Arubber balloon was filled with helium at 25.0˚c and placed in a beaker of liquid nitrogen at -196.0˚c. the volume of the cold helium was 15.6 cm3. assuming ideal gas behavior and isobaric conditions, what was the volume of the helium at 25.0˚c?

The volume of helium at 25.0 °C is 60.3 cm³.

Explanation:

In order to work with ideal gases we need to consider absolute temperatures (Kelvin). To convert Celsius to Kelvin we use the following expression:

K = °C + 273.15

The initial and final temperatures are:

T₁ = 25.0 + 273.15 = 298.2 K

T₂ = -196.0 + 273.15 = 77.2 K

The volume at 77.2 K is V₂ = 15.6 cm³. To calculate V₁ in isobaric conditions we can use Charle's Law.

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its first and third is your answer i did the qustion the fourth isnt right