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Gases have three characteristic properties:
(1) they are easy to compress,
(2) they expand to fill<span> their containers, and
(3) they occupy far more space than the liquids or solids from which they form.</span>
Answer:
- Question 1: You cannot make sure the ballon will not burst before it reaches 3,000m altitude because the volume will exceed 47.0 liters
Explanation:
<u>1. Data</u>
- Maximum volume of the balloon: 47.0 liters
At 3,000 m:
- Temperature at 3,000 m, T₁: 6.0ºC
- Pressure at 3,000m, P₁: 0.565atm
At ground:
- Temperature at ground, T₂: 20ºC
- Pressure at ground, P₂: 765mmHg
- Volume at ground, V₂: 30.0 liters
Questions:
- Will the balloon's volume be more than 47.0 liter?
- Amount in grams of helium in the ballon:?
<u>2. Unit conversions:</u>
a) Convert P₂ to atm:
- P₂ = 765mmHg × 1 atm/760.0mmHg = 1.00657895atm
b) Convert the temperatures to kelvin:
- T₁ = 6.0 + 273.15 = 279.15K
- T₂ = 20 + 273.15 = 293.15K
<u>3. Solution</u>
Question 1.
<u>Calculate the final volume of the balloon:</u>
Since the number of moles of helium gas inside the balloon remains unchanged, pV = nRT yields the combined gas law:
From which you can solve for V₁ and compute it:
Then, the volume of the balloon will exceed the gurantee of the manufacturer.
Question 2.
<u>a) Calculate the number of moles of helium</u>
<u>b) Calculate the mass in grams of helium</u>
<u />
Use the atomic mass of helium: 4.003g/mol
- mass = number of moles × molar mass
- mass = 1.2558mol × 4.003g/mol = 5.02g
Rounding to 2 significant figures: 5.0g