A mixture of H_(2) and water vapor is present in a closed vessel at 20.00^circ C The total pressure of the system is 755.0 mmHg. The partial pressure of the water vapor 17.50 mmHg. What is the partial pressure of H_(2) ? Type in your answer using the correct number of significant figures. square mmHg

To find the partial pressure of \( H_2 \) in the mixture, we can use Dalton's Law of Partial Pressures, which states that the total pressure of a gas mixture is the sum of the partial pressures of the individual gases in the mixture.<br /><br />Given:<br />- Total pressure, \( P_{\text{total}} = 755.0 \) mmHg<br />- Partial pressure of water vapor, \( P_{\text{H}_2\text{O}} = 17.50 \) mmHg<br /><br />The partial pressure of \( H_2 \) can be calculated as:<br />\[ P_{H_2} = P_{\text{total}} - P_{\text{H}_2\text{O}} \]<br /><br />Substituting the given values:<br />\[ P_{H_2} = 755.0 \, \text{mmHg} - 17.50 \, \text{mmHg} \]<br />\[ P_{H_2} = 737.5 \, \text{mmHg} \]<br /><br />Therefore, the partial pressure of \( H_2 \) is \( 737.5 \) mmHg.