number of moles (n) of nitrogen gas, and subsequently convert the number of moles to grams given the molar mass of nitrogen (N₂). **Conditions Provided:** - Volume (V) = 5.00 L - Pressure (P) = 4.00 × 10³ mm Hg - Temperature (T) = 23.0°C or 296.15 K (23.0 + 273.15) - Gas constant (R) depending on pressure units. Note: The Ideal Gas Constant (R) is 0.0821 L·atm/mol·K when pressure is in atmospheres (atm). Convert pressure to atm if mm Hg is provided (1 atm = 760 mm Hg).
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