It's 32°F (0°C) outside under normal atmospheric conditions (1 atm) at a stunt
a
performer's birthday party. There is a huge blue balloon filled with flammable hydrogen
(H2, molar mass = 2.02 g/mol) gas that she plans to safely ignite, causing a massive
explosion. Inside the balloon is 239 g of H2(g).
What is the volume of the balloon, in liters? Round to the nearest whole number.


Its 32F 0C Outside Under Normal Atmospheric Conditions 1 Atm At A Stunt A Performers Birthday Party There Is A Huge Blue Balloon Filled With Flammable Hydrogen class=

Sagot :

The volume of the balloon is approximately 2652 liters.

How to determine the volume occupied by the gas in a balloon

Let suppose that flammable hydrogen behaves ideally. GIven the molar mass ([tex]M[/tex]), in kilograms per kilomole, and mass of the gas ([tex]m[/tex]), in kilograms. The volume occupied by the gas ([tex]V[/tex]), in cubic centimeters, is found by the equation of state for ideal gases:

[tex]V = \frac{m\cdot R_{u}\cdot T}{P\cdot M}[/tex]   (1)

Where:

  • [tex]R_{u}[/tex] - Ideal gas constant, in kilopascal-cubic meters per kilomole-Kelvin.
  • [tex]T[/tex] - Temperature, in Kelvin
  • [tex]P[/tex] - Pressure, in kilopascals

If we know that [tex]m = 0.239\,kg[/tex], [tex]R_{u} = 8.314\,\frac{kPa\cdot m^{3}}{kmol\cdot K}[/tex], [tex]T = 273.15\,K[/tex], [tex]P = 101.325\,kPa[/tex] and [tex]M = 2.02\,\frac{kg}{kmol}[/tex], then the volume of the balloon is:

[tex]V = \frac{(0.239\,kg)\cdot \left(8.314\,\frac{kPa\cdot m^{3}}{kmol\cdot K} \right)\cdot (273.15\,K)}{\left(101.325\,kPa\right)\cdot \left(2.02\,\frac{kg}{kmol} \right)}[/tex]

[tex]V = 2.652\,m^{3}[/tex] ([tex]2652\,L[/tex])

The volume of the balloon is approximately 2652 liters. [tex]\blacksquare[/tex]

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