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

Question

Part A

A 3.00-L flask is filled with gaseous ammonia, NH3. The gas pressure measured at 22.0 C is 2.55 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.

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(L2atm)/mol2 and b=0.03219L/mol.

Express your answer to two significant figures and include the appropriate units.

Explanation / Answer

PV = nRT

n = mass/MW

PV = m/MW*RT

m = PV*MW/(RT)

m = 2.55*3*17/(0.082*(22+273)) = 5.376 g of NH3

B)

PV = nRT

P = nRT/V = 1*0.082*(26+273)/(0.5) = 49.036 atm

For VDW

(P + a(n/V)^2) (V - nB) = nRT

a = 1.345

b = 0.03219

(P + a(n/V)^2) (V - nB) = nRT

(P + 1.345(1/0.5)^2) (0.5 - 1*0.03219) = 1*0.082(26+273)

P = 47.03 atm

Difference:

49.036 -47.03 = 2.006 atm in difference

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