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Slav-nsk [51]
3 years ago
8

You have 4 moles of a gas in a 50 L container held at 2 atm pressure. Currently the temperature is 27 ºC. R = 0.0821 L*atm/(mol*

K)
• What is the temperature in Kelvins? ----- K = 27 +273.15 = 300.15
• Assuming that everything else remains constant, what will happen to the pressure if the temperature decreases to -15 ºC? ------ the pressure should decrease as well, I believe
• If you increase the number of moles to 6 moles, increase temperature to 400K and reduce the volume to 25 L, what will the new pressure be? ------- I have no idea what formula to use
Chemistry
1 answer:
Mariulka [41]3 years ago
3 0
The formula used for determining gas pressure, volume and temperature interaction would be PV=nRT. 

<span>• What is the temperature in Kelvins?
</span>You already right at this part. Kelvin temperature formula from celsius should be:
K= C+273.15= 
<span>K= 27 +273.15 = 300.15 
It is important to remember that the formula in this question is using Kelvin unit at temperature, not Celcius or Fahrenheit.
</span>
<span>• Assuming that everything else remains constant, what will happen to the pressure if the temperature decreases to -15 ºC?
</span>In this case, the temperature is decreased from 27C into -15C and you asked the change in the pressure.
Using PV=nRT formula, you can derive that the temperature will be directly related to pressure. If the temperature decreased, the pressure will be decreased too. 

<span> If you increase the number of moles to 6 moles, increase temperature to 400K and reduce the volume to 25 L, what will the new pressure be?
</span>PV=nRT
P= nRT/V
P= 6 moles* <span>0.0821 L*atm/(mol*K) * 400K/25L= 7.8816 atm</span>
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