00:01
So the actual rate law is rate is equal to k observed, multiplied by the concentration of n2, multiplied by the concentration of h2 squared.
00:20
So it's first order with respect to n2 and second order with respect to h2.
00:25
But if the h2 concentration is kept high so that it doesn't change, then we can write the rate law as a pseudo first order.
00:34
Rate is equal to, i'll call it k prime, multiplied by the concentration of n2, where k prime is equal to k observed, multiplied by the concentration of h2 squared.
00:52
So to determine what k observed is, that will simply be equal to k prime, divided by the concentration of h2 squared.
01:03
To get k prime, we'll use the half -life information when the h -2 concentration was set at 2 molar.
01:13
K -prime will be equal to the natural log of 2 divided by the half -life...