Calculating Joules of Heat

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<h3>Calculating Joules of Heat</h3>

Back in the early 19th century, a British brewer and physicist named James Joule demonstrated that heat and mechanical work were two forms of the same thing: energy. His discovery earned him a lasting place in science history; today, the unit in which energy and heat are measured is named after him. You can easily calculate the amount of heat absorbed or released by an object as long as you know three things: its mass, the change in its temperature, and the type of material it’s made from.

TL;DR (Too Long; Didn’t Read)

**TL;DR**



Calculate the joules of heat absorbed or released using the formula:

Heat = mass of object × change in temperature × specific heat capacity of material

1. Find the Specific Heat Capacity

Look up the specific heat capacity of your material. The first link under the resources section lists the specific heat capacities of common solids; the second link lists the heat capacities of common liquids. Use the value under the column with units of kJ/kg K. Note that kJ stands for kilojoule, one thousand joules, while kg is a kilogram, a unit of mass, and K is Kelvin, a unit of temperature. A change of one degree Kelvin is equal to a change of one degree Centigrade.

2. Find the Change in Temperature

Subtract the starting temperature of your object from its final temperature to find the change in temperature. If your change in temperature is in Fahrenheit, convert it to degrees Kelvin by using the following formula:



(Temperature in Fahrenheit – 32) × 5/9 = temperature in Celsius

3. Perform the Calculation

Multiply the change in temperature by the specific heat capacity and the mass of your object. This will give you the heat lost or gained in joules.

Example: If 10 kilograms of water are heated from 10 degrees Celsius to 50 degrees Celsius, how much energy (in joules) did they absorb?



Answer: The specific heat capacity of water is (roughly) 4.184 kilojoules / kg K.

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(10 kg) × (40 degrees Celsius temperature change) × (4.184 kJ / kg K) = 1673.6 kilojoules.

Dave Pennells

By Dave Pennells

Dave Pennells, MS, has contributed his expertise as a career consultant and training specialist across various fields for over 15 years. At City University of Seattle, he offers personal career counseling and conducts workshops focused on practical job search techniques, resume creation, and interview skills. With a Master of Science in Counseling, Pennells specializes in career consulting, conducting career assessments, guiding career transitions, and providing outplacement services. Her professional experience spans multiple sectors, including banking, retail, airlines, non-profit organizations, and the aerospace industry. Additionally, since 2001, he has been actively involved with the Career Development Association of Australia.