A 0.239 g sample of a gas in a 100-mL flask exerts a pressure of 600 mmHg at 14 °C. What is the gas?

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We can use the Ideal gas law here

`1mmHg = 1.316*10^-3 atm`

`PV = nRT`

`P=600xx1.316xx10^3 =0.79 atm`

`V=0.1L`

`n=(0.239xx10^-3)/M`

`R=0.08206(atmL)/(molK)`

`T=273+14 = 287K`

`0.79xx0.1 =(0.239xx10^-3xx0.08206xx287)/M`

`M=0.014 (Kg)/(mol)=14g/(mol)`

*So the gas could be Nitrogen Or `N_2` .*

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