A reaction represented by the equation 3O2 (g)? 2O3 (g) was studied at a specifi

Question

A reaction represented by the equation
            3O2 (g)? 2O3 (g)
        was studied at a specifictemperature and the following data were collected:
        time(seconds)        total pressure(atm)
        0    1.000
        46.89   0.9500
        98.82   0.9033
        137.9   0.8733
        200.0   0.8333
        286.9   0.7900
        337.9   0.7700
        511.3   0.7233
   Which is the rate law for this reaction?
    Which is the value of the rate constant?


I have no idea on how to do this does anyone know?

Explanation / Answer

You don't really need T and V. You can just use the stoichiometry of the reaction to find moles of O2 remaining. For each mole of O2 that reacts, you form 2/3rds mol (0.667 mol) of O3. You start with 1 mol of O2, so when the reaction is done, you will have 0.667 mol of O3. Use this to find the number of moles of O2 reacted at each time point. For example:

At t = 46.89s, mol O2 reacted = (1 - 0.95)/(1 - 0.667).

That allows you to find mol of O2 remaining at each point.

To find the rate law, you next need the reaction order. If you plot natural log of mol O2 remaining vs. t, I think you will find a straight line. This should tell you the reaction order. From that, you can find the rate law.

Related Questions

Navigate

• Browse (All)
• Browse A
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.