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You fill a balloon with 2.50 moles of gas at 25°C at a pressure of 1.49 atm. What is the volume of the balloon?

Sagot :

You need to use the ideal gas equation: 

[tex]PV = nRT[/tex]

P is pressure (in atm or bar)

V is volume (in L)

n is the number of moles (in mol)
 
R is an experimentally determined ratio of about 0.82 

T is the temperature (in Kelvin)

Note: For all gases, you need to convert Celsius or Fahrenheit to Kelvin.

[tex] 25C + 273.15 = 298.15K [/tex]

Get V alone.

[tex] V = \frac{nRT}{P} [/tex]

Plug in the values you have.

[tex] V = \frac{2.50 mol * 0.82 * 298.15 K}{1.49 atm}[/tex]

you get:

[tex] V = 611.2075L [/tex]

A fun fact: the gas used to fill up a balloon is Helium. 
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