**Charles's Law:**

$\overline{)\frac{{\mathbf{V}}_{{\mathbf{1}}}}{{\mathbf{T}}_{\mathbf{1}}}{\mathbf{=}}\frac{{\mathbf{V}}_{{\mathbf{2}}}}{{\mathbf{T}}_{\mathbf{2}}}}$

V_{1} = 1.56 mL

V_{2} = ??

T_{1} = 95°C + 273.15 = 368.15 K

T_{2} = 0.6°C + 273.15 = 273.75 K

A syringe containing 1.56 mL of oxygen gas is cooled from 95.0°C to 0.6°C. What is the final volume V_{f} of oxygen gas? (Assume that the pressure is constant.)

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