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A gas is placed in a 5.0-mL syringe. It exerts 141 mm Hg of pressure on the inside walls of the syringe. The syringe's plunger is pressed, reducing the volume of the syringe to 2.9 mL. The cap was not removed from the syringe, so none of the gas escapes. Assuming the temperature of the gas does not change, use Boyle's law (below) to determine the pressure of the compressed gas. P_1V_1 = P_2V_2

Sagot :

Answer: [tex]243.10\ mm\ \text{of}\ Hg[/tex]

Explanation:

Given

The initial volume of gas [tex]V_1=5\ ml[/tex]

Initial pressure is [tex]P_1=141\ mm\ \text{of}\ Hg[/tex]

Final volume is [tex]V_2=2.9\ ml[/tex]

As it is given [tex]P_1V_1=P_2V_2[/tex]

insert the values

[tex]141\times 5=P_2\cdot 2.9\\P_2=243.10\ mm\ \text{of}\ Hg[/tex]

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