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aliina [53]
3 years ago
7

What is the pressure of 2.50 moles of an ideal gas if it has a volume of 50.0 liters when the temperature is 300.0 K

Chemistry
1 answer:
Ierofanga [76]3 years ago
7 0
Start with the ideal gas equation, <span><span><span>PV=nRT</span> </span><span>PV=nRT</span></span> and rearrange for pressure to get <span><span><span>p=<span><span>nRT</span>V </span></span> </span><span>p=<span><span>nRT</span>V</span></span></span> . You have all the necessary variables in their proper units, so plug em' into the equation to solve for pressure in units of atmospheres.

<span><span><span>P=<span><span>(2.5 mol)(300 K)(0.08206 L atm <span><span>K </span><span><span>−1</span> </span></span> mo<span><span>l </span><span><span>−1</span> </span></span></span><span>50.0 L</span> </span>=1.23 atm</span> </span><span>P=<span><span>(2.5 mol)(300 K)(0.08206 L atm <span>K<span>−1</span></span> mo<span>l<span>−1</span></span></span><span>50.0 L</span></span>=1.23 atm</span></span>

All that needs to be done now is converting atmospheres to mm <span><span><span>Hg</span> </span><span>Hg</span></span> .

<span><span><span>1.23 atm∗<span><span>760 mm Hg</span><span>1 atm</span> </span>=935 mm Hg</span> </span><span>1.23 atm∗<span><span>760 mm Hg</span><span>1 atm</span></span>=935 mm Hg</span></span> .

That value makes sense, since the original pressure in atmospheres was above 1, the pressure in mm <span><span><span>Hg</span> </span><span>Hg</span></span> will be above 760.
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Using the combined gas law equation as follows;

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