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?

Question

Quizplus · Accepted Answer

First, we need to convert the temperatures to Kelvin: 0.00°C + 273.15 = 273.15 K and 325 K. Next, we need to use the combined gas law to find the final pressure. (P1V1/T1) = (P2V2/T2) We'll use P1V1/T1 for CO and P2V2/T2 for N₂. When we combine them, we get: (P1V1/T1) + (P2V2/T2) = Pf(V1+V2)/Tf where Pf is the final pressure and Tf is the final temperature. Plugging in the values, we get: (1.2 atm x 0.589 L)/(325 K) + (2.6 atm x 0.473 L)/(298 K) = Pf(1.062 L)/(273.15 K) Solving for Pf, we get: Pf = [(1.2 atm x 0.589 L)/(325 K) + (2.6 atm x 0.473 L)/(298 K)] x (273.15 K/1.062 L) = 1.7 atm Therefore, the final pressure is 1.7 atm.

A Syringe Contains 589 ML of CO at 325 K