A syringe contains CO and N2: What is the final pressure when injected into a container?
What is the final pressure if the contents of two syringes, one containing 610 mL of CO at 310 K and 1.5 atm, and the other containing 520 mL of N2 at 325 K and 3.5 atm, are injected into a 2.00 L container at 10.0C?
P = 1.21 atm
Explanation:
Using the ideal gas law equation PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature, we can calculate the final pressure when the contents of the two syringes are mixed in a 2.00 L container at 10.0C.
Moles Calculation:
Moles of CO:
n = PV / RT
n = 1.5 atm * 0.610 L / (0.082 atmL/molK * 310 K)
n = 0.0360 moles
Moles of N2:
n = PV / RT
n = 3.5 atm * 0.520 L / (0.082 atmL/molK * 325 K)
n = 0.0683 moles
When the gases are mixed in the container, the total moles in the container are:
n = 0.0360 + 0.0683 = 0.1043 moles
Conditions in the Container:
V = 2.00 L
T = 273.15 K + 10°C = 283.15 K
n = 0.1043 moles
Substitute the values into the ideal gas law equation to find the final pressure:
P = nRT / V
P = 0.1043 mol * 0.082 atmL/molK * 283.15 K / 2.00 L
P = 1.21 atm
Therefore, the final pressure in the container when the contents of the two syringes are injected is 1.21 atm.