thank you ### Mole Fraction and Partial Pressure Calculation**Scenario:**Some \( \text{N}_2 \) gas is mixed with some \( \text{O}_2 \) gas, and the sketch below shows a representative sample of the mixture. The total pressure of the mixture is measured and found to be 0.120 kPa.**Diagram Explanation:**- The image shows a mixture of gas molecules.- Red circles represent oxygen molecules.- Blue circles represent nitrogen molecules.**Key:**- **Carbon:** Black- **Nitrogen:** Blue- **Oxygen:** Red- **Hydrogen:** White- **Sulfur:** Yellow- **Chlorine:** Green**Objective:**Calculate the mole fraction and partial pressure of each gas in this mixture. Round your answers to 3 significant digits. You may assume each gas behaves as an ideal gas.**Calculation:**1. **Count the Molecules:** - Count the number of each type of molecule in the diagram.2. **Determine Mole Fraction:** The mole fraction \( (X) \) can be calculated using the formula: \[ X_i = \frac{n_i}{n_{\text{total}}} \] where \( n_i \) is the number of molecules of gas \( i \), and \( n_{\text{total}} \) is the total number of gas molecules.3. **Calculate Partial Pressure:** The partial pressure \( P_i \) can be calculated using Dalton's Law of Partial Pressures: \[ P_i = X_i \times P_{\text{total}} \] where \( P_{\text{total}} \) is the total pressure of the gas mixture.**Input Fields:**Fill in the calculated values in the provided table:\[\begin{array}{|c|c|c|}\hline\text{gas} & \text{mole fraction} & \text{partial pressure} \\\hline\text{N}_2 & & \text{kPa} \\\hline\text{O}_2 & & \text{kPa} \\\hline\end{array}\]

Number of O2 molecules = 10 Number of N2 molecules = 10 Total number of molecules = 10 +10 = 20

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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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