Reaction Diagrams and Collision Theory

A chemical reaction occurs when reactant particles

• are separated by great distances

• have no attractive forces between them

• convert chemical energy into nuclear energy

• collide with proper energy and proper orientation

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The energy needed to start a chemical reaction is called

• activation energy

• ionization energy

• kinetic energy

• potential energy

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As the number of effective collisions between reacting particles increases, the rate of reaction

• decreases

• increases

• remains the same

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The collision theory states that a reaction is most likely to occur when the reactant particles collide with the proper

• density and volume

• energy and orientation

• formula masses

• molecular masses

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What is required for a chemical reaction to occur?

• standard temperature and pressure

• a catalyst added to the reaction system

• effective collisions between reactant particles

• an equal number of moles of reactants and products

A short-lived structure formed during a collision is a(n)

• activated complex.

• catalyst.

• reagent.

• inhibitor.

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The minimum energy required for an effective collision is called

• energy of enthalpy.

• activation energy.

• free energy.

• kinetic energy.

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If a collision between molecules is very gentle, the molecules are

• more likely to be favorably oriented

• less likely to be favorably oriented.

• more likely to react.

• more likely to rebound without reacting.

How does the energy of the activated complex compare with the energies of reactants and products?

• It is lower than the energy of both reactants and products.

• It is lower than the energy of the reactants but higher than the energy of products.

• It is higher than the energy of reactants but lower than the energy of products.

• It is higher than the energy of both reactants and products.

Reaction enthalpy is negative for

• an endothermic reaction.

• an exothermic reaction.

• an inhibited reaction.

• a stable reaction.

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