Energy
Energy produces heat and it has the ability to do work
2 Types of Energy:
1. Potential energy
2. Kinetic energy
*break bonds to release chemical energy
Temperature- the measurement of every and it measures random motion
heat- the flow of energy due to temperature difference
endothermic- something gains heat
exothermic- something loses heat
Thermodynamic- the study of energy
1st law of thermodynamic- energy of the universe is constant because of the law of conservation
Internal energy- energy of the system
the change of energy is heat and work: DE = q + w
work = f x d
units of energy :
Joules = J
calories = cal
Calories= Cal
Cl = 1000 cal
formula: q = mcAT
q = heat
m = mass
c = specific heat capacity
t = temperature
specific heat capacity= the amount required to change the temperature by 1 degrees C of a 1 g substance
q = 41.840 J
m = ?
C = 4.184 J/ degrees C
TF = 28.5 degrees C
TI = 22.0 degrees C
41.840/(4.184 (28.5 - 22.0) = m
41.840/27.196 = 1.5x10^3
enthalpy- flow of heat
exothermic- negative
endothermic- positive
Calculate the heat of reaction of C2H4(g) + H2(g) -> C2H6(g)
1.) 3H2 + 1/2 N2 -> 2NH3 delta H = -92kJ
2.) NO2 + 2H2 -> 1/2 N2 + 2H2O delta H = -170kJ
NO2 + 7/2 H2 -> 2H2O + NH3 delta H = -216kJ
the answer is -216kJ
2 Types of Energy:
1. Potential energy
- elastic- energy stored in something elastic
- gravitational- gravity
- chemical- energy stored in bond
2. Kinetic energy
- energy of motion
*break bonds to release chemical energy
Temperature- the measurement of every and it measures random motion
heat- the flow of energy due to temperature difference
- if something is hot, it has a lot of energy
- if something is cold it does not have a lot of energy
endothermic- something gains heat
exothermic- something loses heat
Thermodynamic- the study of energy
1st law of thermodynamic- energy of the universe is constant because of the law of conservation
Internal energy- energy of the system
the change of energy is heat and work: DE = q + w
work = f x d
units of energy :
Joules = J
calories = cal
Calories= Cal
Cl = 1000 cal
formula: q = mcAT
q = heat
m = mass
c = specific heat capacity
t = temperature
specific heat capacity= the amount required to change the temperature by 1 degrees C of a 1 g substance
q = 41.840 J
m = ?
C = 4.184 J/ degrees C
TF = 28.5 degrees C
TI = 22.0 degrees C
41.840/(4.184 (28.5 - 22.0) = m
41.840/27.196 = 1.5x10^3
enthalpy- flow of heat
exothermic- negative
endothermic- positive
Calculate the heat of reaction of C2H4(g) + H2(g) -> C2H6(g)
1.) 3H2 + 1/2 N2 -> 2NH3 delta H = -92kJ
2.) NO2 + 2H2 -> 1/2 N2 + 2H2O delta H = -170kJ
NO2 + 7/2 H2 -> 2H2O + NH3 delta H = -216kJ
the answer is -216kJ