Ch 21: The Second Law of ThermodynamicsSee all chapters

Sections | |||
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Intro to Heat Engines | 12 mins | 0 completed | Learn |

Efficiency of Heat Engines | 14 mins | 0 completed | Learn |

Heat Engines & PV Diagrams | 19 mins | 0 completed | Learn |

Four Stroke Piston Engine | 44 mins | 0 completed | Learn |

Carnot Cycle | 8 mins | 0 completed | Learn |

Refrigerators | 54 mins | 0 completed | Learn |

Intro to Refrigerators | 27 mins | 0 completed | Learn |

Refrigerators & PV Diagrams | 27 mins | 0 completed | Learn |

Entropy and the Second Law | 46 mins | 0 completed | Learn |

Entropy & The Second Law | 27 mins | 0 completed | Learn |

Statistical Interpretation of Entropy | 12 mins | 0 completed | Learn |

Second Law for Ideal Gas | 7 mins | 0 completed | Learn |

Concept #1: Heat Engines and PV Diagrams

**Transcript**

Hey guys, in this video we're going to talk about heat engines and PV diagrams. PV diagrams were great resources when talking about thermal processes and we're going to see that the cycle in a heat engine is always composed of discrete thermal processes. So we're also going to want to use PV diagrams when talking about heat engines. Let's get to it. Real engine are always cyclical processes and a cyclic process is a process that always returns to its initial state. If the gas that made up the heat engine only went from state A to state B, sure heat could flow into it, we could have some Q in. This could produce some work and return some heat to the cold reservoir, sure, it could act entirely like an engine but the gas ends in the final state which is not the starting state of the engine. Gas needs to be in state A for the engine to work so unless you have some way of taking this gas and converting it back into state A, the engine can only operate once otherwise the engine will only be good for a single instance when work is produced. If the gas is a cyclic process, if you can get B back into A, then you can keep doing the engine you can keep doing the cycle indefinitely so long as there is a temperature difference so long as there is a hot reservoir and a cold reservoir. Now in reality everytime heat leaves the hot reservoir the temperature of the hot reservoir drops. In reality every time heat interest the cold reservoir, the temperature of the cold reservoir rises so in reality the hot reservoir is going to get colder, the cold reservoir is going to get hotter and eventually they will end at the same temperature, they'll end in thermal equilibrium and there will be no more heat flow that's driving the engine however in physics problems we're considering it as a hot reservoir and a cold reservoir. Remember guys that ideally, reservoirs can give up as much heat as they want. They can absorb as much heat as they want and never change their temperature. So ideally this temperature difference is never going to change. Delta T is zero for a reservoir always. So that temperature gradient, that temperature difference is never actually going to change in a physics problem, in reality it will. Remember guys on a PV diagram the work done in any cyclic process is the area enclosed by that cycle. We want to approximate the area, the shape of the cycle as some regular polygon, like a triangle, like a rectangle like a circle and that way we know the formula to find the area enclosed by it so we can always approximate the work done as just the area of a regular shape.

Now remember if the cycle is clockwise, the work done is negative. That is the work of the gas. So work is done by the gas. That released energy is what's converted into mechanical energy so the work by the gas which is negative is what produces the mechanical work of the engine which is positive. So if the gas loses energy, it loses that mechanical energy that is absorbed by the environment and that is the energy that is actually produced by the engine. So you always want the work due to the gas to be negative that's the only way that you can produce an engine because the gas has to release energy in order for an engine to work. If a gas absorbs energy, then that's not an engine because that requires you to input work to do anything that's absolutely not an engine if energy is not released.

