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The gas inside of a container exerts #9 Pa# of pressure and is at a temperature of #650 ^o K#. If the temperature of the gas changes to #220 ^oC# with no change in the container's volume, what is the new pressure of the gas?

Answer 1

Charles Aeschliman

#3.046 Pa#

#(p1)/"T1"# = #(p2)/"T2"#

#(9)/"650"# = #(p2)/"220"#

#p2# = #3.046 Pa#

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Answer 2

Axel Acevedo

To find the new pressure of the gas when the temperature changes, you can use the ideal gas law equation:

[ P_1 \times V_1 / T_1 = P_2 \times V_2 / T_2 ]

Since the volume (( V )) remains constant, it cancels out from both sides of the equation. Rearranging the equation to solve for ( P_2 ), the new pressure, we get:

[ P_2 = P_1 \times \frac{T_2}{T_1} ]

Substitute the given values into the equation:

[ P_2 = 9 , \text{Pa} \times \frac{220 + 273.15}{650} ]

[ P_2 ≈ 4.395 , \text{Pa} ]

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Answer from HIX Tutor

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