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
General Chemistry - Standalone book (MindTap Course List)
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Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
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Chapter5: The Gaseous State
Section: Chapter Questions
Problem 5.128QP: Plot the data given in Table 5.3 for oxygen at 0C to obtain an accurate molar mass for O2. To do...
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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).](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F10c6e2dc-d615-4613-bf12-6e31522fc631%2Fd3d19f79-adf4-42bf-b1e3-8c623aacde16%2Fjrm8eu_processed.jpeg&w=3840&q=75)
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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