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UNIT 12 REVIEW HINTS
Given a phase diagram and a set of conditions be able to determine what state and or what
phase occurred when the conditions were altered. Be able to locate solid, liquid and gas
phases. Like #2 on the Review
Know the specific phases involved during melting, freezing, condensation, vaporization,
sublimation and deposition. See page 5 of notes and page 4 in packet
Know which phase change is endothermic and exothermic and know definitions of
exothermic(release of heat, heat is a product) and endothermic(heat is required, heat is a
reactant). See page 5 of notes and #4 on Review and page 4 in packet
Be able to determine if an equation is thermochemical (has phases, ΔH & balanced) and
determine whether it is endo or exo. See page 4 of notes and the equation in #8 on the
Review (ΔH is positive so reaction is endothermic) and #14 on the Review(See review key)
Heating curve of water know how PE, KE, and Temperature change (as energy is added what
happens to the KE & PE of the particles) See page 11 in the packet and #11 on the Review
Be able to define and identify the location of the triple point (where three phases exist at the
same time) and critical point (beyond this point you can no longer have a liquid) on a phase
diagram. page 5 of notes and page 5, 7 and 12 in the packet
Know what is meant by normal atmospheric pressure. See page 6 of review
Be able to read a reaction diagram and determine whether the reaction is endothermic or
exothermic. Use the diagram to calculate ∆H. Be able to calculate ∆H given the H of the
products and H of the reactants. See page 3 in packet and page 4 of notes
What medium does heat transfer occur in conduction (solid), convection(liquid and gas) &
radiation(sun)See notes page 1
Convert between units of energy, Cal, cal, Joules, kJ You will only be given 1cal=4.184 J.
You have to know metric prefixes and what Capital C means. Page 2 of notes and Book
problems
Use the equation q=m Cp ∆T to calculate any variable page 2 and 3 of notes, book problem
#78 and review problems #16 and #17.
Know how to calculate ∆T. (difference in temperature (always +)
What do we call the solid(ice, below 0°C), liquid(water, between 0°C and 100°C) and
gas(vapor, greater than 100°C) phases of H2O.
Be able to apply the law of conservation of energy. Be able to tell how energy is transformed
i.e. kinetic to potential or vice versa Page 1 of notes rollercoaster
What happens to the energy when a hot substance is added to a cold substance. Page 3 of
Notes
Be able to solve for Cp or mass or Tf in a calorimetry problem. See notes page 3, packet page
2 and review problems #6 and #7
Use the equation q=n∆H for reactions and phase changes. See notes page 6, review #8, #9
and #19.
Be able to calculate total heat using the heating curve of water. See note page 5, packet page
4 and review problems #20 and #21.
Know SI unit of energy(J) and definition of calorimeter(insulated container used to measure
energy changes) Notes pages 1 and 2
Distinguish between calorie (for water) and specific heat (for any substance). See notes page
1 and 2 and packet page 1
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What does the sign of ∆H indicate.(tells you whether the reaction is endothermic or
exothermic) If the sign is positive, compare the energy stored in the bonds of the reactants
and the energy stored in the bonds of the products. Know that ∆H is equal to products minus
reactants. (if ∆H is positive that means the Products have a greater energy in the bonds than
the reactants do in the bonds) See review #14.
Define volatile (easily evaporated) be able to read graph on page 6 and tell which substance
is more volatile
On a phase diagram, know what the lines represent (equilibrium) and be able to recognize a
water phase diagram(solid-liquid line has a negative slope) and know if a solid will float or
sink in its own liquid (if negative slope it is water and solid will float)