A rate law in this form is said to be of the fourth order.

这种形式的速率定律被称为四阶速率定律。

So in the rate law this can be expressed be the concentration being raised to the power of 1.

所以在速率定律中，这可以表示为浓度提高到 1 的次方。

The exponents in rate laws are tricky even for professional chemists and engineers because like I said they can only be determined experimentally.

即使对于专业化学家和工程师来说，速率定律中的指数也很棘手，因为就像我说的那样，它们只能通过实验来确定。

The rate law for a reaction is written like this: The rate equals a constant, k, times the concentrations of each reactant, raised to some power.

反应的速率定律是这样写的：速率等于常数 k 乘以每种反应物的浓度，提高到某个幂。

The forward rate law if k multiplied by the concentration of A raised to some power times the initial concentration of B raised to some power.

如果 k 乘以 A 的某个幂的浓度乘以 B 的初始浓度的某个幂，则正向速率定律。

The rate law for our nitric oxide reaction then ends up as k times the nitric oxide concentration raised to some power, times the hydrogen concentration also raised to some power.

然后，我们的一氧化氮反应的速率定律最终为 k 乘以一氧化氮浓度的某个幂，乘以氢气浓度的某个幂。

So if we were to find the reverse rate law for a reaction it would take the same form as the forward one, but using the initial concentrations for the products rather than the reactants.

因此，如果我们要找到反应的反向速率定律，它将采用与正向速率相同的形式，但使用产物而不是反应物的初始浓度。

This means that the final rate law for this reaction is: k times the concentration of hydrogen gas to the first power, you need to write out the 1 obviously, times the concentration of nitric oxide cubed.

这意味着这个反应的最终速率定律是：k乘以氢气浓度的一次方，显然你需要写出1乘以一氧化氮浓度的立方。