Question

The diagram below represents a spontaneous reaction (deltaG degree < 0). Drag the labels to the correct bins. uncatalyzed rx'n Delta G degree standard free E of activation products reactants catalyzed rx?n

Answer 1

Concepts and reason

In energy profile diagram, if the reactants are at lower energy and products are at higher energy, then the reaction is non-spontaneous reaction. On the other hand, if the reactants are at higher energy and the products are at lower energy, then the reaction is spontaneous reaction. The energy of transition state is higher than the energy of reactants and products.

Fundamentals

Energy profile diagram is the plot of energy of the system as the reaction is going on.

If the reaction is exothermic, products have less energy than the reactants then the free energy change of the reaction is less than zero $\left( {\Delta {{\rm{G}}^o} < 0} \right)$ .

If the reaction is endothermic, reactants have less energy than the products then the free energy change of the reaction is greater than zero $\left( {\Delta {{\rm{G}}^o} > 0} \right)$ .

The horizontal portion in the left side of the curve represents the energy of reactants and the horizontal portion on the right side of the curve represents the energy of products.

The energy difference between reactants and transition state is called the activation energy.

The energy difference between reactants and products is called change in free energy of the reaction which is represented by $\Delta {{\rm{G}}^o}$ .

The blue curve represents the uncatalyzed reaction and the green curve represents the catalyzed reaction.

Drag the labels in the diagram as follows:

Ans: