A proposed mechanism for the reaction of NO2 and CO is
1 answer:
Answer:
a.
1. NO2(g): Reactant.
2. CO(g): Reactant.
3. NO3(g): Intermediate.
4. CO2(g): Product.
5. NO(g): Product.
b. See attached picture.
Explanation:
Hello,
a. In this case, given the reactions, we can identify each species as:
1. NO2(g): Reactant because it remains at the left side in the overall reaction.
2. CO(g): Reactant because it remains at the left side in the overall reaction.
3. NO3(g): Intermediate because it is a product in the step 1 and a reactant in step 2, for that reason it is not present in the overall reaction.
4. CO2(g): Product because it remains at the right side in the overall reaction.
5. NO(g): Product because it remains at the right side in the overall reaction.
b. In this case, given that the first step is slow and endothermic, it has a high activation energy and the products will have more energy than the reactants, for that reason the final energy is above the initial point. Moreover, since the second step is fast and exothermic, it has a low activation energy and the products will have less energy than the reactants, for that reason, the reaction coordinate diagram is shown on the attached file.
Regards.
You might be interested in
Answer : The work, heat during the process and the change of entropy of the gas are, 0 J, 3333.003 J and -10 J respectively.
Explanation :
(a) At constant volume condition the entropy change of the gas is:
We know that,
The relation between the for an ideal gas are :
As we are given :
Now we have to calculate the entropy change of the gas.
(b) As we know that, the work done for isochoric (constant volume) is equal to zero.
(C) Heat during the process will be,
Therefore, the work, heat during the process and the change of entropy of the gas are, 0 J, 3333.003 J and -10 J respectively.