Side A2: Temperature, Ideal Gases & Thermodynamics

understand that (thermal) energy is transferred from a region of higher temperature to a region of lower temperature

understand that regions of equal temperature are in thermal equilibrium

understand that a physical property that varies with temperature may be used for the measurement of temperature and state examples of such properties, including the density of a liquid, volume of a gas at constant pressure, resistance of a metal, e.m.f. of a thermocouple

understand that the scale of thermodynamic temperature does not depend on the property of any particular substance

convert temperatures between kelvin and degrees Celsius and recall that T / K = θ / °C + 273.15

understand that the lowest possible temperature is zero kelvin on the thermodynamic temperature scale and that this is known as absolute zero

define and use specific heat capacity

define and use specific latent heat and distinguish between specific latent heat of fusion and specific latent heat of vaporisation

understand that amount of substance is an SI base quantity with the base unit mol

use molar quantities where one mole of any substance is the amount containing a number of particles of that substance equal to the Avogadro constant NA

understand that a gas obeying pV ∝ T, where T is the thermodynamic temperature, is known as an ideal gas

recall and use the equation of state for an ideal gas expressed as pV = nRT, where n = amount of substance (number of moles) and as pV = NkT, where N = number of molecules

recall that the Boltzmann constant k is given by k = R / NA

state the basic assumptions of the kinetic theory of gases

explain how molecular movement causes the pressure exerted by a gas and derive and use the 1 1

understand that the root-mean-square speed cr.m.s. is given by <c 2 > 1

compare pV = 3 Nm<c2> with pV = NkT to deduce that the average translational kinetic energy of a 3

understand that internal energy is determined by the state of the system and that it can be expressed as the sum of a random distribution of kinetic and potential energies associated with the molecules of a system

relate a rise in temperature of an object to an increase in its internal energy

recall and use W = p∆V for the work done when the volume of a gas changes at constant pressure and understand the difference between the work done by the gas and the work done on the gas

recall and use the first law of thermodynamics ∆U = q + W expressed in terms of the increase in internal energy, the heating of the system (energy transferred to the system by heating) and the work done on the system