Question

Identify which of the following statements are incorrect. If the statement is incorrect, rewrite it to be correct. (a) Reactions are faster at a higher temperature because activation energies are lower. (b) Rates increase with increasing concentration of reactants because there are more collisions between reactant molecules. (c) At higher temperatures, a larger fraction of molecules have enough energy to get over the activation energy barrier. (d) Catalyzed and uncatalyzed reactions have identical mechanisms.

Short answer

(a) and (d) are incorrect; they have been corrected in the solution steps.

Step-by-step solution

Analyze Statement (a)

Statement (a) is "Reactions are faster at a higher temperature because activation energies are lower." This statement is incorrect. Reactions are faster at higher temperatures because a larger fraction of molecules have enough energy to surpass the activation energy barrier, not because the activation energy itself is lower. The revised statement is: "Reactions are faster at a higher temperature because more molecules have sufficient energy to overcome the activation energy barrier."

Analyze Statement (b)

Statement (b) is "Rates increase with increasing concentration of reactants because there are more collisions between reactant molecules." This statement is correct as increasing the concentration of reactants indeed leads to more frequent collisions, which typically increases the rate of reaction.

Analyze Statement (c)

Statement (c) is "At higher temperatures, a larger fraction of molecules have enough energy to get over the activation energy barrier." This statement is correct. Increasing the temperature results in more molecules having the necessary kinetic energy to overcome the activation energy barrier, thus increasing reaction rates.

Analyze Statement (d)

Statement (d) is "Catalyzed and uncatalyzed reactions have identical mechanisms." This statement is incorrect. Catalysts provide an alternative reaction pathway with a lower activation energy. Thus, the mechanism of a catalyzed reaction often differs from that of an uncatalyzed reaction. The revised statement is: "Catalyzed and uncatalyzed reactions typically have different mechanisms."

Key concepts

Activation Energy

Activation energy is a fundamental concept in understanding reaction rates. It's the minimum amount of energy required for a chemical reaction to occur.
This energy barrier must be overcome for reactants to transform into products.
In essence, think of activation energy as a hurdle. Reactant molecules need to have enough energy to get over it. If they don't, the reaction won't proceed. Physically, this energy is needed to break bonds in reactants so new ones can form in products.

• Without sufficient energy, molecules remain unchanged, and the reaction remains slow or doesn't occur.
• When a reaction has a low activation energy, it's generally faster because more molecules can meet the energy requirement.

Visualization can help; imagine pouring balls up a hill (representing activation energy). Only balls with enough initial speed (energy) make it to the other side.
Remember, high activation energy means only a few molecules have the energy to react, slowing down the reaction rate.

Temperature Effect on Reactions

Temperature has a significant impact on the rate of chemical reactions. As the temperature increases, so does the kinetic energy of molecules.
The molecules move faster and collide more frequently. When molecules collide with higher energy, it's more likely for them to overcome the activation energy barrier.

• Increased temperature results in greater molecular motion and energy.
• This shift leads to more effective collisions where molecules can transform into products.

Some molecules might already be energetic enough to react at lower temperatures, but others will require thermal energy from higher temperatures.
It's not just about how often molecules collide – it's also about how hard the collisions are. Increased temperature results in more energetic and frequent collisions, thus increasing the reaction rate.
This is why bread dough rises faster in a warm environment or why ice melts quicker when brought into a hot room.

Catalysis and Reaction Mechanisms

Catalysts are substances that speed up reactions without being consumed in the process.
They do this by providing an alternative pathway for the reaction with a lower activation energy. Thus, more reactant molecules have the energy needed to react at a given temperature. Contrary to what some might think, catalyzed reactions have different mechanisms than uncatalyzed ones. Rather than fundamentally changing the reactants or products, a catalyst offers a new "route" for the reaction.

• The catalyst effectively lowers the energy hurdle, simplifying or altering the steps involved.
• Even though it speeds up the reaction, the catalyst remains unchanged after the reaction.

Catalysts play a critical role in industrial processes and even biological systems like enzymes, which are natural catalysts in living organisms.
Remember, the mechanism change due to catalysis is crucial – it can make reactions feasible or economically viable, such as in the synthesis of certain chemicals.