What is the value of the activation energy of the uncatalyzed reaction? Express your answer to three significant figures and inc
lude the appropriate units.
2 answers:
Answer:
175KJ
Explanation:
I will assume the diagram is as in the attachment I’ve supplied herein.
Activation energy is the minimum energy required by reactant particles for a chemical reaction to occur. Depending on reaction conditions, especially for reversible reactions, reactants can become products and vice versa.
Activation energy for a forward reaction = energy of the activated complex (transition state) – energy of the reactants.
Activation energy for a reverse reaction = energy of the activated complex – energy of the products.
For the forward reaction above, reading the values from the diagram,
Activation energy = energy of the activated complex –energy of the reactants
Activation energy = (400 – 225)KJ = 175KJ
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Answer : It takes less amount of heat to metal 1.0 Kg of ice.
Solution :
The process involved in this problem are :
Now we have to calculate the amount of heat released or absorbed in both processes.
<u>For process 1 :</u>
where,
= amount of heat absorbed = ?
m = mass of water or ice = 1.0 Kg
= enthalpy change for fusion =
Now put all the given values in , we get:
<u>For process 2 :</u>
where,
= amount of heat absorbed = ?
m = mass of water = 1.0 Kg
= specific heat of liquid water =
= initial temperature =
= final temperature =
Now put all the given values in , we get:
From this we conclude that, that means it takes less amount of heat to metal 1.0 Kg of ice.
Hence, the it takes less amount of heat to metal 1.0 Kg of ice.