Login
Copyright

Calorimetry: Measuring Heat Transfer and Heat Capacity

An error occurred trying to load this video.

Try refreshing the page, or contact customer support.

Coming up next: Predicting the Entropy of Physical and Chemical Changes

You're on a roll. Keep up the good work!

Take Quiz Watch Next Lesson
 Replay
Your next lesson will play in 10 seconds
  • 0:03 Introduction to Calorimetry
  • 0:33 Units of Heat
  • 2:10 Specific Heat Capacity
  • 4:41 Calorimetry & Heat…
  • 7:52 Lesson Summary
Add to Add to Add to

Want to watch this again later?

Log in or sign up to add this lesson to a Custom Course.

Login or Sign up

Timeline
Autoplay
Autoplay
Create an account to start this course today
Try it free for 5 days!
Create An Account

Recommended Lessons and Courses for You

Lesson Transcript
Instructor: Nicola McDougal

Nicky has taught a variety of chemistry courses at college level. Nicky has a PhD in Physical Chemistry.

This video lesson explains the technique of calorimetry used to measure heat transfer in chemical reactions. You will see how different materials have different specific heat capacities. You will learn how to carry out heat calculations using a simple equation.

Introduction to Calorimetry

Have you ever read the food label of your hamburger and seen how many calories your burger contains? Ever wondered how they know this? The technique used is calorimetry. This is the science of measuring heat transfer when a substance absorbs or gives out heat. A calorimeter is a device that we use to experimentally determine the heat associated with a chemical reaction. We will discuss two types of calorimeters later in the lesson.

Units of Heat

Before we start to measure heat transfer, let me introduce you to two common units of heat or energy you will come across. Firstly, the calorie; this is defined as the amount of energy, or heat, required to raise the temperature of one gram of water by one Celsius degree. The calorie is an old unit, but is still commonly used today. The calorie used to describe the amount of energy in food is actually a kilocalorie (which is 1,000 calories). So, our 500-calorie burger is really a 500,000-calorie burger!

The SI unit for heat is called the joule and is defined in terms of the calorie: 1 cal = 4.184 J. So, now our burger is equal to 500 kilocalories, 500,000 calories, and over 2 million joules! It is important that you can easily convert between calories and joules, so let us do an example now.

Express 28.4 J of heat (or energy) in units of calories. Our conversion factor is 1 cal = 4.184 J. So, 28.4 J * 1 cal / 4.184 J = 6.79 cal. Notice we have set up the calculation so we can cancel the units to leave us with calories. And, don't forget to check for significant figures.

Specific Heat Capacity

In your everyday lives, you probably know that different substances respond differently when heated. It is important to know how materials respond to heat! You also need to think about how much of the material you have. How does the amount of the substance affect the energy required to heat it? Well, I'm sure you can see that heating up a large hamburger takes longer than heating up a small one. The amount of heat energy needed to change the temperature of a substance depends on three things:

  1. The amount of the substance you are heating (which is the number of grams) - the larger hamburger takes longer to increase in temperature compared to the small one.
  2. The amount of temperature change (the number of degrees) - the higher you want the temperature to go the longer you need to heat it.
  3. The identity of the substance.

Now, we have already observed that different substances react differently when heated. It is also true that some substances require relatively large amounts of energy to change their temperatures, while others require relatively little. We call these differences 'heat capacity.' Specific heat capacity is the amount of energy required to change the temperature of one gram of a substance by one Celsius degree.

Here, we can see a table of specific heat capacities of common substances. The higher the number, the more energy is needed to change the temperature of the substance:

Substance Specific Heat Capacity (J/g degrees C)
Water (l) 4.184
Beeswax 3.4
Wool 1.26
Aluminum 0.89
Iron 0.45
Bone 0.44
Carbon (diamond) 0.52
Silver 0.24
Gold 0.13

Notice that water has a very high specific heat capacity compared to the other substances. This is hugely important and is the reason why lakes and oceans are relatively slow to respond to heating or cooling compared to the land around it. Now we have the three factors that affect how much heat is needed to change the temperature. We can represent this by the following equation:

Q = s * m * change in temperature, where Q = heat (or energy), s is specific heat capacity, m is mass in grams, and delta T is the change in temperature in degrees Celsius.

In the next section, we will use this equation to do some heat calculations.

Calorimetry and Heat Calculations

Let us return to the way we measure heat transfer using calorimetry. There are many different types of calorimeters, but I am only going to talk about the two you are most likely to come across. The first one is called the 'Bomb Calorimeter.' Here, a chemical reaction is performed inside of a metal container that is immersed in water. All of the energy released by the reaction goes into heating the water.

Our newly learned heat equation is used to figure out the heat of reaction. We know the specific heat capacity of the water, we know how much water we have, and we can measure the change in temperature. This is exactly the way nutritionists work out the energy content of food. The food is burned in the chamber and the temperature of the water is measured. The higher the temperature rises, the more heat is given out, and the more calories the food contains.

The other type of calorimeter you may encounter in the school or college lab is the 'Coffee Cup Calorimeter.' The setup is much simpler, with just an insulated Styrofoam cup, stirrer, and a thermometer. The chemical reaction takes place in the coffee cup and the same calculations can be made. So, let us finish with a couple of simple heat calculations.

Question 1: 'How much energy does it take to heat 120 grams of water from 20 to 45°C?'

To unlock this lesson you must be a Study.com Member.
Create your account

Register for a free trial

Are you a student or a teacher?
I am a teacher

Unlock Your Education

See for yourself why 30 million people use Study.com

Become a Study.com member and start learning now.
Become a Member  Back

Earning College Credit

Did you know… We have over 95 college courses that prepare you to earn credit by exam that is accepted by over 2,000 colleges and universities. You can test out of the first two years of college and save thousands off your degree. Anyone can earn credit-by-exam regardless of age or education level.

To learn more, visit our Earning Credit Page

Transferring credit to the school of your choice

Not sure what college you want to attend yet? Study.com has thousands of articles about every imaginable degree, area of study and career path that can help you find the school that's right for you.

Create an account to start this course today
Try it free for 5 days!
Create An Account
Support