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If #17/6 L# of a gas at room temperature exerts a pressure of #24 kPa# on its container, what pressure will the gas exert if the container's volume changes to #5/4 L#?

Answer 1

Charles Aeschliman

#54.4kPa#

We can obtain the final pressure via Boyle's Law:

Let's identify the known and unknown variables:

#color(blue)("Knowns:")#
- Initial Volume
- Final Volume
- Initial Pressure

#color(magenta)("Unknowns:")#
- Final Pressure

All we have to do is rearrange the equation to solve for the final pressure. We do this by dividing both sides by #V_2# in order to get #P_2# by itself like this:
#P_2=(P_1xxV_1)/V_2#

Now all we do is plug in the values and we're done!

#P_2= (24kPa xx 17/6cancel"L")/(5/4\cancel"L")# = #54.4 kPa#

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Answer 2

Leo Abeyta

Use Boyle's Law to find the new pressure:

[P_1 \cdot V_1 = P_2 \cdot V_2]

[24 , \text{kPa} \cdot \frac{17}{6} , \text{L} = P_2 \cdot \frac{5}{4} , \text{L}]

[P_2 = \frac{24 , \text{kPa} \cdot \frac{17}{6} , \text{L}}{\frac{5}{4} , \text{L}}]

[P_2 \approx 163.2 , \text{kPa}]

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Answer from HIX Tutor

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