A syringe contains 589 mL of CO at 325 K and 1.2 atm pressure. A second syringe contains 473 mL of N2 at 298 K and 2.6 atm. What is the final pressure if the contents of these two syringes are injected into a 1.00 L container at 0.00°C?

1.7 atm

Explanation:

For first syringe:

Pressure = 1.2 atm

Temperature = 325 K

Volume = 589 mL = 0.589 L (1 mL = 0.001 L)

Using ideal gas equation as:

PV=nRT

where,

P is the pressure

V is the volume

n is the number of moles

T is the temperature

R is Gas constant having value = 0.0821 L. atm/K. mol

Applying the equation as:

1.2 atm * 0.589 L = n * 0.0821 L. atm/K. mol * 325 K

⇒n = 0.02649 moles

For second syringe:

Pressure = 2.6 atm

Temperature = 298 K

Volume = 473 mL = 0.473 L (1 mL = 0.001 L)

Using ideal gas equation as:

PV=nRT

Applying the equation as:

2.6 atm * 0.473 L = n * 0.0821 L. atm/K. mol * 298 K

⇒n = 0.050266 moles

Total moles = 0.02649 moles + 0.050266 moles = 0.076756 moles

Volume = 1 L

Temperature = 0.00 °C

The conversion of T (°C) to T (K) is shown below:

T (K) = T (°C) + 273.15

So,

T = (0 + 273.15) K = 273.15 K

Using ideal gas equation as:

PV=nRT

Applying the equation as:

P * 1 L = 0.076756 * 0.0821 L. atm/K. mol * 273.15 K

⇒Total P = 1.7 atm