Knowledge-13 TP

Cards (35)

  • Internal energy is the sum of the randomly distributed kinetic energies and potential energies of the particles in a body.
  • The internal energy of an object can be:
    • increase healing it , or by doing work on it
    • reduced by cooling it or if work is done by it.
  • According to the first law of thermodynamics , when work is done on or by an object and/or energy is transferred to or from it by heating.
  • when changing state:
    • its temperature stays constant
    • the kinetic energy of its particles does not change
    • its internal energy changes because the potential energy of its particles changes as forces between them change and bonds between them are made or broken.
  • Specific latent heat of fusion of a substance is the amount of energy needed to change 1kg of it from solid to liquid without a change in temperature.
  • Specific latent heat of vaporization of a substance is the amount of energy needed to change 1kg of a liquid to gas without a change in temperature.
  • The specific heat capacity of a substance c is the amount of energy needed to raise the temperature of 1kg of a substance by 1 kelvin or degree.
  • if a substance is heated using an electrical heater , the energy transferred to it can be calculated using:
    • E = IVt
    • E = electrical energy supplied in joules
    • I = current in A
    • V = p.d in V
    • t = heating time in s
  • Continuous flow heating is the process of heating a fluid by having it flow continuously over a heater.
    • energy transfer per second = power of heating = mass flow per second x specific heat capacity x change in temp.
  • one mole of any substance contains 6.02 x 10^23 particles of that substance.
  • the molar mass of a substance s the mass of one mol of that substance in kgmol^-1.
  • The molar mass of an element in g equal to its relative atomic or relative molecular mass , depending on whether their particles are atoms or molecules.
  • The molar mass of a compound in g can be calculated by adding in the relative atomic masses of its constituent atoms shown in its chemical formula.
  • Absolute zero is defined as 0 K on the kelvin scale.
  • To convert between kelvin and Celsius you add 273.15 to celsius.
  • Boyles law states that for a fixed mass of gas at constant temperature the pressure p and the volume V are inversely proportional :
    • p proportional to 1/v or pv
  • The pressure law states that for a fixed mass of gas at constant volume the pressure p and absolute temperature T are directly proportional:
    • p is proportional to temperature.
    • plotting data for p against t gives a straight line through the origin.
  • Charles law states that for a fixed mass of gas at constant pressure , the volume V and absolute temperature T are directly proportional.
  • The gas laws describe the behavior of gases using following quantities and units:
    • volume V in m^3
    • pressure p in Nm^-2 or pascals Pa
    • temperature T in K
    • number of atoms or molecules N
    • amount of gas n in mol
  • An ideal gas is a theoretical gas that obeys the experimental gas laws at all pressures and temperatures. The internal energy of a gas is only dependent on the kinetic energy of its particles ; they do not have any potential energy.
  • The energy transferred to increase or decrease the volume of a gas at a constant pressure is given by:
    • W = p x change in volume
  • Brownian motion is the random motion of small particles suspended in a fluid.
  • Brownian motion provided evidence for the existence of atoms. Albert Einstein showed mathematically that the jiggling motion of particles suspended in a fluid could be caused by random collisions with much smaller particles that are in constant random motion.
  • pressure is caused by the change in momentum of the molecules colliding with the container walls or surfaces.
  • temperature is proportional to the average kinetic energy of the molecules.
  • Boyles law:
    the pressure of a gas at constant temp is increased by reducing its volume because the gas molecules travel a smaller distance between collisions with the container walls, so there are more collisions per second and a greater pressure.
  • The pressure law:
    the pressure of a gas at constant volume is increased by raising its temperature because this raises the average kinetic energy of the molecules.
  • Charles law:
    the volume of a gas at constant pressure is increased by raising its temperature because this raises the average kinetic energy of the molecules.
  • According to kinetic theory , an ideal gas considering of N identical molecules , each of mass m, in a container of volume V , the pressure of gas is given by the kinetic theory question:
    • pV = 1/3 Nm (crms)^2
  • To derive the kinetic theory equation , the following assumptions about an ideal gas are made:
    • all molecules are identical and the volume of one is negatable compared with the volume of gas.
    • molecules are in continual , random motion
    • newtons law can be applied to the molecules and there are enough molecules to apply statistical laws.
    • collisions between particles and walls are perfectly elastic.
  • With a cubic container:
    if a molecule collides with the right-hand wall:
    • x-component of its velocity ,c , reverses and becomes -c but cy and c z remain the same
    • x-component of its momentum reverses and becomes -mc
    • change in the momentum of the particle is -mc -mc = -2mc
  • With a cubic container:
    • time t between successive impacts with this wall is the total distance to the opposite wall and back divided by the x-component of the velocity
    • t = 2l / c
    • number of collisions per second = 1/t = c/2l
  • With a cubic container:
    • force on the molecule is equal to its rate of change on momentum , which is equal to the momentum charge per collisions multiplied by the number of collisions per second.
    • according to newtons third law , the force on the molecule is equal to opposite to the force on the wall so force on wall
    • F = mc^2 / l
  • For a cubic container:
    • pressure on wall = mc^2 / volume
  • The ideal gas equation and the kinetic theory equation are equivalent to each other and show that:
    • average molecular kinetic energy of particles in a gas are directly proportional to its temperature in K