**Question:**Use the ideal gas law to determine the pressure, in atmospheres, of 2.00 moles of CO gas in a 3.00 L flask at 25.0 °C.**Explanation:**To solve this problem, we use the Ideal Gas Law equation:\[ PV = nRT \]Where:- \( P \) is the pressure in atmospheres (atm)- \( V \) is the volume in liters (L)- \( n \) is the number of moles of gas- \( R \) is the ideal gas constant, \( 0.0821 \, \text{L atm/mol K} \)- \( T \) is the temperature in Kelvin (K)First, convert the temperature from Celsius to Kelvin:\[ 25.0 \, °C + 273.15 = 298.15 \, \text{K} \]Now, substitute the known values into the equation:\[ P \times 3.00 \, \text{L} = 2.00 \, \text{moles} \times 0.0821 \, \text{L atm/mol K} \times 298.15 \, \text{K} \]Solve for \( P \):\[ P = \frac{2.00 \times 0.0821 \times 298.15}{3.00} \]Calculate \( P \) for the final answer. **Understanding the van der Waals Equation**The van der Waals equation compensates for non-ideal behavior of gases by incorporating intermolecular forces and the volume of gas molecules into calculations. This adjustment provides a more accurate description of real gases compared to the ideal gas law.**Example Calculation with Carbon Monoxide (CO)**- For CO, the constants are: - \( a = 1.505 \, \text{L}^2\text{atm/mol}^2 \) - \( b = 0.03985 \, \text{L/mol} \)- Task: Use the van der Waals equation to determine the pressure, in atmospheres, of 2.00 moles of CO gas in a 3.00 L flask at 25.0 °C.- Remember: The gas constant \( R \) is 0.08206 L·atm/mol·K.**Van der Waals Equation**\[ \left( P + a \left( \frac{n}{V} \right)^2 \right) (V - nb) = nRT \]**Explanation of the Components**- \( P \): Pressure of the gas- \( V \): Volume of the container- \( n \): Moles of gas- \( T \): Temperature in Kelvin- \( R \): Ideal gas constant- \( a \) and \( b \): van der Waals constants specific to each gasThis equation modifies the ideal gas law to enable more precise calculations for gases that do not behave ideally, by accounting for molecular interactions and finite molecular sizes.

The ideal gas equation is: PV = nRT ......(1) Here, P is pressure, V is volume, n is the number of…

The van der Waals equation compensates for non-ideal behavior of gases by taking into account intermolecular forces and the volume of the gas molecules. For CO, a = 1.505 L²atm/mol² and b = 0.03985 L/mol. Use the van der Waals equation to determine the pressure, in atmospheres, of 2.00 moles of CO gas in a 3.00 L flask at 25.0 °C. Remember the gas constant, R, is 0.08206 L.atm/mol.K. P+a (V - nb) = nRT

The van der Waals equation compensates for non-ideal behavior of gases by taking into account intermolecular forces and the volume of the gas molecules. For CO, a = 1.505 L²atm/mol² and b = 0.03985 L/mol. Use the van der Waals equation to determine the pressure, in atmospheres, of 2.00 moles of CO gas in a 3.00 L flask at 25.0 °C. Remember the gas constant, R, is 0.08206 L.atm/mol.K. P+a (V - nb) = nRT

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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