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mash [69]
3 years ago
10

A Goodyear blimp typically contains 5400 m³ of helium (He) at an absolute pressure of 1.10 × 10 5 1.10 × 10 5 Pa. The temperatur

e of the helium is 295 K. What is the mass (in kg) of the helium in the blimp?(The molar mass of Helium is 4.0026 g)
Physics
1 answer:
Wewaii [24]3 years ago
4 0

The concept related to this exercise to solve this problem is the ideal Gas law which establishes

PV = nRT

P= Pressure

V= Volume

n = Number of moles

R= Gas ideal Constant

T= Temperature

Our values are given as,

V =5400m^3 \\P = 1.1*10^5Pa\\T = 295K \\M_m =4.0026g\\R = 8.3145J\cdot mol^{-1}K^{-1}\\

From the ideal gas equation then we rearrange the equation to obtain the number of moles, then

PV=nRT\\n = \frac{PV}{RT}\\n= 242174.43

By definition the molecular mass (n) is expressed in terms of the mass and molecular weight therefore

n = \frac{m}{M_m}

m = n*M_m

m = (242174.43)(4.0026)n

m = 969327.37

m = 968.327Kg

Therefore the mass of the helium in the blimp is 968.327Kg

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