The half-life for the first-order decomposition of is 1.3*10^-5.
If N2O4 is introduced into an evacuated flask at a pressure of 17.0 mmHg , how many seconds are required for the pressure of NO2 to reach 1.4mmHg ?
i know that the half life equation is t1/2= ln2/k which allowed me to calculate k, but i am having trouble with figuring out how the stoichiometry and pressure come into play. Since there are 2 moles of NO2 and only one mole of N2O4.
The question doesn't ask anything about NO2; only N2O4. I would ignore the NO2 since the question is about pressure of N2O4 and it will exhibit its own partial pressure independent of NO2.
did you ever solve this?? because i need help on it too