Question

An ideal gas at 54.5°F and a pressure of 1.50 x 10^5 Pa is in a container having a volume of 1.00 L. (a) Determine the number of moles of gas in the container. (b) The gas pushes against a piston, expanding to twice its original volume, while the pressure falls to atmospheric pressure. Find the final temperature. Note: 1 L = 1.0 x 10^-3 m^3

          An ideal gas at 54.5°F and a pressure of 1.50 x 10^5 Pa is in a container
having a volume of 1.00 L.

(a) Determine the number of moles of gas in the container.

(b) The gas pushes against a piston, expanding to twice its original volume,
while the pressure falls to atmospheric pressure. Find the final temperature.

Note: 1 L = 1.0 x 10^-3 m^3

An ideal gas at 54.5°F and a pressure of 1.50 x 10^5 Pa is in a container
having a volume of 1.00 L.

(a) Determine the number of moles of gas in the container.

(b) The gas pushes against a piston, expanding to twice its original volume,
while the pressure falls to atmospheric pressure. Find the final temperature.

Note: 1 L = 1.0 x 10^-3 m^3

Added by Martin H.

University Physics with Modern Physics

Hugh D. Young 14th Edition

Instant Answer

Solved by Expert Krishna G

03/01/2022

Step 1

\(T(K) = (54.5 - 32) \times \frac{5}{9} + 273.15\) \(T(K) = 22.5 \times \frac{5}{9} + 273.15\) \(T(K) = 12.5 + 273.15\) \(T(K) = 285.65 K\) Show more…

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An ideal gas at 54.5°F and a pressure of 1.50 x 10^5 Pa is in a container having a volume of 1.00 L. (a) Determine the number of moles of gas in the container. (b) The gas pushes against a piston, expanding to twice its original volume while the pressure falls to atmospheric pressure. Find the final temperature. Note: 1 L = 1.0 x 10^-3 m^3.