- official UT ID card (with your picture and name on it)
- a simple scientific calculator (not a graphing calculator)
- a pencil(s) and eraser
- memorized formulas in your head - not on paper or anything else
- nothing else is allowed

- A printed copy of the exam (every exam has a unique version number on it).
- An answer sheet for the exam. This is a bubblesheet for your answers.
- An exam cover page that has ALL needed conversion factors and data. No formulas will be given.
- A periodic table of the elements with symbols, atomic number, and atomic weights.

\(q = m\cdot C_{\rm s}\cdot \Delta T\)

\(q = m \cdot \Delta H_{\rm transition}\)

\( \ln\left({P_2\over P_1}\right) = {\Delta H_{\rm vap}\over R}\left({1\over T_1}-{1\over T_2}\right) \)

\(\Delta H_{\rm solution} = \Delta H_{\rm lattice} + \Delta H_{\rm hydration}\)

\( C_{\rm gas} = k_{\rm H} \; P_{\rm gas} \)

\(P_{\rm solution} = \chi_{\rm solvent}\cdot P^\circ \)

\(\Delta T_{\rm f} = i\cdot k_{\rm f} \cdot m \)

\(\Delta T_{\rm b} = i\cdot k_{\rm b} \cdot m \)

\(\Pi = i\cdot MRT \)

\( K_{\rm sp} = [{\rm M}^{y+}]^x\,[{\rm A}^{x-}]^y \hskip16pt {\rm for\;salt} \;\; {\rm M}_x {\rm A}_y \)

Periodic Table

Conversion factors

All physical constants and data needed for the exam

such as: \(R \; K_{\rm sp} \; k_{\rm b} \; k_{\rm f} \; k_{\rm H} \; \Delta H_{\rm transition} \; C_{\rm s} \)

Students will be able to...

- Demonstrate mastery of and compound and reaction stoichiometry (mole to mole conversion and grams to mole conversions).
- Predict the sign of Δ
*G*, Δ*H*, and/or Δ*S*for physical change - Understand the concept of spontaneous change and equilibrium in the context of phase changes, including calculating phase transition temperatures from standard thermodynamic data.
- Interpret heating curves and calculate heat required for phase transitions and temperature changes.
- Describe phase transitions (macroscopically and microscopically).
- Understand phase in the context of Boltzmann distribution.
- Understand how intermolecular forces, temperature, and solute concentration affect vapor pressure.
- Interpret phase diagrams and identify normal boiling and melting point, critical point, and triple point.
- Describe the factors that favor the dissolution process in terms of intermolecular forces and thermodynamics (eg.: enthalpies of solution, hydration, lattice energy, entropies of solution, free energy of solution, and temperature).
- Describe how
*T*and*P*(Henry’s Law) each affect solubility. - Define and perform calculations for common concentration units: molarity, molality, and mole fraction.
- Perform calculations and understand the concepts of the 4 colligative properties: vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure.
- Describe the dissociation of ionic compounds in solution and the effects on colligative properties (van’t Hoff factor,
*i*).

Students will be able to...

- Understand the concept of the solubility product,
*K*_{sp}. - Write total and net ionic equations to identify spectator ions.
- Quantitatively determine solubility from
*K*_{sp}and vice versa. - Estimate molar solubility from
*K*_{sp}. - Understand and apply the "common ion effect" on solubility.
- Given concentrations of specific ions, predict if a precipitate will form (amount or concentration) using
*Q*_{sp}vs*K*_{sp}.