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Thermal Physics Thermal Concepts

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Temperature The absolute temperature scale (measured in Kelvin and with a minimum value of zero Kelvin) is used in physics calculations. (Where a change of one Kelvin equals a change of one degree Celsius) (i.e. The KE of the particles is directly proportional to the temperature) Kelvin Temperature = Celsius Temperature + 273 The absolute (Kelvin) temperature of a body is a measure of the average amount of kinetic energy that each of its molecules have.

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Thermal Equilibrium When two bodies are at the same temperature as each other, they are in thermal equilibrium. This leads to the Zeroth law of thermodynamics: If two bodies A and B are separately in thermal equilibrium with body C, they are also in thermal equilibrium with each other and thus have the same temperature. LinkLink – Thermal equilibriumLinkLink – Heating a solid

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Heat and Internal Energy We know that work can be done on a body, causing energy to be transferred to it mechanically (by a force moving through a distance). The only other way that energy can be transferred is by heat transfer: Note: It is common to mistakenly say that a body contains heat energy. This is wrong. In this sense we need to refer to internal energy: Heat is the energy that will flow between two bodies that are not in thermal equilibrium and that thus have different temperatures.

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Note: While the potential energy of the particles results from their position and the forces between them, the kinetic energy of the particles is not only from their vibration. They may also have KE because they are spinning, moving from place to place etc. The many different ways in which a particle has energy are sometimes known as degrees of freedom. In any body, the internal energy of the body is equal to the sum of the kinetic energy and potential energy of all the particles. molecules

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Temperature and Internal Energy - Link

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Moles and The Avogadro Number The number of molecules in a substance is measured in moles. Just like a dozen means twelve of something, one mole means 6.02 x 10 23 molecules of something. One mole of a substance contains the same number of molecules as in 12 grams of Carbon-12. The Avogadro number (N A ) is equal to the number of molecules in 12 grams of Carbon-12 ( N A = 6.02 x 10 23 ) The molar mass (M) is the mass in grams of one mole of a particular substance. Note: the mass number of an element is equal to the molar mass for atoms of an element. E.g. One mole of Nitrogen atoms will have mass 14g.

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E.g.1 The mass number of Helium is 4. How many atoms are in 4kg of Helium? A.Mass no. is 4 so molar mass is 4g. 4000 g / 4g = 1000 moles 1000 x N A = (1 x 10 3 ) x (6.02 x 10 23 ) = 6.02 x 10 26 atoms E.g.2 The molar mass of iron atoms is 56 g mol -1 and its density is 7.9 g cm -3. a. Find the mass of one atom of Iron. b. Calculate the number of iron atoms in one cubic metre of iron.

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E.g. 2 The molar mass of iron atoms is 56 g mol -1 and its density is 7.9 g cm -3. a. Find the mass of one atom of Iron. b. Calculate the number of iron atoms in one cubic metre of iron. a. If one mole of atoms has mass 56g then one atom will have mass = 56 N A = 56 (6.02 x 10 23 ) = 9.3 x 10 -23 g b. One cm 3 has mass = 7.9 g So one m 3 has mass = 7.9 x (100x100x100) g = 7.9 x 10 6 g So no. of iron atoms per m 3 = 7.9 x 10 6 / 9.3 x 10 -23 = 8.5 x 10 28 atoms

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Further calculations with moles The number of moles of a substance (n) can be determined form the total mass (m) divided by the molar mass (mass per mole, M), usually both measured in grams: Similarly if you knew the total number of molecules (N), you could find the number of moles (n) from… n = m M n = N N A

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E.g. a.Calculate the number of moles of oxygen atoms in 40g of oxygen. N = m / M = 40 / 16 = 2.5 moles b. Calculate the number of moles of oxygen molecules (O 2 ) in 40g of oxygen. N = m / M = 40 / 32 = 1.25 moles c.A sample of fluorine gas contains 20 x 10 23 atoms of fluorine. Calculate the number of moles present. N = N / N A = 20 x 10 23 / 6.02 x 10 23 = 3.3 moles

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Unit 4 – The Mole Honors Chemistry Part 1.

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