exam 1
2/13
exam 1
2/13
The exam will be on Wednesday, 2/13, from 7:30 pm to 9:00 pm in both BUR 106 and UTC 2.112A
Students will split between two rooms on campus according to the first letter of their last name.
A - L go to UTC 2.112A
M - Z go to BUR 106
Make sure you go to the right room according to your letter or face an exam penalty.
What we provide on Exams We will provide all students with:
Note that the periodic table handout is available on the gchem site in the appendix under "Exam Preparation". Here is a direct link to the Periodic Table Handout for Exam 1.
Coverage: Exam 1 covers all the material that was covered on LE's 01-08 and HW's 01-03. Gchem Chapters: The exam covers all of Chapter 7 on Physical Equilibria and most of the first section of Chapter 8 on Chemical Equilibria (to the divider shown in gchem).
Questions: The exam will have about 20 multiple choice questions. The questions will have an equal weight of 5 points each. However, if some very short (easy) questions are included, their point values will be 2-3 points and the question count will go up closer to 25 questions. Point values are included with all questions. We will only grade you by what is bubbled in on the answer sheet. We will not look at your exam copy for answers, nor consider them in any way. Bubble carefully and correctly.
Common Chemistry Knowledge The following are common calculations that you have to know for any chemistry class. I'm a little embarassed including them - but better safe than sorry.
molecular weight =
mass of substance
moles of substance
molarity =
moles of solute
liters of solution
%conc =
mass of solute
mass solution
x 100%
molality =
moles of solute
kg of solvent
mole fraction of A =
moles of A
total moles
Main Equations/Formulas for Exam 1 Note that the student will need to know (memorize) all of the mathematical formulas for the exam. The Periodic Table Handout will only have constants, conversion factors, and data - no formulas.
\(q = m\cdot C_{\rm s}\cdot \Delta T\)
\(q = m \cdot \Delta H_{\rm transition}\)
\( \ln\left({P_2\over P_1}\right) = {\Delta H_{\rm vap}\over R}\left({1\over T_1}-{1\over T_2}\right) \)
\(\Delta H_{\rm solution} = \Delta H_{\rm lattice} + \Delta H_{\rm hydration}\)
\( C_{\rm gas} = k_{\rm H} \; P_{\rm gas} \)
\(P_{\rm solution} = \chi_{\rm solvent}\cdot P^\circ \)
\(\Delta T_{\rm f} = i\cdot k_{\rm f} \cdot m \)
\(\Delta T_{\rm b} = i\cdot k_{\rm b} \cdot m \)
\(\Pi = i\cdot MRT \)
Help Page on van't Hoff Factor
aA + bB ⇌ cC + dD
mass action =
activity, K
aCc aDd
aAa aBb
mass action =
conc, Kc
[C]c [D]d
[A]a [B]b
mass action =
press, Kp
PCc PDd
PAa PBb
Kp = Kc(RT )Δn
Note: remember to use 0.08206 L atm/mol K
for the value of R in this equation. And that...
Δn = (#mol gas products) – (#mol gas reactants)
Heating Curves
heating a substance: \(q = m\cdot C_{\rm s}\cdot \Delta T\)
Phase changes: \(q = m \cdot \Delta H_{\rm change}\)
Know how to calculate for various heating scenarios and phase changes. We WILL provide the heat capacities and enthalpies of change that are needed.
Vapor Pressure vs Temperature
Clausius-Clapeyron Equation: \( \ln\left({P_2\over P_1}\right) = {\Delta H_{\rm vap}\over R}\left({1\over T_1}-{1\over T_2}\right) \)
Your thinking here is that there are 5 variables in this equation. Somehow, we will give you 4 of them and you'll calculate the last one. Also remember... all normal boiling points have vapor pressures equal to 1 atm by definition.
Making Solutions (aka: Dissolving stuff)
Rule of Thumb: "Likes Dissolve Likes"
Which means that polar solvents tend to best dissolve polar substances and non-polar solvents tend to dissolve non-polar substances. If you have a mismatch (polar/non-polar), you are most likely going to have INsoluble substances - or put another way: the solubility will be very very low if there is a mismatch in polarities.
Dissolving Solids
When a solid does dissolve, the following must be true:
\(\Delta H_{\rm solution} = \Delta H_{\rm lattice} + \Delta H_{\rm hydration}\)
The lattice energy for a solid, \(\Delta H_{\rm lattice}\), is always +positive the way we use it (expanding the solid into separate molecules or ions). The hydration energy, \(\Delta H_{\rm hydration}\), is always –negative in the way we use it. Most salts when dissolving in water tend to have slightly bigger (magnitude) lattice energies than hydration energies which means that most salts have endothermic heats of solution (\(+\Delta H\)).
Dissolving Gases
Because gases have no lattice energy, the heat of solution for all gases is exothermic (\(-\Delta H\)). The solubility of a gas in a solvent is directly proportional to the partial pressure of the gas in contact with the solvent. That is Henry's Law. Quantitatively Henry's Law is:
Henry's Law: \( C_{\rm gas} = k_{\rm H} \; P_{\rm gas} \)
Vapor Pressure Lowering
Raoult's Law: \(P_{\rm A} = \chi_{\rm A}\cdot P_{\rm A}^\circ \) for volatile solvent A and non-volatile solute
Raoult's Law: \(P_{\rm total} = \chi_{\rm A}\cdot P_{\rm A}^\circ + \chi_{\rm B}\cdot P_{\rm B}^\circ \) for volatile solvent A and volatile solute B
Freezing Point Depression: \(\Delta T_{\rm f} = i\cdot k_{\rm f} \cdot m \)
Boiling Point Elevation: \(\Delta T_{\rm b} = i\cdot k_{\rm b} \cdot m \)
Osmotic Pressure: \(\Pi = i\cdot MRT \)
Remember: All concentration terms will need adjustment with the van't Hoff factor, \(i\), if the solute dissociates into ions (salts).
Students will be able to...
Note that only the first 4 outcomes are on Exam 1.
Students will be able too...