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The activation energy for the forward reaction A + B ⇔ C + D is 38 kJ and enthalpy of reaction is 20 kJ. The
activation energy for this same reaction in the reverse direction will be
activation energy for this same reaction in the reverse direction will be
- a)20 kJ
- b)38 kJ
- c)58 kJ
- d)18 kJ
Correct answer is option 'D'. Can you explain this answer?
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Most Upvoted Answer
The activation energy for the forward reaction A + B ⇔ C + D is 3...
The activation energy for a forward reaction is the minimum amount of energy required for the reactant molecules to undergo a chemical reaction and form the product molecules. It is represented by the symbol Ea.
In the reaction A → B, the activation energy would be the energy barrier that reactant A molecules must overcome in order to convert into product B molecules. This energy barrier is necessary to break the existing chemical bonds in reactant A and form new bonds in product B.
The activation energy can be thought of as the energy hill that reactant molecules need to climb over before they can proceed to form products. Once the reactant molecules have enough energy to overcome the activation energy barrier, the reaction can proceed and the products can be formed.
The activation energy can be influenced by factors such as temperature, concentration, and catalysts. Increasing the temperature generally increases the kinetic energy of the reactant molecules, making them more likely to have enough energy to overcome the activation energy barrier and proceed to form products. Similarly, increasing the concentration of reactants or using a catalyst can provide an alternative reaction pathway with a lower activation energy, making the reaction occur more easily.
Overall, the activation energy is an important concept in understanding reaction rates and the factors that influence the progress of a chemical reaction.
In the reaction A → B, the activation energy would be the energy barrier that reactant A molecules must overcome in order to convert into product B molecules. This energy barrier is necessary to break the existing chemical bonds in reactant A and form new bonds in product B.
The activation energy can be thought of as the energy hill that reactant molecules need to climb over before they can proceed to form products. Once the reactant molecules have enough energy to overcome the activation energy barrier, the reaction can proceed and the products can be formed.
The activation energy can be influenced by factors such as temperature, concentration, and catalysts. Increasing the temperature generally increases the kinetic energy of the reactant molecules, making them more likely to have enough energy to overcome the activation energy barrier and proceed to form products. Similarly, increasing the concentration of reactants or using a catalyst can provide an alternative reaction pathway with a lower activation energy, making the reaction occur more easily.
Overall, the activation energy is an important concept in understanding reaction rates and the factors that influence the progress of a chemical reaction.
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Community Answer
The activation energy for the forward reaction A + B ⇔ C + D is 3...
Activation energy for the reverse reaction will be activation energy of the forward reaction minus the enthalpy of the forward reacriin,
so that gives us
38-20= 18kJ
so that gives us
38-20= 18kJ
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The activation energy for the forward reaction A + B ⇔ C + D is 38 kJ and enthalpy of reaction is 20 kJ. Theactivation energy for this same reaction in the reverse direction will bea)20 kJb)38 kJc)58 kJd)18 kJCorrect answer is option 'D'. Can you explain this answer?
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