Answer:
Following are the solution to this question:
Explanation:
Following are the lewis structure of the 
:
In the given element two H and one N are used, in which N has 5 valance electrons, and one H has 1 valence which is equal to 2 electrons valance. So, the graph for the given element is defined in the attached file.
No a molecule is 2 different atoms bond
Through manipulation of equations, we are able to obtain the equation:
![-pOH= log [ OH^{-}]](https://tex.z-dn.net/?f=-pOH%3D%20log%20%5B%20OH%5E%7B-%7D%5D%20)
Then we can transform the equation into:
![[ OH^{-}]= 10^{-pOH}](https://tex.z-dn.net/?f=%5B%20OH%5E%7B-%7D%5D%3D%2010%5E%7B-pOH%7D%20%20)
Then we are able to plug in the pOH and directly get [OH-]:
![[ OH^{-}] = 10^{-6.48}](https://tex.z-dn.net/?f=%5B%20OH%5E%7B-%7D%5D%20%3D%2010%5E%7B-6.48%7D%20)
![[ OH^{-}]=3.31* 10^{-7} M](https://tex.z-dn.net/?f=%5B%20OH%5E%7B-%7D%5D%3D3.31%2A%2010%5E%7B-7%7D%20M%20%20)
Answer:Overall equation:
a)CO(g) + NO2(g) → CO2(g) + NO(g)
b)Each step is bimolecular
c)Rate=k[NO2]^2
d)NO3 is an intermediate
Explanation:
To obtain the overall rate equation we cancel out reactants and products that are the same on both sides of the both steps. This leaves us with CO(g) + NO2(g) → CO2(g) + NO(g) as the overall stoichiometric reaction equation. Each step involves the reaction of two molecules hence each step in the mechanism is bimolecular. The slow step involves the reaction of NO2 hence the rate of reaction depends on the first step of the reaction hence the rate equation shown in the answer. Intermediates only take part in elementary steps but do not appear as products or reactants. They are produced and consumed transiently. NO3 is an intermediate in this reaction.
