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3 years ago

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A sample of nitrogen gas occupies a volume of 1.40L at 297K with a pressure of 776mmHg. The volume increases to 2.70L and the te

mperature decreases to 274K. What is the final pressure in atmospheres exerted on the gas?

1 answer:

konstantin123 [22]3 years ago

6 0

Hey it isnt letting me submit my answer to your question on the Japanese chart, so imma just submit it here

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If a gas occupies a volume of 950 mL at standard temperature, what volume will it

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Voulme 1= 950 mL
Volume 2= ?
Temperature 1 = 25 C
Temperature 2 = 50 C
Convert your temperature to Kelvin
C+273=K
Temperature 1 = 25 C + 273 = 298 K
Temperature 2 = 50 C + 273 = 323 K

Plug in to the Formula
950 mL/298 K = ? / 323 K

Rearrange the formula to make one to solve for what is missing.
To get 323 K out of the denominator multiply by it.
Making it
950 mL x 323 K / 298 K = ?

Plug it in
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Since water is already at 100<span>°C all the energy is used to evaporate it.
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