Thermodynamics and Statistical Mechanics

Heat from the sun travels through space to the moon via electromagnetic radiation. When the sun's rays hit the moon's surface, they are absorbed and heat up the surface of the moon. However, the moon has no atmosphere to trap the heat, so temperatures fluctuate drastically between day and night.

The first law of thermodynamics requires that energy input must equal energy output plus energy accumulation. In this case that translates to;

430 J = 120 J + (internal energy change)

so

Internal energy change = 430 J - 120 J = +310 J (the internal energy increased by 310 Joules)

A solar powered air compressor is not a thermodynamic impossibility, but it may be challenging to design a system that efficiently converts solar energy into mechanical energy to compress air. It requires careful engineering to ensure that the system can capture and convert enough solar energy to meet the energy demands of compressing air. Additionally, the intermittent nature of solar energy may require energy storage solutions for continuous operation.

Thermal conductivity depends upon the nature/identity of the substance and upon

temperature. In some cases, such as wood, it depends upon the conduction heat transfer direction with respect to the material structure.

The Ideal Gas Law, equation PV = nRT relates the pressure to the constant R, where P is pressure, V is volume, n is number of moles, and T is temperature.

Boyle's Law provides a relationship between the volume of a gas and its pressure where temperature is constant. The equation is PV = k where P is the pressure of the gas, V is the volume of the gas, and k is a constant.

Charles' law states that the volume of a given mass of a gas, at constant pressure, is directly proportional to its temperature. V1/T1 = V2/T2

The three major modes of heat transfer are conduction, convection, and radiation. Conduction is the transfer of heat through a material by direct contact of particles. Convection involves the movement of fluids or gases to transfer heat. Radiation is the transfer of heat through electromagnetic waves.

1. Airplanes have streamlined shapes to reduce drag and improve aerodynamics.
2. Fish have streamlined bodies to move efficiently through water.
3. Cars often incorporate streamlined designs to enhance fuel efficiency and reduce wind resistance.
4. Speedboats are built with streamlined hulls to glide smoothly through water.
5. Bullet trains have streamlined profiles to decrease air resistance and achieve high speeds.

dU=q-w

where

dU is the differential change in internal energy

q is the differential quantity of heat added to a system

w is the differential quantity of work done by a system on its surroundings

Heat makes things hot.

Usable energy is inevitably used for productivity, growth and repair. In the process, usable energy is converted into unusable energy. Thus, usable energy is irretrievably lost in the form of unusable energy.

No. The second law still determines if a process will take place spontaneously. The first law does not say that if you drop a block of hot iron into a water bath that the iron can't absorb enough energy from the water to melt it while freezing the water as long as the energy absorbed by the iron matches the energy lost by the water. HOWEVER, the second law tells us this won't happen.

The thermal energy change of the system can be calculated using the first law of thermodynamics, which states that the change in internal energy of a system is equal to the heat added to the system minus the work done by the system. Therefore, the thermal energy change would be 100 J (heat added) - 60 J (work done) = 40 J.

Not at all. The First Law states that energy is conserved - you can't create energy out of nothing, or make it disappear. The Second Law distinguishes usable from unusable energy, and states that the amount of unusable energy will increase over time - but the total (usable plus unusable energy) will still remain constant.

Not at all. The First Law states that energy is conserved - you can't create energy out of nothing, or make it disappear. The Second Law distinguishes usable from unusable energy, and states that the amount of unusable energy will increase over time - but the total (usable plus unusable energy) will still remain constant.

Not at all. The First Law states that energy is conserved - you can't create energy out of nothing, or make it disappear. The Second Law distinguishes usable from unusable energy, and states that the amount of unusable energy will increase over time - but the total (usable plus unusable energy) will still remain constant.

Not at all. The First Law states that energy is conserved - you can't create energy out of nothing, or make it disappear. The Second Law distinguishes usable from unusable energy, and states that the amount of unusable energy will increase over time - but the total (usable plus unusable energy) will still remain constant.

Exothermic means that heat energy is given off from the reaction. In turn this means that the enthalpy (stored chemical energy) decreases. Best example of an exothermic reaction is combustion reactions (reacting with oxygen, or even more simply: burning). The opposite of exothermic is endothermic.

That's kind of a trick question. Specific heat - also known as "heat capacity" is the energy required to change the temperature by a fixed amount. In the case of an isothermal process, the temperature isn't changing.

Since specific heat is defined as (δH/δT), isothermal heat capacity would be (δH/δT)T which means, in English, the change in enthalpy with a change in temperature when the temperature isn't changing... you see the problem. If δT = 0, then δH/δT = ±∞ (positive if heat is added to the system to keep the temperature constant, negative if heat was removed to keep it isothermal)

You could write some equations such that the heat capacity becomes a term in the equation. What you will generally find though is that the heat capacity is multiplying a dT term and when dT is zero, that term drops out and heat capacity is irrelevant for the calculation.

An oversimplification of the second law of thermodynamics would state, "Everything cools down." Then the nature of living things would be the need to add energy to counter this cooling down. Humans add this energy by eating food and combining it with oxygen. Thus, the food and oxygen produces energy that can be lost to entropy.

Water droplets will start evaporating on contacting the pan bottom, and they will tend to "dance" on the produced steam.

Vc is the specific volume (volume per mole) at the critical point of a substance.

Vr is the "reduced volume" which is equal to the specific volume divided by the critical volume.

Vr = V/Vc

Many thermodynamic models correlate behavior of different substances in terms of their reduced volume. The principle of corresponding states indicates that substances at equal reduced pressures and temperatures have equal reduced volumes. This relationship is approximately true for many substances, but becomes increasingly inaccurate for large values of Pr. (Where Pr = P/Pc and Pc is the pressure at the critical point.)

The fluctuation theorem of statistical physics oversees this possibility, but the net result is the expected one. Some experiments with particles show local decrease in entropy. But, again, the net result is the expected one. To build a macro system which violates the law, it's just a matter of building a wall separating two regions of an isolated box filled with a gas. This wall should possess a special property: It allows the gas to pass in a single direction only. Such a system has an overnight capacity of realizing work internally. If external high entropy heat is allowed to enter the system, then work can be executed outside the system. The system "cleans" the input energy. Whoever builds this wall is eligible for a Nobel Prize.

Well the predictable pattern is when the warmer object always flows energy to the cooler until they both are the same temp

Only the simpler concepts of the 2nd law can be stated at a child's level. Many of them have no simple explanation because they involve equations that can only be written as differentials and integrals.

Some of the simple parts of it though are:

To warm up something cold, you have to use something that is warmer. To cool something down, you have to use something that is cooler.

No matter how hot they are, you can't just pull heat out of the air or water to run a machine; you have to have something cold for the heat to move into and then you might be able to get some work out a machine you put between the hot and the cold that can use some of the energy moving from the hot to the cold.

While energy is not created or destroyed according to the first law of thermodynamics, it can be converted from one form to another. The challenge lies in ensuring that energy remains usable and available in the desired form, without excessive losses or inefficiencies. Conservation efforts focus on reducing waste and maximizing the efficiency of energy conversion processes to minimize environmental impact and resource depletion.

No - to straighten a messy room requires work, and in the process energy is released as heat into the environment. The room may become more orderly, but the net effect on the universe is an increase in entropy because of the heat released.

If a source of heat energy starts radiating from a point and continues without stop the entropy around that point will never decrease. As sun is the endless heat energy radiating source and surrounding's of that is known as universe accepted by everybody. So this is the example for the statement ' the entropy of the universe can never decrease.'

True