InterviewSolution
Saved Bookmarks
InterviewSolution
| 1. |
A 10 litre flask contains 0.2 mole of methane, 0.3 mole of hydrogen and 0.4 mole of nitrogen at `25^(@)C`. What is the partial pressure of each component and what is the pressure inside the flask ? |
|
Answer» `P = (nRT)/(V)` Partial pressure of methane `= (0.2 xx 0.00821 xx 298)/(10) = 0.489 atm` Partial pressure of hydrogen `= (0.3 xx 0.0821 xx 298)/(10) = 0.734 atm` Partial pressure of nitrogen `= (0.4 xx 0.0821 xx 298)/(10) = 0.979` atm Total pressure `= (0.489 + 0.8734 + 0.979) atm` `= 2.202 atm` Alternative solution: Total number of moles `= 0.2 + 0.3 + 0.4 = 0.9` Let the total pressure be P. We know that, `P = ("total number of moles")/(V). RT` `V = 10` litre, `R = 0.0821 L atm K^(-1), T = (25 + 273) = 298 K` `+ (0.9)/(10) xx 0.0821 xx 298 = 2.20 atm` Partial pressure of `CH_(4) =` Mole fraction of methane `xx` total pressure `= (0.2)/(0.9) xx 2.20 = 0.489 atm` Partial pressure of `H_(2) =` Mole fraction of `H_(2) xx` total pressure `= (0.3)/(0.9) xx 2.20 = 0.489 atm` Partial pressure of `H_(2) =` Mole fraction of `H_(2) xx` total pressure `= (0.3)/(0.9) xx 2.20 = 0.733` atm Partial pressure of `N_(2) =` Mole fraction of `N_(2) xx` total pressure `= (0.3)/(0.9) xx 2.20 = 0.733 atm` Partial pressure of `N_(2) =` Mole fraction of `N_(2) xx` total pressure `= (0.4)/(0.9) xx 2.20 = 0.978 atm` |
|