CHEM 122 Final Exam

When a reaction is spontaneous, you can predict: K>1, products will be favored, -ΔG, -ΔH, +ΔS, and +E°.

Collision theory - An effective collisions is one where particles must collide, collide in proper orientation, and have sufficient energy.

A lower activation energy (E_a) means a faster reaction.

Reaction Rate (Products): Rate = \dfrac{\Delta\left[concentration\right]}{\Delta t}

Reaction Rate (Reactants): Rate = \dfrac{-\Delta\left[concentration\right]}{\Delta t}

Relative rate law: \frac{1}{coef} (Rate of reaction) = \frac{1}{coef} (Rate of reaction) = \frac{1}{coef} (Rate of reaction)….

Rate law: Rate = k[A]^m[B]ⁿ

Zero order is where n=0 and has the units Ms^-

First order is where n=1 and has the units s^-

Second order is where n=2 and has the unitsM^-s^-

Finding the overall order: n+m

Arrhenius equation: ln\left(\frac{k2}{k1}\right)=-\frac{Ea}{R}\left(\frac{1}{T2}-\frac{1}{T1}\right)

Equilibrium expression: Keq=\frac{\left\lbrack C\right\rbrack^{c}\left\lbrack D\right\rbrack^{d}}{\left\lbrack A\right\rbrack^{a}\left\lbrack B\right\rbrack^{b}}

When the reaction is written backwards, the equilibrium constant is inverted.

When the coefficient of an equation are multiplied by a factor, the equilibrium constant is raised to the power of that factor.

When you add equations to get a new equation, the equilibrium constant of the new equation is the product of the original K values.

Arrhenius acid - a substance that increases the concentration of hydrogen ions (H⁺) in aqueous solution, contributing to its acidity.

Arrhenius base - a substance that increases the concentration of hydroxide ions (OH⁻) in aqueous solution, thus contributing to its basicity.

Bronsted-Lowry acid - a proton donor

Bronsted-Lowry base - a proton acceptor

K in terms of pressure (gases only): Kp=Kc\left(RT\right)^{\Delta n}

\Delta n = moles of products - moles of reactants