Four balloons, each with a mass of 10.0 g, are inflated to a volume of 20.0 L, e

Question

Four balloons, each with a mass of 10.0 g, are inflated to a volume of 20.0 L, each with a different gas: helium, neon, carbon monoxide, or nitrogen monoxide. If the temperature is 25.0°C and the atmospheric pressure is1.00 atm, what is the density of each filled balloon? Number Number Helium = Neon = 1.63x 10g/mL 8.24x 10g/mL Number Number Carbon monoxide= Nitrogen monoxide- 122x 103g/mL | | 1.22 x 103 | g/ nn L | | 1.14 x 103 In Did you account for the mass that each balloon contributes to the total density? If the density of air at 25°C and 1.00 atm is 0.00117 g/mL, will any of the balloons float in this air? Nitrogen monoxide Carbon monoxide Helium

Explanation / Answer

d = PM/RT

n / v = P / (RT)

density = (molecular weight) (P / (RT))

here T= 25 C = 298 K , R = 0.08206 L-atm/mol- K

P =1.00 atm

V= 20.0 L

For He;

Molar mass of He = 4.002 g/ mole

density = (4.002) (1.00 / (0.08206*298))

= 0.164 g/ L

= 1.64*10^-4 g/ ml

For Ne;

Molar mass of Ne = 20.18 g/ mole

density = (20.18) (1.00 / (0.08206*298))

= 0.825 g/ L

= 8.25*10^-4 g/ ml

For CO;

Molar mass of CO = 28.01 g/ mole

density = (28.01) (1.00 / (0.08206*298))

= 1.15 g/ L

= 1.15*10^-3 g/ ml

For NO;

Molar mass of NO = 30.01 g/ mole

density = (30.01) (1.00 / (0.08206*298))

= 1.23 g/ L

= 1.23*10^-3 g/ ml

The density of He and Ne is less than AIR thus both are floating in air

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