Complete the following statements by writing one of these words or phrases in each
blank.
$$
\begin{array}{ll}
\begin{array}{l}
\text { activated complex } \\
\text { alternative pathway } \\
\text { balanced } \\
\text { change } \\
\text { close to each other } \\
\text { collide }
\end{array} & \begin{array}{l}
\text { kilojoules per mole, } \mathrm{kJ} / \mathrm{mol} \\
\text { larger } \\
\text { collision }
\end{array} \\
\text { lower activation energy } \\
\text { coefficient } & \text { minimum } \\
\text { disrupts } & \text { moles per liter } \\
\text { endergonic } & \text { more quickly } \\
\text { endergonic reaction } & \text { net } \\
\text { equal } & \text { new bonds } \\
\text { equal to } & \text { no effect } \\
\text { equilibrium constant } & \text { old bonds } \\
\text { exergonic } & \text { orientation } \\
\text { fraction } & \text { phase } \\
\text { greater than } & \text { positive } \\
\text { heterogeneous } & \text { pressures } \\
\text { homogeneous } & \text { products } \\
\text { increases } & \text { reactants } \\
K_P & \text { released } \\
\hline
\end{array}
$$
Increasing the concentration of one or both reactants will lead to
_____________ distances between reactant particles and to their occupying a
larger percentage of the volume. Therefore, more collisions can be expected to
occur per second.