Thermochemistry The branch of chemistry concerned with the quantities of heat evolved or absorbed during chemical reactions.

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Presentation transcript:

Thermochemistry The branch of chemistry concerned with the quantities of heat evolved or absorbed during chemical reactions

Example Problem 15-1 Calculating Heat A silver bar with a mass of 250.0 g is heated from 22.0°C to 68.5°C. How much heat does the silver bar absorb? Use the equation for heat. q = c x m x ∆T

The temperature change is the difference between the final temperature and the initial temperature. ∆T = 68.5°C - 22.0°C = 46.5°C The specific heat of silver is 0.235 J/(g°C). Substitute the known values to solve for the amount of heat absorbed.

q = 0.235 J/(g°C) x 250.0 g x 46.5°C = 2730 J

How much heat does a 23.0-g ice cube absorb as its temperature increases from -17.4°C to 0.0°C? Give the answer in both joules and calories.

1674 J or 400 cal

A sample of an unknown metal has a mass of 120.7 g. As the sample cools from 90.5°C to 25.7°C, it releases 7020 J of energy. What is the specific heat of the sample?

Specific heat 0.898 J/(g°C). The specific heat is very close to the value for aluminum.

A 15.6-g sample of ethanol absorbs 868 J as it is heated. If the initial temperature of the ethanol was 21.5°C, what is the final temperature of the ethanol?

44.3°C

Heat changes that occur during chemical and physical processes can be measured using an insulated device called a calorimeter. In one type of calorimeter, the temperature change of a known mass of water is used to determine the amount of energy released or

absorbed by a system undergoing a chemical or physical change.