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You can use the ideal gas law to find the number of moles of gas present. I'll be converting the mL to L, the Celsius to Kelvin, and the torrs to atmospheres.

Ideal gas law :

PV = nRT

P = (659 torr) x (1 atm / 760 torr) = 0.867 atm

V = 14.3 mL = 0.0143 L

n = ?

R = (0.08206 L•atm / mol•K)

T = 295 K ................... [ converting Celsius to Kelvin; (22 + 273) = 295 ]

Rearranging the ideal gas law equation to solve for n gives

n = (PV / RT)

= (0.867 atm x 0.0143 L) / [(0.08206 L•atm / mol•K) x 295 K]

= 5.12 x 10^(-4) moles gas

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A mole of any gas at STP has volume 22.4 L , so that's the conversion factor to use :

(5.12 x 10^(-4) moles) x (22.4 L / 1 mole) = 0.0115 L = 11.5 mL

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what if you had 16.4mL? what would the volume be at?