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RoseWind [281]
3 years ago
8

You have a partially filled party balloon with 2.00 g of helium gas. you then add 2.74 g of hydrogen gas to the balloon. assumin

g constant temperature and pressure, how many times bigger is the party balloon - comparing before and after the hydrogen gas has been added?
Chemistry
1 answer:
Elanso [62]3 years ago
5 0
First, we need to get moles of He:

moles of He = mass/molar mass of He

when the molar mass of He = 4 g/mol
                     
and when the mass = 2 g 
 
by substitution:

  moles of He = 2 g / 4 g/mol 

                        = 0.5 moles

and when V = nRT/P and n is the number of moles

so, V1 = 0.5RT/P

then, we need moles of H2 = mass / molar mass 

                                               = 2.74g / 2g/mol

                                               = 1.37 moles

∴ moles of He + moles of H2 = 0.5 moles + 1.37 moles 

                                                 = 1.87 moles

so, V2= 1.87RT/P

from the V1 and V2 formula:

∴V2/V1 = 1.87 / 0.5

              = 3.74 

∴ the party balloon is 3.74 times bigger
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Calcular la presión final de un gas que inicialmente está a 21°C y 0,98 atm. Sabiendo que su temperatura aumenta a 37°C.
KatRina [158]

Answer:

1.03 atm

Explanation:

Primero <u>convertimos 21 °C y 37 °C a K</u>:

  • 21 °C + 273.16 = 294.16 K
  • 37 °C + 273.16 = 310.16 K

Una vez tenemos las temperaturas absolutas, podemos resolver este problema usando la<em> ley de Gay-Lussac</em>:

  • T₁P₂ = T₂P₁

En este caso:

  • T₁ = 294.16 K
  • P₂ = ?
  • T₂ = 310.16 K
  • P₁ = 0.98 atm

Colocando los datos:

  • 294.16 K * P₂ = 310.16 K * 0.98 atm

Y <u>despejando P₂</u>:

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