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

Question

Quizplus · Accepted Answer

First, we need to calculate the number of moles for each gas using the ideal gas law: PV = nRT For CO at 325 K and 1.2 bar: nCO = (1.2 bar * 0.589 L) / (0.08206 L·atm/mol·K * 325 K) = 0.0283 mol For N₂ at 298 K and 2.6 bar: nN₂ = (2.6 bar * 0.473 L) / (0.08206 L·atm/mol·K * 298 K) = 0.0540 mol The total number of moles is therefore: ntotal = nCO + nN₂ = 0.0823 mol Next, we can use the ideal gas law to calculate the final pressure at STP (0°C and 1 atm) with a volume of 1.00 L: PtotalV = ntotalRT Ptotal = (ntotal * R * 273.15 K) / 1 L Ptotal = (0.0823 mol * 0.08206 L·atm/mol·K * 273.15 K) / 1 L Ptotal = 1.68 bar ≈ 1.7 bar Therefore, the answer is (C) 1.7 bar.

A Syringe Contains 589 ML of CO at 325 K