Calculate the pressure exerted by 0.5900 mole of  in a 1.1000-L container at 25.0°C. (The gas constant is 0.08206 L·atm/mol·K. Take absolute zero to be –273.2°C.) Use the ideal gas law. (Enter your answer to four significant figures.) Pressure =  atm Use the van der Waals equation. (For : a = 1.39 atm L2/mol2, and b = 0.0391 L/mol. Enter your answer to four significant figures.) Pressure =  atm Compare the results. (Enter your answer to two significant figures.) The _________ideal gas lawvan der Waals equation is higher by  atm, or %.

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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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Calculate the pressure exerted by 0.5900 mole of  in a 1.1000-L container at 25.0°C.

(The gas constant is 0.08206 L·atm/mol·K. Take absolute zero to be –273.2°C.)

  1. Use the ideal gas law.

    (Enter your answer to four significant figures.)

    Pressure =  atm

  2. Use the van der Waals equation.

    (For : a = 1.39 atm L2/mol2, and b = 0.0391 L/mol. Enter your answer to four significant figures.)

    Pressure =  atm

  3. Compare the results.

    (Enter your answer to two significant figures.)

    The _________ideal gas lawvan der Waals equation is higher by  atm, or %.

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