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A 2.50 L sample of dry air in a cylinder exerts a pressure of 3.00 atm at 25 ˚C. Without changing the temperature, a piston is moved until the pressure in the cylinder is reduced to 1.00 atm. What is the final volume of the gas?

Sagot :

[tex]\tt{\huge{\red{Solution:}}}[/tex]

Step 1: List the given values

[tex]\begin{aligned} P_1 & = \text{3.00 atm} \\ V_1 & = \text{2.50 L} \\ P_2 & = \text{1.00 atm} \end{aligned}[/tex]

Final Step: Calculate the final volume using Boyle's law.

[tex]\begin{aligned} V_2 & = \frac{P_1V_1}{P_2} \\ & = \frac{(\text{3.00 atm})(\text{2.50 L})}{\text{1.00 atm}} \\ & = \boxed{\text{7.50 L}} \end{aligned}[/tex]

Hence, the final volume of the gas is 7.50 L.

[tex]\\[/tex]

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