A syringe contains 610 mL of CO at 310 K and 1.5 atm pressure. A second syringe contains 520 mL of N2 at 325 K and 3.5 atm. What is the final pressure if the contents of these two syringes are injected into 2.00 L container at 10.0C
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Ответ:
P = 1.21atm
Explanation:
Using PV = nRT, moles of both syringes is:
Moles CO:
n = PV / RT
n = 1.5atm*0.610L / 0.082atmL/molK*310K
n = 0.0360 moles
Moles N₂:
n = PV / RT
n = 3.5atm*0.520L / 0.082atmL/molK*325K
n = 0.0683 moles.
As in the container you mix both gases, moles in the container are:
n = 0.0360 + 0.0683 = 0.1043 moles
Conditions of the container are:
V = 2.00L; T = 273.15K + 10°C = 283.15K; n = 0.1043 moles.
Thus, pressure is:
P = nRT / V
P = 0.1043mol*0.082atmL/molK*283.15K / 2.00L
P = 1.21atmОтвет:
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Explanation: