Answered

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Swift has a 5.55mol sample of carbon dioxide. If the sample is 24.29kpa, and the volume is 525.79mL, what will the temperature of the sample be in Kelvin?

Sagot :

The first step is to convert the kPa to atm, using a conversion factor:

[tex]24.29kPa\cdot\frac{1atm}{101.325kPa}=0.24atm[/tex]

Also convert the ml to L, using a conversion factor:

[tex]525.79ml\cdot\frac{1l}{1000ml}=0.52579l[/tex]

Use the ideal gas law to find the temperature of the gas:

[tex]\begin{gathered} Pv=nRT \\ T=\frac{Pv}{nR} \end{gathered}[/tex]

Where T is the temperature, P is the pressure, v is the volume, n is the number of moles and R is the ideal gas constant (0.082atm*L/mol*K):

[tex]T=\frac{0.24atm\cdot0.52579l}{5.55mol\cdot0.082\frac{atm\cdot L}{mol\cdot K}}=0.28K[/tex]

The answer is 0.28K.

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