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(a)
Interpretation:
On increasing the concentration of the reactant, the average energy of collision increases or not is to be identified.
(b)
Interpretation:
On increasing the concentration of reactant, the collision frequency increases or not is to be identified.
(c)
Interpretation:
On increasing the concentration of reactant, the fraction of collisions with proper molecular orientation increases or not is to be identified.
Explanation:
With an increase in the concentration of reactant, the number of molecules colliding increases and the space between these molecules decreases. Hence, the possibility of molecules colliding increases, which leads to an increase in the collision frequency. However, there is no increase in the fraction of molecules with proper orientation because there is no increase in the kinetic energy or temperature.
(d)
Interpretation:
On increasing the concentration of reactant, the fraction of collision with sufficient energy increases or not is to be identified.
Explanation:
With an increase in the concentration of reactant, the number of molecules colliding increases and the space between these molecules decreases. Hence, the possibility of molecules colliding increases. As the collision increases, the energy of molecules increases and molecules start colliding with sufficient energy to overcome the activation energy.
(e)
Interpretation:
On increasing the concentration of reactant, the reaction rate increases or not is to be identified.
Explanation:
With an increase in the concentration of reactant, the number of molecules colliding increases and the space between these molecules decreases. Hence, the possibility of molecules colliding increases. As the collision increases, the energy of molecules increases and molecules start colliding with sufficient energy to overcome the activation energy and more reactants get converted into products. This leads to an increase in the
(d)
Interpretation:
On increasing the concentration of reactant, the fraction of collision with sufficient energy increases or not is to be identified.
(e)
Interpretation:
On increasing the concentration of reactant, the reaction rate increases or not is to be identified.
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Chapter 12 Solutions
INTRODUCTION TO CHEMISTRY(LL)-W/CONNECT
- What happens to the reactants in an ineffective molecular collision?arrow_forwardWhich reaction mechanism assumptions are unimportant in describing simple ionic reactions between cations and anions? Why?arrow_forwardClassify each of the following statements as true or false. aSome equilibria depend on a steady supply of a reactant in order to maintain the equilibrium. bBoth forward and reverse reactions continue after equilibrium is reached. cEvery time reactant molecules collide, there is a reaction. dPotential energy during a collision is greater than potential energy before or after the collision. eThe properties of a transition state are between those of the reactants and products. fActivation energy is positive for both the forward and reverse reactions. gKinetic energy is changed to potential energy during a collision. hAn increase in temperature speeds the forward reaction but slows the reverse reaction. iA catalyst changes the steps by which a reaction is completed. jAn increase in concentration of a substance on the right-hand side of an equation speeds the reverse reaction rate. kAn increase in the concentration of a substance in an equilibrium increases the reaction rate in which the substance is a product. lReducing the volume of a gaseous equilibrium shifts the equilibrium in the direction of fewer gaseous molecules. mRaising temperature results in a shift in the forward direction of an endothermic equilibrium. nThe value of an equilibrium constant depends on temperature. oA large K indicates that an equilibrium is favored in the reverse direction.arrow_forward
- Apply collision theory to explain why increasing the concentration of a reactant usually increases the reaction rate.arrow_forwardHow do chemists envision reactions taking place in terms of the collision model for reactions? Give an example of a simple reaction and how you might envision the reaction’s taking place by means of a collision between the molecules.arrow_forwardApply collision theory to explain why powdered zinc reacts to form hydrogen gas faster than large pieces of zinc when both are placed in hydrochloric acid solution.arrow_forward
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