Answer:
The name of the products are CO2 = carbon dioxide and H2O = water. The type of reaction is a combustion reaction. 
Explanation:
 
        
                    
             
        
        
        
Answer: Option (d) is the correct answer.
Explanation:
Steps involved for the given reaction will be as follows.
Step 1:  (fast)
    (fast)
Rate expression for step 1 is as follows.
                Rate = k ![[NO]^{2}](https://tex.z-dn.net/?f=%5BNO%5D%5E%7B2%7D)
Step 2: 
This step 2 is a slow step. Hence, it is a rate determining step.
Step 3.  (fast)
    (fast)
Here,  is intermediate in nature.
 is intermediate in nature.
All the steps are bimolecular and it is a second order reaction. Also, there is no catalyst present in this reaction.
Thus, we can conclude that the statement step 1 is the rate determining step, concerning this mechanism is not directly supported by the information provided. 
 
        
             
        
        
        
Answer:
21.86582KJ
Explanation:
The graphical form of the Arrhenius equation is shown on the image attached. Remember that in the Arrhenius equation, we plot the rate constant against the inverse of temperature. The slope of this graph is the activation energy and its y intercept is the frequency factor.
Applying the equation if a straight line, y=mx +c, and comparing the given equation with the graphical form of the Arrhenius equation shown in the image attached, we obtain the activation energy of the reaction as shown.