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

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

c. electrical charges of ionic bonds.