Questions: Water vapor is added to a cylinder containing 0.39 atm of nitrogen and 0.19 atm of oxygen to give a total pressure of 0.94 atm of gas. What is the partial pressure of each gas in the final mixture? Be sure each of your answer entries has the correct number of significant figures. Part 1 of 3 PN2= atm Part 2 of 3 PO2= atm Part 3 of 3 PH2O= atm

Water vapor is added to a cylinder containing 0.39 atm of nitrogen and 0.19 atm of oxygen to give a total pressure of 0.94 atm of gas. What is the partial pressure of each gas in the final mixture? Be sure each of your answer entries has the correct number of significant figures.

Part 1 of 3
PN2= atm

Part 2 of 3
PO2= atm

Part 3 of 3
PH2O= atm

Transcript text: Water vapor is added to a cylinder containing 0.39 atm of nitrogen and 0.19 atm of oxygen to give a total pressure of 0.94 atm of gas. What is the partial pressure of each gas in the final mixture? Be sure each of your answer entries has the correct number of significant figures. Part 1 of 3 $P_{\mathrm{N}_{2}}=\square$ atm Part 2 of 3 $P_{\mathrm{O}_{2}}=$ atm Part 3 of 3 $P_{\mathrm{H}_{2} \mathrm{O}}=\square \mathrm{atm}$

Solution

Solution Steps

Step 1: Identify Initial Partial Pressures

We are given the initial partial pressures of nitrogen ($ \mathrm{N}_2 $) and oxygen ($ \mathrm{O}_2 $) in the cylinder:

$ P_{\mathrm{N}_2} = 0.39 $ atm
$ P_{\mathrm{O}_2} = 0.19 $ atm

Step 2: Determine Total Final Pressure

The total final pressure after adding water vapor is given as:

$ P_{\text{total}} = 0.94 $ atm

Step 3: Calculate Partial Pressure of Water Vapor

The partial pressure of water vapor ($ P_{\mathrm{H}_2\mathrm{O}} $) can be found by subtracting the sum of the initial partial pressures of nitrogen and oxygen from the total final pressure: \[ P_{\mathrm{H}_2\mathrm{O}} = P_{\text{total}} - (P_{\mathrm{N}_2} + P_{\mathrm{O}_2}) \] \[ P_{\mathrm{H}_2\mathrm{O}} = 0.94 \, \text{atm} - (0.39 \, \text{atm} + 0.19 \, \text{atm}) \] \[ P_{\mathrm{H}_2\mathrm{O}} = 0.94 \, \text{atm} - 0.58 \, \text{atm} \] \[ P_{\mathrm{H}_2\mathrm{O}} = 0.36 \, \text{atm} \]

Final Answer

\[ \boxed{P_{\mathrm{N}_2} = 0.39 \, \text{atm}} \] \[ \boxed{P_{\mathrm{O}_2} = 0.19 \, \text{atm}} \] \[ \boxed{P_{\mathrm{H}_2\mathrm{O}} = 0.36 \, \text{atm}} \]

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