Thermodynamics and Statistical Mechanics

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

A tri-atomic molecule should have 3 vibrational degrees of freedom (one for each "end" atom vibrating on its bond with the central atom and one for the flexing of the bonds like scissors opening and closing). If it is non-linear, it should also have a three rotational degrees of freedom. All molecules (including a triatomic one) will have 3 degrees of freedom for translational motion. All totaled, it will have 3+3+3 = 9 degrees of freedom. Note that this does not address the question of independence of the degrees of freedom - for example - if the two "end" atoms are identical, not all the rotational degrees of freedom are independent.

Entropy tends to increase in a system.

The change in internal energy is 205 cal. The change in internal energy (ΔU) is given by the formula ΔU = Q - W, where Q is the heat added (500 cal) and W is the work done by the gas (500 J = 119.6 cal). Therefore, ΔU = 500 cal - 119.6 cal = 380.4 cal.

If the liquid surface tension is less than or equal to the critical surface tension of a surface, you would expect the liquid to spread out and wet the surface. This is because the liquid will be able to overcome the cohesive forces holding it together and adhere to the surface.

Temperature is proportional to the average kinetic energy of the molecules of a gas substance, as a good example. Hence, when temperature rises, the molecules move faster, they hit the walls of containers more (hence raising pressure), which may increase the volume (depending on the container - eg. plastic container vs a balloon). If the volume is not able to be increased, the pressure remains at that level.

PV=nRT

P=pressure

V=volume

n=number of moles

R=a constant

T=temperature

With the above equation, you can see that by decreasing T, either/both of pressure and/or volume must change so that the left side of the equation equals the right.

The first law states that energy can neither be created nor destroyed; it can only change form. Photosynthesis is an example of this. The energy of sunlight is converted via photosynthesis to energy stored in the chemical bonds of the molecules making up the plant.

At those conditions, the ideal gas law should be quite good for calculating pressure. Solving the ideal gas law for pressure:

P = nRT/V

= (1/6.02214129×1023 mol−1)(8.3144621×106 cm3 Pa K−1 mol−1)(3 K)/(1 cm3)

= 4.14195x10-17 Pa

Heat transfer generally follows the laws of thermodynamics, including the first law (conservation of energy) and the second law (entropy). Heat transfer can occur through conduction, convection, or radiation, with the direction of heat flow determined by temperature differences and the properties of the materials involved.

The first law of thermodynamics (law of energy conservation) states that energy cannot be created or destroyed, only transferred or converted. The second law of thermodynamics states that the entropy (disorder) of an isolated system always increases over time, reflecting the tendency of systems to move towards thermodynamic equilibrium.

Kathmandu is at a very high elevation in the Himalayas, where the atmospheric pressure is lower than at sea level. This causes water to boil at a temperature less than 100 oCelsius.

Three thermodynamic properties are internal energy (U), temperature (T), and entropy (S). The relationship between them is described by 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, expressed as ΔU = Q - W. The Second Law of Thermodynamics quantifies the relationship between entropy, heat transfer, and temperature as dS = δQ/T, where dS is the change in entropy, δQ is heat transferred, and T is the temperature.