For oxygen gas, the van der Waals equation of state achieves its best fit for a = 0.14 N.m²/mol² and b = 3.2 x 10-5 m³/mol. Part A Determine the pressure in 1.3 mol of the gas at 6 °C if its volume is 0.50 L, calculated using the van der Waals equation. Express your answer using two significant figures. IVE| ΑΣΦ ? Pa Request Answer Part B Determine the pressure in 1.3 mol of the gas at 6 °C if its volume is 0.50 L, calculated using the ideal gas law. Express your answer using two significant figures. [ΕΙ ΑΣΦ ? P= Submit P = Submit Request Answer Pa

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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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For oxygen gas, the van der Waals equation of state achieves
its best fit for a = 0.14 N.
·m²/mol² and
4
b = 3.2 × 10−5 m³/mol.
Part A
Determine the pressure in 1.3 mol of the gas at 6 °C if its volume is 0.50 L, calculated using the van der Waals equation.
Express your answer using two significant figures.
17| ΑΣΦ
?
Pa
Request Answer
Part B
Determine the pressure in 1.3 mol of the gas at 6 °C if its volume is 0.50 L, calculated using the ideal gas law.
Express your answer using two significant figures.
VE ΑΣΦ
P =
Pa
Submit
P =
Submit
Request Answer
Transcribed Image Text:For oxygen gas, the van der Waals equation of state achieves its best fit for a = 0.14 N. ·m²/mol² and 4 b = 3.2 × 10−5 m³/mol. Part A Determine the pressure in 1.3 mol of the gas at 6 °C if its volume is 0.50 L, calculated using the van der Waals equation. Express your answer using two significant figures. 17| ΑΣΦ ? Pa Request Answer Part B Determine the pressure in 1.3 mol of the gas at 6 °C if its volume is 0.50 L, calculated using the ideal gas law. Express your answer using two significant figures. VE ΑΣΦ P = Pa Submit P = Submit Request Answer
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