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A 155.0 −L helium tank contains pure helium at a pressure of 1835 psi and a temperature of 298 K. How many 3.5−L helium balloons can be filled from the helium in the tank? (Assume an atmospheric pressure of 1.0 atm and a temperature of 298 K.)

Respuesta :

Answer:

5528 balloons

Explanation:

Explanation:

At constant pressure and number of moles, using Boyle's law  

[tex]{P_1}\times {V_1}={P_2}\times {V_2}[/tex]

Given ,  

V₁ = 155.0 L  

V₂ = ?

P₁ = 1835 psi

P₂ = 1 atm  = 14.7 psia

Using above equation as:

[tex]{P_1}\times {V_1}={P_2}\times {V_2}[/tex]

[tex]{1835}\times {155.0}={14.7}\times {V_2}[/tex]

[tex]{V_2}=\frac{{1835}\times {155.0}}{14.7}\ L[/tex]

[tex]{V_2}=19348.64\ L[/tex]

Volume of each balloon = 3.5 L

Thus, number of balloons, [tex]n=\frac{19348.64\ L}{3.5\ L}=5528\ balloons[/tex]

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