Recall that the ** ideal gas law** is:

$\overline{){\mathbf{PV}}{\mathbf{=}}{\mathbf{nRT}}}$

Therefore, the initial and final pressure and volume of the gas are related by ** Boyle’s Law**:

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

A fixed quantity of gas at 23 ^{o}C exhibits a pressure of 756
torr and occupies a volume of 5.32
L.

Calculate the volume the gas will occupy if the pressure is increased to 1.88 atm while the temperature is held constant.

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