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A monatomic ideal gas initially fills a container of volume V = 0.25 m3 at an initial pressure of P = 250 kPa and temperature T = 275 K. The gas undergoes an isobaric expansion to V2 = 0.55 m3 and then an isovolumetric heating to P2 = 760 kPa.

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Answer:

number of moles = 27.34 moles

the temperature of gas after it undergoes the isobaric expansion = 605 K

Explanation:

Given that:

V = 0.25 m³

P = 250 kPa

T = 275 K

V₂ = 0.55 m³

P₂ = 760 kPa

a)

Using ideal gas equation ; PV = nRT

[tex]n = \frac{PV}{RT}\\\\n = \frac{250*10^3*0.25}{8.314*275}\\\\n = \frac{62500}{2286.35}\\\\n = 27.34 \ moles[/tex]

b) To calculate the temperature of gas after it undergoes the isobaric expansion; we have:

  1. [tex]\frac{V_1}{T_1}= \frac{V_2}{T_2}\\\\\frac{0.25}{275}= \frac{0.55}{T_2}\\\\T_2=\frac{0.55*275}{0.25}\\\\T_2 = 605 K[/tex]

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