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17) (18 points total) Pure Nitrogen gas is contained within a piston as shown to the right. The gas is initially at a pressure of 110,000 Pa (absolute), a volume of 0.10 m$^3$, and a temperature of 900. K. The end of the piston has an area of 0.3 m$^2$. $k_B = 1.38 \cdot 10^{-23} \frac{J}{K}$ $R = 8.314 \frac{J}{mol \cdot K}$ $m_{N_2} = 4.65 \cdot 10^{-26} \frac{kg}{molecule}$ (a) Determine the number of molecules present in the cylinder. (b) Determine the rms speed at 900 K (c) Determine the gauge pressure in the cylinder (1 atm = 101,325 Pa). (d) How much force would be required to compress the cylinder? (Hint use the gauge pressure since the atmosphere will help push.) (e) Determine the work the cylinder if it expands to 0.17 m$^3$ at constant pressure. (f) Determine the final temperature of the gas. Answers:

          17) (18 points total) Pure Nitrogen gas is contained within a piston as shown to the right. The gas is initially at a pressure of 110,000 Pa (absolute), a volume of 0.10 m$^3$, and a temperature of 900. K. The end of the piston has an area of 0.3 m$^2$.
$k_B = 1.38 \cdot 10^{-23} \frac{J}{K}$ 
$R = 8.314 \frac{J}{mol \cdot K}$
$m_{N_2} = 4.65 \cdot 10^{-26} \frac{kg}{molecule}$
(a) Determine the number of molecules present in the cylinder.
(b) Determine the rms speed at 900 K
(c) Determine the gauge pressure in the cylinder (1 atm = 101,325 Pa).
(d) How much force would be required to compress the cylinder?
(Hint use the gauge pressure since the atmosphere will help push.)
(e) Determine the work the cylinder if it expands to 0.17 m$^3$ at constant pressure.
(f) Determine the final temperature of the gas.
Answers:

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17) (18 points total) Pure Nitrogen gas is contained within a piston as shown to the right. The gas is initially at a pressure of 110,000 Pa (absolute), a volume of 0.10 m^3, and a temperature of 900. K. The end of the piston has an area of 0.3 m^2.
kB = 1.38 · 10^-23(J)/(K)
R = 8.314 (J)/(mol · K)
mN2 = 4.65 · 10^-26(kg)/(molecule)
(a) Determine the number of molecules present in the cylinder.
(b) Determine the rms speed at 900 K
(c) Determine the gauge pressure in the cylinder (1 atm = 101,325 Pa).
(d) How much force would be required to compress the cylinder?
(Hint use the gauge pressure since the atmosphere will help push.)
(e) Determine the work the cylinder if it expands to 0.17 m^3 at constant pressure.
(f) Determine the final temperature of the gas.
Answers:

Added by Joshua T.

University Physics with Modern Physics

Hugh D. Young 14th Edition

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Solved by Expert Cyra Jelle Calleja

05/25/2022

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Given: Pressure (P) = 110,000 Pa Volume (V) = 0.10 m^3 Temperature (T) = 900 K Gas constant (R) = 8.314 J/(mol*K) Molecular mass of N2 (m_N2) = 4.65*10^(-26) kg/molecule Using the ideal gas law equation: PV = nRT, where n is the number of moles, we can rearrange Show more…

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(18 points total) Pure Nitrogen gas is contained within a piston as shown to the right. The gas is initially at a pressure of 110,000Pa (absolute), a volume of 0.10m^(3), and a temperature of 900. K. The end of the piston has an area of 0.3m^(2). k_(B)=1.38*10^(-23)(J)/(K),R=8.314(J)/(mol*K),m_(N_(2))=4.65*10^(-26)(kg)/( molecule ) (a) Determine the number of molecules present in the cylinder. (b) Determine the rms speed at 900K (c) Determine the gauge pressure in the cylinder ( 1atm=101,325Pa. (d) How much force would be required to compress the cylinder? (Hint use the gauge pressure since the atmosphere will help push.) (e) Determine the work the cylinder if it expands to 0.17m^(3) at constant pressure. (f) Determine the final temperature of the gas. Answers: kg kB=1.38.10-23 K R=8.314 mol-K mN=4.65.10-26 molecule (a) Determine the number of molecules present in the cylinder. (b) Determine the rms speed at 900 K (c) Determine the gauge pressure in the cylinder (1 atm = 101,325 Pa). (d) How much force would be reguired to compress the cylinder? (Hint use the gauge pressure since the atmosphere will help push.) (e) Determine the work the cylinder if it expands to 0.17 m3 at constant pressure. (f) Determine the final temperature of the gas. Answers:

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