Partial Pressure Calculation for Argon Gas Collected Over Water at 30.0oC

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To calculate the number of moles of argon gas collected over water at 30.0°C, the total pressure of 771 torr is adjusted for the vapor pressure of water at 31.8 torr, resulting in a partial pressure of argon of approximately 739.2 torr. This leads to the calculation of moles of argon, yielding 9.78e-3 mol. The partial pressure of argon is converted to atmospheres, resulting in approximately 0.973 atm. However, the total mass of gas cannot be expressed in atmospheres, indicating an error in the initial mass calculation. Accurate mass determination requires converting moles of argon to grams using its molar mass.
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A sample of argon gas is collected over water at 30.0oC. The level of the
water is adjusted until the total pressure in the flask is 771 torr and the volume is 250.0
mL. The vapor pressure of water is 31.8 torr at 30.0oC.

A. How many moles of argon are in the flask?
B. What is the partial pressure of argon in the flask?
C. What is the total mass of gas in the flask?

I got:
a) 9.78e-3 mol
b) .973atm
c) 1.946 atm
 
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And?

c is definitely wrong - mass is not measured in atm.
 
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