Question A 3.00-L flask is filled with gaseous ammonia, NH3. The gas pressure me

Question

Question A 3.00-L flask is filled with gaseous ammonia, NH3. The gas pressure measured at 19.0?C is 2.25atm . Assuming ideal gas behavior, how many grams of ammonia are in the flask?

Given Formualas 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

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:

(P+an2V2)(V?nb)=nRT

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

Explanation / Answer

Remember the beautiful equation of: PV=nRT where P is pressure (in ATM), V is volume (in L), n is moles, R is the gas constant (0.08206 l*atm/k*mol), and t is temperature (in K. To convert from C to K, take C+273.15). So, for the first one. You would solve for it like this: 2.25atm*3.00L=n(0.08206 LAtm/Kmol)(295.15K) When we solve for n, we get 0.27m of NH3. Since the molecular weight of NH3 is 17.031g/Mol, we can take 0.27m and multiply it by 17.031, and get 4.7g of NH3.

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