Gases begin to lose their ideal behavior under conditions of low temperature and/or highpressures. At wer temperatures and/or high pressures, interparticular attractions canbegin to take place, which result in attractive forces between gas particles, which result ina diminished collision frequency and force on the container walls, which results in a gaspressure that is lower than would be expected from ideal-behaving gas. Therefore thePV/RT ratio that is normally equal to 1 for one mole of gas is now less than 1. At verylow temperatures and/or very high pressures, the particles of gas become significant withrespect to the gas volume due to repulsive forces between the particles, which results in agas volume that is higher than would be expected from ideal-behaving gas. Therefore thePV/RT ratio that is normally equal to 1 for one mole of gas is now greater than 1. Toadjust for this deviation from ideal behavior, the van der Waals equation below adjusts thepressure UP and the volume DOWN when considering the PV = nRT equation of state fornon-ideal gas behavior:(P+n²a/V²) (V-nb) = nRTwhers a and b are van der Waals constantsGenerally speaking, the larger the gas (the greater number of electrons, the greater theelectron distribution, the more complex gas particle, and the stronger attractive forcesbetween the particles), the larger the van der Waal constant a. The larger the particlevolume, the larger the van der Waals constant b.Which statement(s) is/are true?I. Ideally, the molar volume of a gas is 22.414 L at 1 atm and 25°C.II. The van der Waals "a" is greater for SO₂(g) than for He(g).III. For most gases, the slope of the PV/RT vs. Pext plot is initially negative.IV. The value of the van der Waals "b" is an indication of the strength of the IMF'sin the gas. VIR Mution, une vie complex gas parucie, and the stronger attractive forcesbetween the particles), the larger the van der Waal constant a. The larger the particlevolume, the larger the van der Waals constant b.Which statement(s) is/are true?I. Ideally, the molar volume of a gas is 22.414 L at 1 atm and 25°C.II. The van der Waals "a" is greater for SO₂(g) than for He(g).III. For most gases, the slope of the PV/RT vs. Pext plot is initially negative.IV. The value of the van der Waals "b" is an indication of the strength of the IMF'sin the gas.O I,II,IV onlyO Ill onlyO II,III onlyO I,II,III only

Vanderwaal's constant "a" represents for inter-molecular forces constant "b" is a correction for…

tractive forces between the particles), the larger the van der Waal constant a. The larger the particle volume, the larger the van der Waals constant b. Which statement(s) is/are true? I. Ideally, the molar volume of a gas is 22.414 L at 1 atm and 25°C. II. The van der Waals "a" is greater for SO₂(g) than for He(g). III. For most gases, the slope of the PV/RT vs. Pext plot is initially negative. IV. The value of the van der Waals "b" is an indication of the strength of the IMF's in the gas. O I,II,IV only Ill only O II,III only O I,II,III only

tractive forces between the particles), the larger the van der Waal constant a. The larger the particle volume, the larger the van der Waals constant b. Which statement(s) is/are true? I. Ideally, the molar volume of a gas is 22.414 L at 1 atm and 25°C. II. The van der Waals "a" is greater for SO₂(g) than for He(g). III. For most gases, the slope of the PV/RT vs. Pext plot is initially negative. IV. The value of the van der Waals "b" is an indication of the strength of the IMF's in the gas. O I,II,IV only Ill only O II,III only O I,II,III only

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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