Final Exam Review Section 4 Flashcards
Calories
1 Calorie (C) = 1000 calories (c) = 1 Kilocalorie = 4.184 kJ
Change in internal energy
delta E = q + W
Work EQ
W = -P * (delta V)
1 L*atm
101.33 J
Pressure volume work
only done if number of moles of gas on left is different than number of moles of gas on right
+ Work
Work is being done on the system
Surrounding doing work on system (endo)
(-) Work
Work is being done by system
System doing work on surroundings (exo)
Enthalpy
change in energy of system under constant pressure
Delta H = q
Exothermic process
system releases energy as form of heat
-q
Endothermic process
system absorbs energy from heat in surroundings
+q
Specific Heat (C)
energy transferred as heat that is required to raise temperature of 1 g of a substance
greater the heat capacity the more energy required to change its heat
C water
4.184 J/(g* deg C)
Heat formula
q = mC(delta T)
q metal + q water = 0
q water = -q metal
q rxn + q cal = 0
q cal = - q rxn
q Cal
C cal * (delta T)
Standard State
Standard enthalpy is 0
enthalpy change for reaction formula
sum of products - sum of reactants
Dimagenetic
All electrons are spin-paired p
paramagnetic
any element with unpaired electrons
wave formula
c = lambda * frequency
c (speed of light)
2.998 x 10^8 m/s
Photon Energy
E = h * (frequency) or E = h * (c/lambda)
J/photon
h (planck’s constant)
6.626 x 10^(-34) J * s
Bohr Model of atom
a. electrons can only have certain value of energy corresponding to their energy level
b. Electrons move around the nucleus of the atom in a fixed circular pattern without losing energy
c. spacing of energy levels changes with increasing n values
Change in Energy Formula
Ef - Ei = -2.179 x 10^(-18) *[(1/nf2) - (1/ni2)]
Wavelength momentum
lambda = h/(m*v)
m in kg
