An Ideal Gas Ocuppying A 2.0l Flask Is Allowed To Expand To A Volume Of 6.00 Ml.Calculate The Final Pressure In Atm

an ideal gas ocuppying a 2.0L flask is allowed to expand to a volume of 6.00 ml.calculate the final pressure in atm

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An ideal gas ocuppying a 2.0L flask is allowed to expand to a volume of 6.00 ml.calculate the final pressure in atm

V1 (initial volume) = 2.0 L

V2 (final volume) = 6.00 mL → 0.006 L

P1 (initial pressure) = 1 atm (in STP)

P2 (final pressure) = ? (in atm)

We have an isothermal transformation, that is, its temperature remains constant, if the volume of gas in the container decreases, then its pressure increases since it is known that pressure and volume of a gas are inversely proportional. Applying the data to the formula of Boyles Law, we have:

P_1*V_1 = P_2*V_2

1*2.0 = P_2*0.006

2.0 = 0.006\:P_2

0.006\:P_2 = 2.0

P_2 = \dfrac{2.0}{0.006}

\boxed{\boxed{P_2 \approx 333.33\:atm}}\end{array}}\qquad\checkmark

Answer:  

The final pressure is approximately 333.33 atm  

_______________________________  

I Hope this helps, greetings ... Dexteright02! =)


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