Calorimetry and Enthalpy

Question 1

Calorimetry

Answer 1

• Science of measuring heat
• Based on observing the temperature change when a body absorbs or releases energy as heat

Question 2

Calorimeter

Answer 2

A device that can be used to measure thermal energy changes in a chemical reaction

Question 3

Specific Heat Capacity

Answer 3

• Quantity of thermal energy required to raise the temp of 1 gram of a substance by 1℃

Question 4

What’s the SI unit for specific heat capacity?

Answer 4

J/g℃

Question 5

What does high specific heat capacity mean?

Answer 5

The substance requires a larger amount of thermal energy to raise the temp and take a longer time to cool

Question 6

What does low specific heat capacity mean?

Answer 6

The substances takes less thermal energy to raise the temp and is quicker to cool down

Question 7

2 Parts of value “q”

Answer 7

1. Magnitude
2. Sign

Question 8

Magnitude

Answer 8

Calculated value

Question 9

Sign

Answer 9

Indicates the type of thermochemical reaction

Question 10

Enthalpy Definition

Answer 10

• Sum of internal energy
• Product of pressure and volume

Question 11

What happens when a process occurs at a constant pressure?

Answer 11

The heat involved is equal to the change in enthalpy

Question 12

Molar Enthalpy Definition

Answer 12

• Enthalpy change associated with a physical, chemical or nuclear change
• Involving one mole of a substance

Question 13

Note about enthalpy of neutralization

Answer 13

It can be written per mole of the base or acid

Question 14

4 ways to represent enthalpy changes:

Answer 14

1. Thermochemical equation with energy terms
2. Thermochemical equation with delta H values
3. Molar enthalpies
4. Potential energy diagrams