The pressure is about 2.13 atm
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Further explanation
The Ideal Gas Law that needs to be recalled is:
[tex]\large {\boxed {PV = nRT} }[/tex]
P = Pressure (Pa)
V = Volume (m³)
n = number of moles (moles)
R = Gas Constant (8.314 J/mol K)
T = Absolute Temperature (K)
Let us now tackle the problem !
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Given:
initial pressure = P₁ = 2.00 atm
initial temperature = T₁ = 30 + 273 = 303 K
final temperature = T₂ = 50 + 273 = 323 K
Unknown:
final pressure = P₂ = ?
Solution:
We will use ideal gas law as follows:
[tex]\frac{P_1V_1}{T_1} = \frac{P_2V_2}{T_2}[/tex]
[tex]\frac{P_1V}{T_1} = \frac{P_2V}{T_2}[/tex]
[tex]\frac{P_1}{T_1} = \frac{P_2}{T_2}[/tex]
[tex]\frac{2.00}{303} = \frac{P_2}{323}[/tex]
[tex]P_2 = \frac{323}{303} \times 2.00[/tex]
[tex]P_2 \approx 2.13 \texttt{ atm}[/tex]
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Learn more
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Answer details
Grade: High School
Subject: Physics
Chapter: Pressure
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Keywords: Gravity , Unit , Magnitude , Attraction , Distance , Mass , Newton , Law , Gravitational , Constant , Liquid , Pressure, Ideal , Gas , Volume , Temperature
