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The way to keep this simple is to assume that the pressure in the balloon
remains constant throughout the operation.

The only trick to this whole thing is to understand that

-- At constant pressure, volume is directly proportional to temperature.
Volume2/Volume1 = Temperature2/Temperature1
-- 'Temperature' means absolute temperature ... Kelvin, or (Celsius + 273).?
The initial temperature of 20 C is absolute temp of 293 K.

If the pressure remains constant, then

Absolute-temp2 = Absolute-temp1 x (Volume2/Volume1) = 1,000 x 293/750 = 3902/3 K.

°Celsius = Absolute - 273 = 117 2/3 ° C.




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11y ago
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1mo ago

To find the temperature at which the air must be heated to increase the volume from 750 L to 1000 L, you can use the formula (V1/T1) = (V2/T2), where V1 is the initial volume (750 L), T1 is the initial temperature (20 degrees Celsius + 273 = 293 K), V2 is the final volume (1000 L), and solve for T2. Plug these values into the formula to find the final temperature needed.

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Q: How hot must the air in a balloon be heated if initially it has a volume of 750 L at 20 degrees celsius and the final volume must be 1000 L?
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