4. What is the total pressure of a gas containing a mixture with N_(2) with a partial pressure of 2.4 kPa and Cl_(2) with a partial pressure of 7.9 kPa? square square square square .square square square

To find the total pressure of a gas 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 each individual gas in the mixture.<br /><br />Given:<br />- Partial pressure of \( N_2 \) = 2.4 kPa<br />- Partial pressure of \( Cl_2 \) = 7.9 kPa<br /><br />The total pressure \( P_{total} \) is calculated as follows:<br /><br />\[ P_{total} = P_{N_2} + P_{Cl_2} \]<br /><br />Substituting the given values:<br /><br />\[ P_{total} = 2.4 \, \text{kPa} + 7.9 \, \text{kPa} \]<br /><br />\[ P_{total} = 10.3 \, \text{kPa} \]<br /><br />Therefore, the total pressure of the gas mixture is \( 10.3 \, \text{kPa} \).