thermodynamics and engines Flashcards
first law of thermodynamics
describes how energy is conserved in a system through heating, cooling and doing work
equation for first law of thermodynamics
Q = △U + W
U = internal energy
positive and negative Q
+Q = energy transferred to system
-Q = energy transferred away from system
non-flow process
a process which occurs in a closed system
no gas flows in or out the system
condition to apply first law of thermodynamics to a closed system
gas has to be an ideal gas
means energy is only dependent on the temperature
need to assume that if any work is done there is a change in volume
ideal gas equation
pV = nRT
p1 V1 / T1 = P2 V2 / T2
positive and negative meaning for work done
+W = work done by the system
-W = work done on the gas
isothermal
a process in which the temperature of the system remains constant
as internal energy is dependent on only temperature, △U = 0
so Q = W
what does it mean when Q = W
supplying heat energy to the system will result in an equivalent amount of work being done by the gas (volume increases)
if work is done on system then an equivalent amount of energy is lost
isothermal equations
pV = constant
p1 V1 = p2 V2
adiabatic process
a process in which no heat is gain or lost in a system
Q = 0
so △U = -W
what does △U = -W mean
any change in the internal energy is caused by work done on/by system
if work is done by system then internal energy will decrease by the equivalent amount vice versa
adiabatic process equations
pV^γ = constant
p1 V1^γ = p2 V2^γ
changes at a constant pressure equation
W = p△V
V1 / T1 = V2 / T2
Changes at a constant volume
W = 0 so Q = △U
means all of the heat transferred to/out the system goes directly to increasing/decreasing internal energy
p / T = constant
p1 / T1 = p2 / T2
p/V graph
arrow drawn to indicate in which direction the change is happening
area under = magnitude of work done
isotherm
p ∝ 1/V
isothermal expansion = right
isothermal compression = left
the higher the temperature the further the curve is from the origin
p-V diagrams for adiabatic processes
have a steeper gradient than a isotherm
area is larger than isotherm curve so more work is done to compress a gas adiabatically than isothermally
the gas does less work if it expand adiabatically instead on isothermally
cyclic process
a system can go through different processes to form a loop
net work done of cyclic curve
find the difference between work done by the system and work done to the system
work done per cycle = area of loop
four stroke engines
engines which burn fuel once every four strokes of a piston
internal combustion engines
contains cylinders filled with air
air is mixed with fuel, which is then burned, releasing a large amount of energy
the air fuel mixture is trapped by two tight fitting pistons which move up and down
induction
piston starts at top of cylinder and moves down, increasing the volume of the gas above it
this sucks in a mixture of air and fuel in the open inlet valve
pressure remains constant, just below atmospheric pressure
indictaor diagram is straight horizontal line
compression
inlet valve is closed and the piston moves back up
work is done on the gas increasing the pressure
just before the piston is at the end of the stroke, the spark plug creates a spark which ignites the air-fuel mixture
temperature and pressure increases at an almost constant volume