- 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.
- A separate sheet showing a periodic table of the elements with symbols, atomic number, and atomic weights.
- Also on that separate sheet will be numerous constants, conversion factors, and common data that is needed to solve exam problems.

\[PV=nRT\]

Boyle's Law: \(P_1V_1 = P_2V_2\) (constant *n*, *T*)

Charles' Law: \(\displaystyle{V_1\over T_1} = {V_2\over T_2}\) (constant *n*, *P*)

Avogadro's Law: \(\displaystyle{V_1\over n_1} = {V_2\over n_2}\) (constant *P*, *T*)

Gay-Lussac's Law: \(\displaystyle{P_1\over T_1} = {P_2\over T_2}\) (constant *n*, *V*)

Air Up Your Tires Law: \(\displaystyle{P_1\over n_1} = {P_2\over n_2}\) (constant *V*, *T*)

Difficult to Do This Law: \(n_1T_1 = n_2T_2\) (constant *P*, *V*)

(note that you will be tested on the actual relationships of the physical properties and not the scientist's names)

and because density (*ρ*) is *m/V* and molar mass (*M*) is *m/n*, then you also know the molar mass of an ideal gas via:

\[{M={\rho RT\over P}}\]

Dalton's Law of Partial Pressures

\[P_{\rm total}=P_{\rm A} + P_{\rm B} + P_{\rm C} + \cdots\]

mole fraction of gas A: \(x_{\rm A}=P_{\rm A}/P_{\rm total}\)

Van der Waal's Equation of State (Gas Model)

\[\left(P+a{n^2 \over V^2}\right)(V-nb)=nRT\]

The average kinetic energy of an ideal gas

\[E_{\rm k} = U = {3\over 2}RT = {1\over 2}mv^2\]

Root mean squared velocity of a gas

\[{v_{\rm rms}=\sqrt{3RT \over M}}\]

Comparing rms velocities of two different gases at the same temperature

\[{{v_1\over v_2}=\sqrt{M_2 \over M_1}}\]

*R* = 0.08206 L atm/mol K

*R* = 62.36 L torr/mol K

*R* = 0.08314 L bar/mol K

*R* = 8.314 J/mol K

*N*_{A} = 6.022 × 10^{23} mol^{-1}

1 atm = 1.01325 × 10^{5} Pa

1 atm = 760 torr

1 atm = 14.7 psi

1 bar = 10^{5} Pa

1 in = 2.54 cm

1 lb = 453.6 g

1 gal = 3.785 L

\(\rho_{\rm water} = 1.00\) g/mL

\(\rho_{\rm mercury} = 13.6\) g/mL