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.