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* Ideal versus Real Gases A Review Constants Periodic Table The ideal gas law describes the relationship among the volume of an ideal gas (V), its pressure (P), its absolute temperature (T), and number of moles (n) PV = nRT Part A Under standard conditions, the ideal gas law does a good job of approximating these properties for any gas. However, the ideal gas law does not account for all the properties of real gases such as intermolecular attraction and molecular volume, which become more pronounced at low temperatures and high pressures. The van der Waals equation corrects for these factors with the constants a and b, which are unique to each substance A3.00-L flask is filled with gaseous ammonia, NH3. The gas pressure measured at 26.0 °C is 2.15 atm Assuming ideal gas behavior, how many grams of ammonia are in the flask? Express your answer to three significant figures and include the appropriate units. View Available Hint(s) IHHA ? (P + **) (V – nb) = nRT mass of NH3 = Value Units The gas constant Ris equal to 0.08206 L.atm/(K.mol) Submit Ideal versus real behavior for gases In the following part you can see how the behavior of real gases deviates from the ideal behavior. You will calculate the pressure values for a gas using the ideal gas law and also the van der Waals equation. Take note of how they differ. Part B If 1.00 mol of argon is placed in a 0.500-L container at 26.0 °C, what is the difference between the ideal pressure (as predicted by the ideal gas law) and the real pressure (as predicted by the van der Waals equation)? For argon, a = 1.345 (L? .atm)/mol and b=0.03219 L/mol Express your answer to two significant figures and include the appropriate units. View Available Hint(s) THA ? Pideal - Preal Value Units Submit Part C Complete previous part(s)