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 a) 12.66 x 10^-2 mol; b) 390 a) 6.16 x 10^-2 mol; b) 495 K a) 6.16 x 10^-2 mol; b) 395 K a) 8.45 x 10^-2 mol; b) 395 K

          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

a) 12.66 x 10^-2 mol; b) 390
a) 6.16 x 10^-2 mol; b) 495 K
a) 6.16 x 10^-2 mol; b) 395 K
a) 8.45 x 10^-2 mol; b) 395 K

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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

a) 12.66 x 10^-2 mol; b) 390
a) 6.16 x 10^-2 mol; b) 495 K
a) 6.16 x 10^-2 mol; b) 395 K
a) 8.45 x 10^-2 mol; b) 395 K

Added by Earl W.

University Physics with Modern Physics

Hugh D. Young 14th Edition

Instant Answer

Solved by Expert Adi S

06/07/2022

Step 1

50 \times 10^5 \, Pa\) \(V = 1.00 \, L = 1.0 \times 10^{-3} \, m^3\) \(T = 285.65 \, K\) \(R = 8.314 \, J/(mol \cdot K)\) Substitute the values into the equation: \(n = \frac{PV}{RT} = \frac{(1.50 \times 10^5 \, Pa) \times (1.0 \times 10^{-3} \, m^3)}{(8.314 \, 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 a) 12.66 x 10^-2 mol; b) 390 a) 6.16 x 10^-2 mol; b) 495 K a) 6.16 x 10^-2 mol; b) 395 K a) 8.45 x 10^-2 mol; b) 395 K

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