The balanced equation below shows the products that are formed when butane (C4H10) is combusted. 2C4H10 + 13O2 mc009-1.jpg 8CO2
2 answers:
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<u>Answer:</u>
<u>For A:</u> The for the given reaction is
<u>For B:</u> The for the given reaction is 1642.
<u>Explanation:</u>
The given chemical reaction follows:
- <u>For A:</u>
The expression of for the above reaction follows:
We are given:
Putting values in above equation, we get:
Hence, the for the given reaction is
- <u>For B:</u>
Relation of with
is given by the formula:
where,
= equilibrium constant in terms of partial pressure =
= equilibrium constant in terms of concentration = ?
R = Gas constant =
T = temperature = 500 K
= change in number of moles of gas particles =
Putting values in above equation, we get:
Hence, the for the given reaction is 1642.
Answer:
See explanation
Explanation:
The reaction that we are considering here is quite a knotty reaction. It is difficult to decide if the mechanism is actually E1 or E2 since both are equally probable based on the mass of scientific evidence regarding this reaction. However, we can easily assume that the methylenecyclohexane was formed by an E1 mechanism.
Looking at the products, one could convincingly assert that the reaction leading to the formation of the two main products proceeds via an E1 mechanism with the formation of a carbocation intermediate as has been shown in mechanism attached to this answer. Possible rearrangement of the carbocation yields the 3-methylcyclohexene product.
