Complete the following statements by writing one of these...

Complete the following statements by writing one of these words or phrases in each blank. $$ \begin{array}{ll} \begin{array}{l} \text { activated complex } \\ \text { alternative pathway } \\ \text { balanced } \\ \text { change } \\ \text { close to each other } \\ \text { collide } \end{array} & \begin{array}{l} \text { kilojoules per mole, } \mathrm{kJ} / \mathrm{mol} \\ \text { larger } \\ \text { collision } \end{array} \\ \text { lower activation energy } \\ \text { coefficient } & \text { minimum } \\ \text { disrupts } & \text { moles per liter } \\ \text { endergonic } & \text { more quickly } \\ \text { endergonic reaction } & \text { net } \\ \text { equal } & \text { new bonds } \\ \text { equal to } & \text { no effect } \\ \text { equilibrium constant } & \text { old bonds } \\ \text { exergonic } & \text { orientation } \\ \text { fraction } & \text { phase } \\ \text { greater than } & \text { positive } \\ \text { heterogeneous } & \text { pressures } \\ \text { homogeneous } & \text { products } \\ \text { increases } & \text { reactants } \\ K_P & \text { released } \\ \hline \end{array} $$ Increased temperature increases the rate of both the forward and the reverse reactions, but it increases the rate of the _____________ reaction more than it increases the rate of the _____________ reaction. Therefore, increasing the temperature of a chemical system at equilibrium will disrupt the balance of the forward and reverse rates of reaction and shift the system in the direction of the _____________.

Complete the following statements by writing one of these words or phrases in each
blank.
$$
\begin{array}{ll}
\begin{array}{l}
\text { activated complex } \\
\text { alternative pathway } \\
\text { balanced } \\
\text { change } \\
\text { close to each other } \\
\text { collide }
\end{array} & \begin{array}{l}
\text { kilojoules per mole, } \mathrm{kJ} / \mathrm{mol} \\
\text { larger } \\
\text { collision }
\end{array} \\
\text { lower activation energy } \\
\text { coefficient } & \text { minimum } \\
\text { disrupts } & \text { moles per liter } \\
\text { endergonic } & \text { more quickly } \\
\text { endergonic reaction } & \text { net } \\
\text { equal } & \text { new bonds } \\
\text { equal to } & \text { no effect } \\
\text { equilibrium constant } & \text { old bonds } \\
\text { exergonic } & \text { orientation } \\
\text { fraction } & \text { phase } \\
\text { greater than } & \text { positive } \\
\text { heterogeneous } & \text { pressures } \\
\text { homogeneous } & \text { products } \\
\text { increases } & \text { reactants } \\
K_P & \text { released } \\
\hline
\end{array}
$$
Increased temperature increases the rate of both the forward and the reverse
reactions, but it increases the rate of the _____________ reaction more than
it increases the rate of the _____________ reaction. Therefore, increasing the
temperature of a chemical system at equilibrium will disrupt the balance of the
forward and reverse rates of reaction and shift the system in the direction of the
_____________.

Key Concepts

Chemical Equilibrium

Chemical equilibrium occurs when the forward and reverse reactions proceed at the same rate, resulting in constant concentrations of reactants and products. This concept is foundational for understanding how systems respond to disturbances, such as changes in temperature, and how shifts in equilibrium occur to re-establish balance in the reaction rates.

Reaction Kinetics

Reaction kinetics involves the study of the rates at which chemical reactions occur and the factors that affect these rates, including temperature and activation energy. Understanding kinetics is crucial for analyzing how changes in conditions alter the speed of both forward and reverse reactions in a chemical system.

Effect of Temperature on Reaction Rate

Temperature significantly influences reaction rates by increasing the kinetic energy of molecules, which leads to more frequent and energetic collisions. As temperature rises, both the forward and reverse reaction rates increase, although not necessarily to the same extent, depending on the activation energies involved.

Activation Energy and the Arrhenius Equation

Activation energy is the minimum energy required for a reaction to occur, and the Arrhenius equation quantitatively relates the rate constant to temperature and activation energy. A higher activation energy means that a reaction's rate is more sensitive to temperature changes, which is key to understanding why one reaction direction might be affected more than the other when temperature is increased.

Le Chatelier's Principle

Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the system will adjust itself to partly counteract the change. In the context of temperature changes, this principle helps explain how an equilibrium will shift—toward the endothermic direction if heat is added—to re-establish equilibrium under the new conditions.

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