# Problem: A 3.00-L flask is filled with gaseous ammonia, NH3. The gas pressure measured at 25.0 °C is 1.55 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.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=nRTUnder 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:(P+an2V2)(V-nb)=nRTThe gas constant R is equal to 0.08206 L ⋅ atm/(K ⋅ mol).

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A 3.00-L flask is filled with gaseous ammonia, NH3. The gas pressure measured at 25.0 °C is 1.55 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.

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):

$\mathbf{PV}\mathbf{=}\mathbf{nRT}$

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:

$\left(P+\frac{{\mathrm{an}}^{2}}{{V}^{2}}\right)\mathbf{\left(}\mathbf{V}\mathbf{-}\mathbf{nb}\mathbf{\right)}\mathbf{=}\mathbf{nRT}$

The gas constant R is equal to 0.08206 L ⋅ atm/(K ⋅ mol).