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 STP? A)0.59 atm B)1.1 atm C)1.7 atm D)1.9 atm E)3.8 atm

Question

Quizplus · Accepted Answer

First, we need to calculate the amount of CO and N2 gas that will be present in the 1.00 L container at STP.

For CO:
P1V1/T1 = P2V2/T2
1.2 atm x 0.589 L / 325 K = P2 x 1.00 L / 273 K
P2 = 0.433 atm

For N2:
P1V1/T1 = P2V2/T2
2.6 atm x 0.473 L / 298 K = P2 x 1.00 L / 273 K
P2 = 1.54 atm

Now we can calculate the total pressure of the mixture in the container:
Ptotal = PCO + PN2
Ptotal = 0.433 atm + 1.54 atm
Ptotal = 1.97 atm, which we can round to 1.7 atm.

Therefore, the final pressure is 1.7 atm (choice C).

A Syringe Contains 589 ML of CO at 325 K