An ideal gas undergoes the following cyclic process, how much work is done by the engine? Well we can approximate this as a rectangle and the area of this rectangle is going to be one half base times height. The base is 0.07 cubic meters, the height is 4 times 10 to the 5 Pascals, so this is one half 0.007, 4 times 10 to the 5, sorry, this is 10 to the 6 and this equals 14000 which is 14 kilojoules. Now what about the sign of the work? Well what about the work of the gas? Work of the gas is negative because this is clockwise. Always remember that the work of the gas is negative because this is clockwise so the work of the gases -14 kilojoules, this is work done by the gas the gas is releasing this energy into the environment. That means that the work of the engine is positive 14 kilojoules. The engine uses whatever energy is released by the gas to power itself and so the gas releases, this negative sign means the gas releases 14 kilojoules so the energy produced, sorry, the engine produces 14 kilojoules of work. Let's do a second problem a gas undergoes the following process beginning at atmospheric pressure and a volume of 0.01 cubic meters, let me just draw this out. It's at atmosphere pressure which is 1 times 10 to the 5 Pascals and 0.0, sorry, just 0.1. The pressure's in units of Pascals, the volume's in units of meters cubed and it's compressed so it drops its pressure sorry it's volume at constant pressure to this. So it's going at constant pressure to this. Then the gas is compressed further to an even smaller volume but this time with a pressure increase to twice the atmospheric pressure so now it's going still to the left it's still dropping its volume but now it's dropping its volume coordinated with a rise in pressure. The gas is then expanded at constant pressure back to this intermediate volume before returning to its initial state. Its initial state's at a lower pressure at the largest volume. This is a clockwise loop. A clockwise loop means that the work due to the gas is negative which means that the work due to the cycle or, sorry, the work released you can say the work in the environments is positive. Which means this is absolutely an engine. Cycles that are clockwise, always engines. Cycles that are counterclockwise, never engines because the work due to the gas is positive in that case so you have to do work on the gas in a counterclockwise cycle so they can never be an engine because work is not released. Alright guys, that wraps up this discussion on the first law of thermodynamics, heat engines and specifically how it applies on PV diagrams. Alright guys. Thanks for watching.

Example #1: Efficiency of a Four-Step Engine

**Transcript**

Hey guys, let's do an example, a proposed four step engine is produced n moles of a monoatomic ideal gas undergo the process shown in the following PV diagram what would the efficiency of engine be? The efficiency is given by the work output by the engine divided by the heat input into the engine remember there's two heats in a cyclic process in an engine there's going to be an amount of heat inputted which is going to be positive heat and an amount of heat output which is going to be negative heat. The work is easy to calculate the work is just the area contained by the cycle with the appropriate sign now first could this even be an engine, yes it can it's a clockwise cycle so it's absolutely an engine, the area is going to be the base times height because it's just a rectangle this is going to be 2Vnot this is going to be one half Pnot so this is 2vnot one half P not write that 2 and one half cancel this is just Pnot Vnot and this is absolute going to be positive it's going to be positive right energy released by engine so that's just the work done by the engine now in order to find how much heat is input we have to analyze the steps individual. I'm going to call this step one this step two this step three and this step four now something important to know about P.V diagrams and you can show this for yourself if you want is that when the process is going up into the right. The heat is always input into the system so process one and process two heat is going to be added into the system so Q is going to go in. When the process is down or to the left heat is always leaving the system. All we need to know is how much heat enters the system right this how much heat enters the system so we only have to look at steps one and two you can use the same method the same process that I'm using here to analyze steps three and four and show that the heat is always going to be leaving in those steps for step one first of all the work is always going to be 0 because this is an isochoric process this means that the first law of thermodynamics which says the change in internal energy is the heat transferred plus the work done just means ops sorry wrong color, it just means that the heat transferred is the change in internal energy for step one. Now the internal energy of any ideal gas is F over 2 NRT right an equation that we used a bunch of times because this is a monoatomic ideal gas the number of degrees of freedom is simply 3 one for each translational direction.

