Under certain conditions the rate of this reaction is zero order in dinitrogen monoxide with a rate constant of ·0.0080Ms−1: 2N2O(g)→2N2(g)+O2(g) Suppose a 5.0L flask is charged under these conditions with 150.mmol of dinitrogen monoxide. After how much time is there only 75.0mmol left? You may assume no other reaction is important.

Explanation:

Hello,

In this case, for the given reaction, the concentration of dinitrogen oxide is quantified as:

Considering that in molar units (M), the initial and final concentration of dinitrogen oxide are:

Now, since the rate is zeroth order in dinitrogen oxide, it depends on the rate constant only:

Thus, by integrating from the initial concentration to the final concentration:

The time finally results:

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water at room temperature is flowing through a pipe with pressure taps located 10 ft apart along one section of the pipe, which are connected to a mercury (s=13.6) manometer.