Heat

CALORIMETRY (return to CONTENTS)


HEAT INVOLVED IN CHANGES OF TEMPERATURE (return to start of page)
(sometimes called ‘sensible heat’)

Heat capacity


We see later, from the definition of a kelvins (K), that a temperature change of 10C = a temperature change of 1K.
Thus, the unit of heat capacity can be expressed as J0C-1 or JK-1

Specific heat capacity, c

The term ‘specific’ here means ‘per unit mass’, which means per kg, in SI units (though we often also use 'per gram').


SI unit: J/(kg 0C) º Jkg-1 0C-1 or J/(kgK) º Jkg-1 K-1

Rearranging, we get:

It is not essential to put the ‘D ’ in, and some prefer to write the equation as:


Example

The temperature of a 500g body rises from 150C to 200C.

a) How much heat is absorbed?
b) What is the heat capacity of the body?
(c = 400 J/(kg 0C)

Example

A 1kg piece of aluminium at 800C is immersed in 2kg of water at 150C. Assuming that no heat is lost to the surroundings, what will be the final temperature of the water?
(for Al, c = 908 J kg-1K-1; for water, c = 4200 J kg-1K-1)

Example

An electric kettle contains 1.5kg of water at 210C. To bring the water to the boil takes 3 minutes 46 seconds. Determine:

  1. the heat absorbed by the water
  2. the power of the electric element (recall that power (W) = energy (J)/time (s))
(for water c = 4200 J/(kg 0C)

Determination of specific heat capacity


HEAT INVOLVED IN CHANGES OF STATE (OR PHASE) (return to start of page)
(called ‘latent heat’)

There are three familar states of matter - solid, liquid and gas (or vapour). Many substances (e.g. water) can change from one state to another:

Suppose that a piece of ice, initially at –500C, is continuously slowly heated. An ‘ideal’ graph of temperature against time (not drawn to scale) would look like:

Changes of phase occur at fixed temperatures. We know that water melts (and freezes) at 00C and boils at 1000C. On the graph this means that we get flat sections during the changes of phase – as the temperatures are fixed. But the sample is being steadily heated all the time. This means that during a change of phase, all the heat supplied is used to bring about the change, and none is used to raise the temperature.

The heat involved in a change of state is called latent or ‘hidden’ heat because it does not ‘reveal’ itself as a change in temperature.

Definitions

Specific latent heat of fusion, Lf

Specific latent heat of vaporisation, Lv

Example

Fifty grams of ice is at 00C. How much total heat is needed to change it to steam at 1000C?
For ice Lf = 330 J/g; for water c = 4.2 J/(g0C) and Lv = 2300 J/g

There are three separate events:



VAPOURS (return to start of page)

Saturated vapour pressure

If a liquid is placed in a closed container, as above, molecules will escape from the liquid (evaporate) to become vapour molecules. Also, molecules in the vapour are moving in all directions, and some will re-enter the liquid. Eventually a state of dynamic equilibrium will be reached, at which:
When this state is reached, the vapour is said to be ‘saturated’, and the pressure it exerts is called its saturated vapour pressure (‘SVP’). Thus, If the above container were heated, more molecules would escape from the liquid, increasing the pressure of the vapour - a new dynamic equilibrium would be established at the higher temperature. Thus, SVP rises with temperature.

For water:

Note: A gas below a certain temperature, called its critical temperature, is called a vapour. A vapour can be liquified by increasing the pressure on it without changing its temperature. In the previous diagram, if the system were in equilibrium at a certain temperature, and then the container were compressed a little, enough vapour would liquify to keep the number of vapour molecules per cm3, and therefore the vapour density and pressure, constant.

Boiling

Boiling occurs at a particular temperature, and consists of the formation of bubbles of vapour throughout a liquid.

For a bubble to exist:


Thus, the boiling point of a liquid is the temperature at which its SVP equals the external pressure - and this is 1000C for water, as shown in the previous graph.

Evaporation

When a liquid evaporates it changes to vapour without reaching its boiling point.

The molecules in a liquid are in constant motion. Those near the surface can actually jump out of the liquid. Most will fall back, but some will escape to become vapour molecules. This is evaporation.

A pool of water evaporates most quickly (and clothes on a line dry most rapidly) when:

  1. it's sunny
  2. it's breezy
  3. there is little water vapour in the atmosphere (low humidity)
The sunshine gives molecules near the surface of a liquid extra kinetic energy ('KE') and so they can jump further out of the liquid. If it is breezy molecules jumping out of the liquid are simply blown away.

Cooling by evaporation

The body makes use of this 'cooling by evaporation' – sweat evaporates, taking heat from the body.

The refrigerator

The pipe contains a volatile liquid (E.g. Freon) – ‘volatile’ meaning it has a low boiling point (below 300C), so it readily vaporises.   Evaporation and boiling compared
(return to start of page)

(return to CONTENTS)

©

 

A Level Physics - Copyright © A C Haynes 1999 & 2004