Ideal Gas Law Calculation for Final Pressure

What is the final pressure when the contents of two syringes are injected into a 1.00 L container at 0.00°C?

Given data: Syringe 1: - CO volume: 589 mL - Temperature: 325 K - Pressure: 1.2 atm Syringe 2: - N2 volume: 473 mL - Temperature: 298 K - Pressure: 2.6 atm Container: - Volume: 1.00 L - Temperature: 0.00°C

Answer:

The final pressure when the contents of the two syringes are mixed is 1.7 atm.

To calculate the final pressure, we first need to determine the number of moles for each gas using the ideal gas law equation PV = nRT. By converting temperatures to Kelvin and following the steps outlined in the gas law equation, we can find the total moles of gas and use this information, along with the volume and temperature of the container, to calculate the final pressure.

Starting with the first syringe containing CO, we use P₁V₁ = n₁RT₁ to find the moles of CO. Then, we repeat the same process for the second syringe containing N2. By adding the moles of CO and N2 together, we get the total moles of gas. Finally, we can calculate the final pressure using the total moles, volume, and temperature of the container in the ideal gas law equation.

By following these steps and substituting the given values, we arrive at a final pressure of 1.7 atm when the contents of the two syringes are injected into a 1.00 L container at 0.00°C.