Chemistry Determining Number of Moles Question

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The discussion revolves around calculating the number of moles of acetone vapor in a Hickman still using the ideal gas law. The temperature is converted to Kelvin at 343K, and the pressure is adjusted to atmospheric units, resulting in 0.736 atm. The volume of the still is set at 25 mL, converted to liters for the calculation. The final calculation yields approximately 8.59 x 10^-7 moles of acetone vapor, confirming the accuracy of the work presented. The answer is validated as correct.
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Hello. Just need this answer checked. Thanks.

If we can reasonably treat acetone vapor as an ideal gas at the Tboil =70° C and we approximate the volume of a Hickman still as ~25mL then how many moles of acetone are in the vapor phase inside the still? (PV=nRT) (R=0.0821 L*atm/mol*K) (Get conversion of P & T in right form.)

Answer:-

T= 70+273=343K
P=0.736/760=9.68x10-4atm
R=0.0821 L*atm/mol*K
V= 25x10-3L
n=no.of moles = PV/RT= 9.68x10-4atm x 25x10-3L /(0.0821 L*atm/mol*K x 343K)
= 8.59x10-7
 
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lol, yes it is correct!
 
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