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

Question

1. A 3.00-L flask is filled with gaseous ammonia, NH3. The gas pressure measured at 18.0 C is 1.95 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.

2. If 1.00 mol of argon is placed in a 0.500-L container at 28.0 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(L2atm)/mol2 and b=0.03219L/mol. Express your answer to two significant figures and include the appropriate units.

Explanation / Answer

(1)

Given data,

Volume of flask, V = 3.00 L

Pressure of gas, P = 1.95 atm

Temperature, T = 18.0 0C = 291. K

Gaseous constant, R = 0.0821 L.atm.K-1.mol-1

Number of moles of NH3, n = ?

Assuming ideal gas behaviou, ideal gas equation,

P V = n R T

n = (1.95 * 3.00 ) / (0.0821 * 291.)

n = 0.245 mol

We know that, number of moles = mass / molar mass

0.245 = mass / 17.0

Mass of NH3 = 4.16 grams

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