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
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>
