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How many molecules of carbon dioxide are in a balloon full of carbon dioxide with a volume of 6.91 liters at STP?​

User Foal
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Answer: 1.855 x 10^23

At STP (Standard Temperature and Pressure), 1 mole of any gas occupies 22.4 liters of volume.

Therefore, the number of moles of carbon dioxide in the balloon can be calculated as:

moles of CO2 = volume of balloon / 22.4

moles of CO2 = 6.91 / 22.4

moles of CO2 = 0.308

Now, we can use Avogadro's number to convert moles to molecules.

1 mole of any substance contains 6.02 x 10^23 molecules.

Therefore, the number of molecules of CO2 in the balloon is:

number of molecules = moles of CO2 x Avogadro's number

number of molecules = 0.308 x 6.02 x 10^23

number of molecules = 1.855 x 10^23

Therefore, there are approximately 1.855 x 10^23 molecules of carbon dioxide in the balloon at STP.
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