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Transcript
Thermodynamics Relationships Between Heat and Work Heat, Work, and Internal Energy • As long as a substance does not change phase, its internal energy will increase as long as its temperature increases • Work can transfer energy to a substance – Results in an increase in internal energy • Can be transferred to another substance as heat • Energy can be transferred to a substance as heat and from the substance as work Heat, Work, and Internal Energy • Heat and work are both energy transferred to or from a system – System – a collection of matter within a clearly defined boundary across which no matter passes – Environment – everything outside a system that can affect or be affected by the system’s behavior • Also called the surroundings • All the parts of a system are in thermal equilibrium with each other both before and after a process adds or removes energy Heat, Work, and Internal Energy • Pressure is the force per unit area acting on an object • Pressure = force / area • P=F/A • Measured in Pascal's = N/m2 – Other units are atmospheres (atm), millimeters of mercury (mmHg), bars (bar), pounds per square inch (psi), technical atmospheres (at), or torr (Torr) • Caused by particle collisions Heat, Work, and Internal Energy • Work done on or by a gas is the pressure multiplied by the change in volume • Work = force * distance • W=Fd • W=pressure * volume change • W=PΔV • Change in volume = area * distance • ΔV = Ad Heat, Work, and Internal Energy • If the gas is compressed, ΔV is negative – Work is done on the system • If the gas expands, ΔV is positive – Work is done by the system • If the volume remains constant, no work is done Heat, Work, and Internal Energy • An engine cylinder has a cross-sectional area of 0.010m2. How much work can be done by a gas in the cylinder if the gas exerts a constant pressure of 7.5*105 Pa on the piston and moves the piston a distance of 0.040 m? • A = 0.010 m2 d = 0.040m • P = 7.5*105 Pa or 7.5*105 N/m2 • ΔV = ? W=? Heat, Work, and Internal Energy • ΔV=Ad = 0.010 m2 * 0.040 m = 4.0*10-4 m3 • W=PΔV = (7.5*105 N/m2) (4.0*10-4 m3) = 3.0*102 J Thermodynamic Processes • Work, internal energy, and heat are all related – Not every one of these is present in all ideal thermodynamic processes • No work is done in constant-volume processes – Called isovolumetric – a thermodynamic process that takes place at constant volume so that no work is done on or by the system • Often take place in a bomb calorimeter Thermodynamic Processes • Internal energy is constant in a constanttemperature process • Isothermal process – a thermodynamic process that takes place at constant temperature and in which the internal energy of a system remains unchanged – Similar to a balloon expanding as the pressure drops before a storm hits • The balloon expands to keep pressure equal with the environment Thermodynamic Processes • Energy is not transferred as heat during an adiabatic process – A thermodynamic process during which work is done on or by the system but no energy is transferred to or from the system as heat – Rapid compression or expansion of gases in insulated containers (refrigerators, internal combustion engines)