**Educational Content: Understanding Pressure and Mole Fraction in a Nitrogen Mixture**1. **What fraction of the pressure is due to nitrogen?** *Note:* The fraction due to nitrogen is calculated using the formula: \[ \text{fraction due to nitrogen} = \frac{\text{N}_2 \text{ pressure}}{\text{total pressure}} = \frac{P_{N_2}}{P_T} \]2. **What is the nitrogen mole fraction in the tank?** *Note:* The mole fraction of nitrogen is determined by: \[ \text{mole fraction of nitrogen} = \frac{\text{moles of N}_2}{\text{total moles}} = \frac{n_{N_2}}{n_T} \]3. **What is the relationship between the nitrogen pressure ratio in Key Question 4 and the nitrogen mole fraction in Key Question 5?** Express this relationship in the form of an equation.This educational content explains how to determine the fraction of pressure and mole fraction in a gas mixture, specifically nitrogen, using fundamental equations in chemistry. **Model: Gases Exert Pressure Independently**This educational table illustrates how gases exert pressure independently under a controlled environment.| Condition | Pressure | Volume | Temperature | Comment ||-----------|----------|--------|-------------|---------|| Initial | 1.0 atm | 22.4 L | 273 K | 1.0 mole of N₂ gas fills the tank. || Final | 3.0 atm | 22.4 L | 273 K | 2.0 moles of O₂ gas have been added to the 1 mole of N₂ gas in the tank. |**Explanation:**- **Initial Condition:** At the start, the tank contains 1.0 mole of nitrogen gas (N₂) at a pressure of 1.0 atm, a volume of 22.4 liters, and a temperature of 273 K.- **Final Condition:** After modifications, the pressure increases to 3.0 atm while keeping the volume and temperature constant. This change results from adding 2.0 moles of oxygen gas (O₂) to the existing nitrogen gas in the tank. This example demonstrates the concept of partial pressures and how gases in a mixture contribute independently to the total pressure.

Given: At constant temperature and volume of 273 K and 22.4 L respectively, the pressure of the tank…

What fraction of the pressure is due to nitrogen? Note: fraction due to nitrogen = N₂ pressure/total pressure = PN₂ / PT What is the nitrogen mole fraction in the tank? Note: mole fraction of nitrogen = moles of N₂ / total moles = = N₂/nT hat is the relationship between the nitrogen pressure ratio in Key Question 4 and the nitrogen ole fraction in Key Question 5? Express this relationship in the form of an equation.

What fraction of the pressure is due to nitrogen? Note: fraction due to nitrogen = N₂ pressure/total pressure = PN₂ / PT What is the nitrogen mole fraction in the tank? Note: mole fraction of nitrogen = moles of N₂ / total moles = = N₂/nT hat is the relationship between the nitrogen pressure ratio in Key Question 4 and the nitrogen ole fraction in Key Question 5? Express this relationship in the form of an equation.

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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