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O Macmillan Learning What pressure is exerted by 905.7 g of CH4 in a 0.570 L steel container at 142.8 K? P= atm

O Macmillan Learning What pressure is exerted by 905.7 g of CH4 in a 0.570 L steel container at 142.8 K? P= atm

Chemistry
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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**Question 16 of 16** What pressure is exerted by 905.7 g of CH₄ in a 0.570 L steel container at 142.8 K? P = _________ atm --- **Explanation:** This question requires calculating the pressure exerted by a given mass of methane (CH₄) gas in a container using the ideal gas law equation: \[ PV = nRT \] Where: - \( P \) is the pressure in atmospheres (atm) - \( V \) is the volume in liters (L) = 0.570 L - \( n \) is the number of moles of CH₄ - \( R \) is the ideal gas constant = 0.0821 L·atm/mol·K - \( T \) is the temperature in Kelvin (K) = 142.8 K **Steps:** 1. **Convert the mass of CH₄ to moles:** - Molecular weight of CH₄ ≈ 16.04 g/mol - Number of moles (\( n \)) = 905.7 g ÷ 16.04 g/mol 2. **Use the ideal gas law to find pressure (\( P \)):** - Rearrange the ideal gas law to solve for \( P \): \[ P = \frac{nRT}{V} \] - Insert the values to find \( P \). This calculation will yield the pressure in atmospheres exerted by the gas under the given conditions.
Transcribed Image Text:**Question 16 of 16** What pressure is exerted by 905.7 g of CH₄ in a 0.570 L steel container at 142.8 K? P = _________ atm --- **Explanation:** This question requires calculating the pressure exerted by a given mass of methane (CH₄) gas in a container using the ideal gas law equation: \[ PV = nRT \] Where: - \( P \) is the pressure in atmospheres (atm) - \( V \) is the volume in liters (L) = 0.570 L - \( n \) is the number of moles of CH₄ - \( R \) is the ideal gas constant = 0.0821 L·atm/mol·K - \( T \) is the temperature in Kelvin (K) = 142.8 K **Steps:** 1. **Convert the mass of CH₄ to moles:** - Molecular weight of CH₄ ≈ 16.04 g/mol - Number of moles (\( n \)) = 905.7 g ÷ 16.04 g/mol 2. **Use the ideal gas law to find pressure (\( P \)):** - Rearrange the ideal gas law to solve for \( P \): \[ P = \frac{nRT}{V} \] - Insert the values to find \( P \). This calculation will yield the pressure in atmospheres exerted by the gas under the given conditions.
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