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Use the ideal gas law to calculate the pressure in atmospheres of 0.214 mol of Helium (He) at 61°C & occupying 2.53 L. You must show all of your work to earn credit. **Don't forget to convert your Celsius temperature to Kelvin. ** (4 points)

Respuesta :

skyluke89

The pressure of the gas is 2.32 atm

Explanation:

We can solve this problem by using the equation of state for ideal gases:

[tex]pV=nRT[/tex]

where:

p is the gas pressure

V is the gas volume

n is the number of moles

R is the gas constant

T is the absolute temperature

For the Helium gas in this problem, we have:

n = 0.214 mol

V = 2.53 L is the volume

[tex]R=0.082 atmL/mol K[/tex] is the gas constant

[tex]T=61^{\circ}+273=334 K[/tex] is the absolute temperature

Solving for p,

[tex]p=\frac{nRT}{V}=\frac{(0.214)(0.082)(334)}{2.53}=2.32 atm[/tex]

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