Lecture 1 1 Overview
... other quantities are not continuous, but discrete. The governing equation is the Schrödinger equation. The state of any system is described by the wave function, which is the solution of the Schrödinger equation. Quantum chemistry typically deals with solving the Schrödinger equation for single m ...
... other quantities are not continuous, but discrete. The governing equation is the Schrödinger equation. The state of any system is described by the wave function, which is the solution of the Schrödinger equation. Quantum chemistry typically deals with solving the Schrödinger equation for single m ...
Thermodynamics
... number of moles is often a helpful method. Letter C refers to the molar specific heat capacity. Use Kelvin as the unit for temperature. Cp and Cv must be used depending on constant pressure or volume conditions. ...
... number of moles is often a helpful method. Letter C refers to the molar specific heat capacity. Use Kelvin as the unit for temperature. Cp and Cv must be used depending on constant pressure or volume conditions. ...
Lecture 5
... the metal are relatively large, and thus the associated energy are passed along the poker, from atom to atom during collisions between adjacent atoms. ...
... the metal are relatively large, and thus the associated energy are passed along the poker, from atom to atom during collisions between adjacent atoms. ...
Section 12.1 Temperature and Thermal Energy
... Temperature – measure of hotness of an object on a quantitative scale. In gases it is proportional to the average kinetic energy of the particles. It does NOT depend on the number of particles in a body. Thermal Equilibrium – state in which the rate of energy flow between 2 or more bodies is equal a ...
... Temperature – measure of hotness of an object on a quantitative scale. In gases it is proportional to the average kinetic energy of the particles. It does NOT depend on the number of particles in a body. Thermal Equilibrium – state in which the rate of energy flow between 2 or more bodies is equal a ...
noneq
... justifies this result. b. Find the change in temperature, pressure and entropy if the volume increases from V0 to V1 in the condition of (a). c. Repeat (b) if the piston is moving very slowly, i.e. an adiabatic process. Adiabatic expansion of the universe The universe is pervaded by a black body rad ...
... justifies this result. b. Find the change in temperature, pressure and entropy if the volume increases from V0 to V1 in the condition of (a). c. Repeat (b) if the piston is moving very slowly, i.e. an adiabatic process. Adiabatic expansion of the universe The universe is pervaded by a black body rad ...
Thermodynamics and the aims of statistical mechanics
... the scale; and (ii) the zero point. For example, inspired by Boyle’s Law that for gases at fixed temperature, p and V are inversely proportional, we might define a scale determined by the change of volume at constant pressure (or vice versa). (It turns out that as p → 0, different gases give the sam ...
... the scale; and (ii) the zero point. For example, inspired by Boyle’s Law that for gases at fixed temperature, p and V are inversely proportional, we might define a scale determined by the change of volume at constant pressure (or vice versa). (It turns out that as p → 0, different gases give the sam ...
Thermal Physics Tutorial
... Note: when a bubble rises from the bottom of a beer glass, the pressure experience by this bubbles decreases. Assuming there is no change in the temperature, there will be an increase in the volume of the bubble. However, to have its volume doubled solely due to decreases in pressure, the beer glass ...
... Note: when a bubble rises from the bottom of a beer glass, the pressure experience by this bubbles decreases. Assuming there is no change in the temperature, there will be an increase in the volume of the bubble. However, to have its volume doubled solely due to decreases in pressure, the beer glass ...
Chapter 3
... The thermodynamic state of a system can be characterized by its properties that can be classified as measured, fundamental, or derived properties. We want to develop relationships to relate the changes in the fundamental and derived properties in terms of the measured properties that are directly ac ...
... The thermodynamic state of a system can be characterized by its properties that can be classified as measured, fundamental, or derived properties. We want to develop relationships to relate the changes in the fundamental and derived properties in terms of the measured properties that are directly ac ...
1 - Moodle Ecolint
... its centre, as shown in the diagram above. The block is heated for time t and the maximum temperature change recorded is Δθ. The ammeter and voltmeter readings during the heating are I and V respectively. The specific heat capacity is best calculated using which one of the following expressions? ...
... its centre, as shown in the diagram above. The block is heated for time t and the maximum temperature change recorded is Δθ. The ammeter and voltmeter readings during the heating are I and V respectively. The specific heat capacity is best calculated using which one of the following expressions? ...
3 - CFD - Anna University
... • Internal energy is the sum of all microscopic forms of energy of a system. • Internal energy will be highest for gas phase and minimum for the solid phase ...
... • Internal energy is the sum of all microscopic forms of energy of a system. • Internal energy will be highest for gas phase and minimum for the solid phase ...
Equipartition theorem
In classical statistical mechanics, the equipartition theorem is a general formula that relates the temperature of a system with its average energies. The equipartition theorem is also known as the law of equipartition, equipartition of energy, or simply equipartition. The original idea of equipartition was that, in thermal equilibrium, energy is shared equally among all of its various forms; for example, the average kinetic energy per degree of freedom in the translational motion of a molecule should equal that of its rotational motions.The equipartition theorem makes quantitative predictions. Like the virial theorem, it gives the total average kinetic and potential energies for a system at a given temperature, from which the system's heat capacity can be computed. However, equipartition also gives the average values of individual components of the energy, such as the kinetic energy of a particular particle or the potential energy of a single spring. For example, it predicts that every atom in a monatomic ideal gas has an average kinetic energy of (3/2)kBT in thermal equilibrium, where kB is the Boltzmann constant and T is the (thermodynamic) temperature. More generally, it can be applied to any classical system in thermal equilibrium, no matter how complicated. The equipartition theorem can be used to derive the ideal gas law, and the Dulong–Petit law for the specific heat capacities of solids. It can also be used to predict the properties of stars, even white dwarfs and neutron stars, since it holds even when relativistic effects are considered.Although the equipartition theorem makes very accurate predictions in certain conditions, it becomes inaccurate when quantum effects are significant, such as at low temperatures. When the thermal energy kBT is smaller than the quantum energy spacing in a particular degree of freedom, the average energy and heat capacity of this degree of freedom are less than the values predicted by equipartition. Such a degree of freedom is said to be ""frozen out"" when the thermal energy is much smaller than this spacing. For example, the heat capacity of a solid decreases at low temperatures as various types of motion become frozen out, rather than remaining constant as predicted by equipartition. Such decreases in heat capacity were among the first signs to physicists of the 19th century that classical physics was incorrect and that a new, more subtle, scientific model was required. Along with other evidence, equipartition's failure to model black-body radiation—also known as the ultraviolet catastrophe—led Max Planck to suggest that energy in the oscillators in an object, which emit light, were quantized, a revolutionary hypothesis that spurred the development of quantum mechanics and quantum field theory.