Now the change in internal energy is what we're interested in and this is going to be three halves NR delta T. We're talking about n moles simply changing its state there's no heat coming into the sorry there's no gas coming into the system no gas leaving the system so the only thing that changes when the internal energy changes is the temperature so the temperature is the only thing that gets this delta, the question is what is the change in temperature. Well PV equals N R T the ideal gas equation is going to tell us how the temperature changes as the gas changes state. This is going to tell us because the volume is a constant this is an isochoric process that V delta P is N R delta T the change in the left sides due entirely to a change in pressure the change on the right side is due entirely to a change in temperature so delta T is V delta P over N R now plugging that in to delta U so I can say delta T1 is equal to this, this equals three halves and N R times V1 delta P1 over N R notice that the N R in the numerator and the N R in the denominator cancel so this is three halves V1 delta P1 which is three halves what's the volume for step one it's just a Vnot what's the change in pressure in step one right from Pnot it's from one half Pnot to Pnot so this is just one half Pnot so this becomes three fourths Pnot Vnot. That's the change in internal energy for step one and by the first law of thermodynamics therefore the heat exchanged in step one is which is delta U1 is going to be positive three fourths Pnot Vnot. It's very important that the heat is positive because we're only looking for heat input into the gas we are not looking for heat output by the gas for step two the pressure doesn't change for step two delta P is 0, but Delta U is still equal to Q plus W. However we do know that at constant pressure W is equal to negative P delta V so this is for step two what's the pressure at step two it's just Pnot right what's the change in volume it's three Vnot minus 2Vnot sorry minus Vnot which is going to be positive 2Vnot so this is negative to Pnot Vnot right this is positive 2Vnot. So that's how much work is done during step two now what's the change in internal energy during step two well it's still three halves NR delta T during step two, what's delta T during step two? Well P.V equals N R T pressure does not change only the volume changes so we have P delta V equals N R delta T so P2 delta V2 equals N R delta T2, NR delta T2 is this whole right portion so delta U2 is three halves P2 delta V2 which is three halves Pnot right the pressure for step two times once again the same change in pressure that we found here. So this is just 3Pnot Vnot so by the first law of thermodynamics Q during step two is just delta U 2 minus W which is three Pnot Vnot minus negative 2Pnot Vnot which is 5Pnot Vnot. So for the cycle sorry the heat the total heat input during the cycle is just the heat input during steps one and steps two because steps three and step four release heat so the amount of heat input is just during step one and step two, step one had three fourths Pnot Vnot and step two had five Pnot Vnot if we find the least common denominator this is three fourths Pnot Vnot plus this common denominator is four this is twenty over four Pnot Vnot so that's 23 over 4Pnot Vnot and what's the work done by the cycle we calculated it to be Pnot Vnot this means that the efficiency which is just the work over the amount of heat input is Pnot Vnot over 23 over 4 Pnot Vnot. Those Pnots Vnots cancel and finally.The efficiency is 4 over 23 now 4 over 23 is an exact answer and you can leave it like that if you want or you can approximate a number 0.174 which is 17.4 % so this engine actually has an incredibly low efficiency only 17.4 % other engines can have much much much higher efficiency. I showed a case in an earlier problem where a car not engine had an 80 % efficiency when it was placed between a reservoir of a 1000 Kelvin and a reservoir of 100 Kelvin this seventeen and a half percent efficiency sort of leaves a lot to be desired but this is an application of the first law of thermodynamics on heat engines and how to find the efficiency using a P.V diagram which can be very useful. Alright guys that wraps up this problem thanks for watching.

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Concept #1: Heat Engines and PV Diagrams

Example #1: Efficiency of a Four-Step Engine

The figure below shows the PV cycle for a heat engine that uses 2 moles of a monoatomic gas. The initial temperature is Ta = 300 K. The engine runs through 3 process: an isotherm, an isobar, and an isochore.(a) Find explicit values of the gas variables P, V, and T at all 3 points on the diagram(b) Calculate ΔU, W, and Q for each leg of the cycle(c) What is the work done by the engine in one cycle?(d) What is the engine's thermal efficiency?

A heat engine uses 1.3 g of hydrogen and follows the cycle shown in the figure below. a) Find the pressure, volume, and temperature of the hydrogen at points 1, 2 and 3.b) What is the thermal efficiency of this engine?

An engine uses 1.4 mol of a monoatomic ideal gas undergoing the cycle shown in the following figure. a) Determine T1, T2, and T3.b) Make a table showing ΔU, W, and Q for each step of the cycle. c) What is the engine's thermal efficiency?

The engine shown in the following figure uses 0.1 mol of a monoatomic ideal gas. What is the thermal efficiency of the engine if Vmax = 1741 cm3?

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