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Using Ideal Gas Laws for gases not at STP

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by

Shane Sampson

on 24 May 2016

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Transcript of Using Ideal Gas Laws for gases not at STP

For gases not at STP (Not at 1 Atm or 273 Kelvin), you are going to want to use the ideal gas law and stoichiometry to solve. The ideal gas law which is PV=nRT includes the pressure (P), volume (V), number of moles (n), the gas constant (R) which is .0821 liters x atm/moles x kelvin, and the temperature (T) of a gas molecule.
Example #2
If you are given 5.0 liters of NO at 50 degrees Celsius and .85 atm, how many moles of NO are there?
Example #2
If you are given 5.0 liters of NO at 50 degrees Celsius and .85 atm, how many moles of NO are there?
Still Need Help?
If you still need help or want extra practice, visit the either of the videos below:
Example #1
If you were given a water vapor at 40 degrees Celsius and 1.2 atm produced by the decomposition of 25 grams NaOH, find the volume of the water vapor in liters.
Example #1
2NaOH (s) -->Na O (s) + H O (g)
Using Ideal Gas Laws for gases not at STP
Shane Sampson
Ideal Gas Law
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First, use stoichiometry to find the n value, amount of moles, of the gas.
If you were given a water vapor at 40 degrees Celsius and 1.2 atm produced by the decomposition of 25 grams NaOH, find the volume of the water vapor in liters.
2NaOH (s) -->Na O (s) + H O (g)
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Example #1
If you were given a water vapor at 40 degrees Celsius and 1.2 atm produced by the decomposition of 25 grams NaOH, find the volume of the water vapor in liters.
Next, plug in your new mole value of 0.31 moles into the ideal gas law and solve for the volume in liters.
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First, plug all your known values into the ideal gas law equation and convert the Celsius into Kelvin.
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Then, set your equation equal to moles (n) and solve.
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