Questions: 25% of Matter Use the References to access important values if needed for this question. A mixture of helium and carbon dioxide gases is maintained in a 7.36 L flask at a temperature of (47^circ C). If the partial pressure of helium is (0.402) atm and the partial pressure of carbon dioxide is 0.370 atm, the total pressure in the flask is (square) atm.

25%
of Matter

Use the References to access important values if needed for this question. A mixture of helium and carbon dioxide gases is maintained in a 7.36 L flask at a temperature of (47^circ C).

If the partial pressure of helium is (0.402) atm and the partial pressure of carbon dioxide is 0.370 atm, the total pressure in the flask is (square) atm.

Transcript text: prod01-cnow-owl.cengagenow.com $25 \%$ of Matter [Review Topics] [References] Use the References to access important values if needed for this question. A mixture of helium and carbon dioxide gases is maintained in a 7.36 L flask at a temperature of $47^{\circ} \mathrm{C}$. If the partial pressure of helium is $\mathbf{0 . 4 0 2}$ atm and the partial pressure of carbon dioxide is 0.370 atm, the total pressure in the flask is $\square$ atm. Submit Answer Retry Entire Group 9 more group attempts remaining

Solution

Solution Steps

Step 1: Identify Given Data

We are given the following data:

Volume of the flask: $7.36 \, \text{L}$
Temperature: $47^{\circ} \text{C}$
Partial pressure of helium: $0.402 \, \text{atm}$
Partial pressure of carbon dioxide: $0.370 \, \text{atm}$

Step 2: Calculate the Total Pressure

The total pressure in the flask is the sum of the partial pressures of the gases present. Therefore, we add the partial pressures of helium and carbon dioxide:

\[ P_{\text{total}} = P_{\text{He}} + P_{\text{CO}_2} \]

Substituting the given values:

\[ P_{\text{total}} = 0.402 \, \text{atm} + 0.370 \, \text{atm} \]

Step 3: Perform the Addition

Adding the partial pressures:

\[ P_{\text{total}} = 0.402 + 0.370 = 0.772 \, \text{atm} \]