Part c show all work ### Van der Waals Real Gas Calculation**Problem Statement:**Calculate the difference in pressure between methane and an ideal gas under the given conditions. **Given:**- **Number of moles (n):** 13.0 moles- **Volume (V):** 8.00 L- **Temperature (T):** 23.6 °C- **Van der Waals constants for methane:** - \( a = 2.300 \, \text{L}^2 \cdot \text{atm/mol}^2 \) - \( b = 0.0430 \, \text{L/mol} \)**Task:**Express your answer with the appropriate units.**Attempted Solution:**- **Pressure Difference:** 32.4 atm- **Result:** Incorrect; 3 attempts remainingThis exercise requires calculating the pressure difference using the Van der Waals equation for real gases and comparing it with the ideal gas law result. The answer input was found to be incorrect, indicating a need to revisit the calculations.

Part C 13.0 moles of gas are in a 8.00 L tank at 23.6°C. Calculate the difference in pressure between methane and an ideal gas under these conditions. The van der Waals constants for methane are a = 2.300 L?. atm/mol and b=0.0430 L/mol. Express your answer with the appropriate units. > View Available Hint(s) HA ? pressure difference = 32.4 atm %3D

Part C 13.0 moles of gas are in a 8.00 L tank at 23.6°C. Calculate the difference in pressure between methane and an ideal gas under these conditions. The van der Waals constants for methane are a = 2.300 L?. atm/mol and b=0.0430 L/mol. Express your answer with the appropriate units. > View Available Hint(s) HA ? pressure difference = 32.4 atm %3D

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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