Question 9 **Calculating the Density of Nitrogen Gas***Assuming it behaves as an ideal gas, calculate the density of nitrogen, N₂, at STP (Standard Temperature and Pressure).***Density Calculation:**\[ \text{density:} \ \underline{\hspace{3cm}} \ \text{g/L} \]---To calculate the density of nitrogen gas (N₂) under standard temperature and pressure conditions (0°C and 1 atm), you can use the ideal gas law:\[ PV = nRT \]Where:- \( P \) is the pressure (1 atm),- \( V \) is the volume in liters,- \( n \) is the number of moles,- \( R \) is the ideal gas constant (0.0821 L·atm/mol·K),- \( T \) is the temperature in Kelvin (273.15 K).For one mole of an ideal gas at STP:\[ V = \frac{RT}{P} = \frac{(0.0821 \ \text{L·atm/mol·K}) \times (273.15 \ \text{K})}{1 \ \text{atm}} \approx 22.414 \ \text{L/mol} \]The molar mass of nitrogen gas (N₂) is approximately 28.02 g/mol.**Density Calculation Steps:**1. **Moles of Nitrogen (N₂):** At STP, 1 mole of nitrogen gas occupies 22.414 L.2. **Calculate Density:** \[ \text{Density} = \frac{\text{Mass}}{\text{Volume}} = \frac{28.02 \ \text{g/mol}}{22.414 \ \text{L/mol}} \approx 1.25 \ \text{g/L} \]So, the density of nitrogen gas at STP is approximately 1.25 g/L.

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Answered: Assuming it behaves as an ideal gas,…

Assuming it behaves as an ideal gas, calculate the density of nitrogen, N,, at STP. density: g/L

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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