Chemistry I
Unit: Energy
Outline
I. kinetic theory and temperature
A. kinetic theory states
1. All matter is made of __________________
2. Atoms have random motion that is perceived as ___________________. The
motion can be __________________, ________________ or
________________
3. If atoms are not in motion, the temperature must be ________________
4. The pressure of a gas is a function of the _________________ hitting the
sides of its container. In gases, all collisions are _________________.
5. In respect to action, the motion of a gas determines its __________________
while the size of the particle is deemed _____________________.
B. Temperature is the measurement of the _________________ of particles.
1. Therefore the ____________________ the temperature, the
____________________ the movement of the particles.
Ex: a piece of aluminum is heated from 10 to 20 C, the particles are moving
the fastest at ________________
2. Temperature is indicated with T, while initial T = _______, final T = _____
and change in T = ________________
Ex. If Ti = _________ , and Tf = _________ , then ΔT = _____________
II. measuring heat energy
A. Heat (Q)- the flow of ________________ due to a difference in temperature
B. Comparisons
1. Heat in a tablespoon of water- vs heat in a bathtub of water
2. Heat in a tablespoon of water vs heat of a tablespoon of oil
3. Temperature vs heat
C. Units- measurement of the amount of ________ required or available for transfer
a. Joules, kilojoules- 4.184 joules is equal to the amount of __________
required to heat one gram of water one degree Celsius
b. calories, Calories (kilocalories) – one calorie is equal to the amount of
_____________required to heat one gram of water one degree Celsius
c. BTU = ___________________________________
d. Conversions
Ex: Convert 350.1 J to calories
Convert 5030 kcal to J
Convert 900.0 kJ to cal
D. Specific heat capacity (s) or (Cp) – quantity of energy required to raise _______
gram of any substance _________ degree Celsius.
a. Valuesi
specific heat of water is 4.184 J/gC OR 1.000 cal/gC
ii specific heat of ___________ is _____________
iii specific heat of ___________ is ______________
b. Calculating heat
i
Equation
Q = (m)(∆T)(s)
m=
∆T =
s=
ii Applications
Ex: How much energy is required to heat 20.0 grams of water from 15.6 C to 26.3
C? Ex: what is the specific heat of a metal if it takes 26.3 joules to heat 1.4 grams
15.2 C? what is this metal?
Ex: what is the final temperature of a 5.3 gram sample of iron that loses 500.2 J of
energy, if the iron beginning temperature is 120.0 C?
III. energy transfer
1. Law of Conservation of energy (Q1 = Q2), states that energy cannot be
_____________________ nor __________________________, but can be
______________________________.
2. Using LCOE to calculate variables
(m1)(∆T1)(s1) = (m2)(∆T2)(s2)
Ex: If 100.0 grams of water is heated 45 C, what amount of zinc must have lost 32
C?
IV. The ‘energy curve’
Endothermic
1. Graph shape
a. Temperature change- temperature is ________________________, energy
is being used to ___________________________________________
b. Phase change- temperature is ___________________, energy is being
used to overcome ____________________________ ________________
2. Reading temperatures
a. Normal boiling/condensation point of water is _________________
b. Normal freezing/ ____________ point of water is _______________
3. Reading energy
a. Heat of fusion- the amount of energy required to ___________ one gram
(or one mol) of any substance
Ex: the heat of fusion of ______________ is ________________
b. Heat of vaporization- the amount of energy required to _______________
one gram (or one mol) of any substance