Aweather balloon is inflated to a volume of 28.5 l at a pressure of 748 mmhg and a temperature of 28.0 degrees c. the balloon rises in the atmosphere to an altitude of 25,000 feet, where the pressure is 385 mmhg and the temperature is -15.0 degrees c. assuming the balloon can freely expand, calculate the volume of the balloon at this altitude.

The volume of the balloon at this altitude is 47.46 Liters.

Explanation:

Initial pressure of the gas =

Initial volume of balloon =

Initial temperature of the gas in the balloon =

Moles of gas in balloon = n

...[1]

Moles of gas will remain the same when the temperature pressure and volume conditions are altered.

Final pressure of the gas at given altitude=

Final volume of balloon at given altitude =

Final temperature of the gas in the balloon  at given altitude =

...[2]

From [1] and [2]

The volume of the balloon at this altitude is 47.46 Liters.

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explanation:

covalent bonds

consist of pairs of electrons shared by two atoms, and bind the atoms to fixed orientation and requre high energies to break them

ionic bonds

when two atoms differ considerably in their electronegativity, then one of the atoms will lose its electron to the other atom. this results in a positively charged ion(cation) and a negatively charged ion (anion)

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