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Consider two flasks at 25°C, one contains an ideal gas and the other contains the real gas SO3. Which statement regarding these gases is true? a. As the temperature approaches 0 K, the volume of the ideal gas will be smaller than the volume of SO3 because ideal gases have larger values of the van der Waals coefficient a. b. As the temperature is decreased, the ideal gas will liquefy first because ideal gases have larger values of the van der Waals coefficient b. c. After the temperature is increased about 100 K, the pressure of the ideal gas will be smaller than the pressure of SO3 because the van der Waals coefficient a for SO3 is large. d. After the temperature has been lowered about 100 K, the pressure of the ideal gas will be smaller than the pressure of SO3 because the van der Waals coefficient a for SO3 is large. e. As the temperature approaches 0 K, the volume of the ideal gas will be larger than the volume of SO3 because ideal gases lack intermolecular forces.