5.1.1
Temperature |
(a) thermal equilibrium |
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| (b) absolute scale of temperature (i.e. the thermodynamic scale) that does not depend on property of any particular substance. |
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(c) temperature measurements both in degrees Celsius (°C) and in kelvin (K) |
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| (d) T(K) ≈ θ(°C) + 273 |
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5.1.2
Solid, liquid and gas |
(a) solids, liquids and gases in terms of the spacing, ordering and motion of atoms or molecules |
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(b) simple kinetic model for solids, liquids and gases |
(c) Brownian motion in terms of the kinetic model of matter and a simple demonstration using smoke particles suspended in air |
(d) internal energy as the sum of the random distribution of kinetic and potential energies associated with the molecules of a system |
(e) absolute zero (0 K) as the lowest limit for temperature; the temperature at which a substance has minimum internal energy |
(f) increase in the internal energy of a body as its temperature rises |
| (g) changes in the internal energy of a substance during change of phase; constant temperature during change of phase. |
5.1.3
Thermal properties of materials |
(a) specific heat capacity of a substance;
the equation
E = mcΔθ
Estimating specific heat capacity, using method of mixture. |
E = mcΔθ |
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| (b) (i) an electrical experiment to determine the specific heat capacity of a metal or a liquid |
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(b) (ii) techniques and procedures used for an electrical method to determine the specific heat capacity of a metal block and a liquid |
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(c) specific latent heat of fusion and specific latent heat of vaporisation;
E = mL |
E = mL |
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(d) (i) an electrical experiment to determine the specific latent heat of fusion and vaporisation |
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(d) (ii) techniques and procedures used for an electrical method to determine the specific latent heat of a solid and a liquid. |
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5.1.4
Ideal gases |
(a) amount of substance in moles; Avogadro constant NA equals 6.02 × 1023 mol–1 |
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(b) model of kinetic theory of gases assumptions for the model:
- large number of molecules in random, rapid motion particles (atoms or molecules) occupy negligible volume compared to the volume of gas
- all collisions are perfectly elastic and the time of the collisions is negligible compared to the time between collisions
- negligible forces between particles except during collision |
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| (c) pressure in terms of this model.
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Explanation of pressure in terms of Newtonian theory. |
| (d) (i) the equation of state of an ideal gas pV = nRT, where n is the number of moles |
pV = nRT |
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(d) (ii) techniques and procedures used to investigate
PV = constant (Boyle's law) and
T/P = constant |
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(d) (iii) an estimation of absolute zero using variation of gas temperature with pressure |
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(e) the equation
where N is the number of particles (atoms or molecules) and c2 is the mean square speed |
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Derivation of this equation is not required.... but you might find it interesting to look at! Click here |
(f) root mean square (r.m.s.) speed; mean square speed |
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Learners should know about the general characteristics of the Maxwell-Boltzmann distribution. |
(g) the Boltzmann constant;
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k = R/NA |
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(h) pV = NkT;
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pV = NkT |
Learners will also be expected to know the derivation of this equation from
and pV = nkT
See here |
(i) internal energy of an ideal gas. |
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