6.3 Heat Capacity and Calorimetry

• The formula for heat capacity is Q
• Match the property with its relationship:

  Heat Capacity ↔️ More heat to raise temperature

  Temperature Change ↔️ Greater heat absorbed/released
• What are the units for specific heat capacity?

  J/g°C or J/gK
• What is molar heat capacity defined as?

  Heat to raise 1 mole by 1 degree
• What is molar heat capacity defined as?

  Heat to raise 1 mole by 1°C
• The molar heat capacity of water is higher than that of copper

  True
• In a constant-volume calorimeter, the volume is constant
• What is heat capacity defined as?

  Heat to raise 1 substance by 1°C
• What is specific heat capacity defined as?

  Heat to raise 1 gram by 1°C
• Water vapor has a lower specific heat capacity than liquid water

  False
• The variable 'n' in the molar heat capacity formula represents the number of moles


  True
• Molar heat capacity allows for comparing thermal properties of substances on a per-mole basis

  True
• A bomb calorimeter measures heat at constant volume
• The formula for heat capacity is Q
• Solids generally have low specific heat capacity compared to liquids


  True
• In the formula $Q =$$C \Delta T$, Q represents the heat absorbed or released
• What is heat capacity defined as?

  Heat to raise temperature
• Higher heat capacity requires more heat to raise the temperature of a substance by 1 degree.


  True
• The formula for specific heat capacity is mc
• Match the state of matter with its example:

  Solid ↔️ Copper

  Liquid ↔️ Water

  Gas ↔️ Water vapor
• What are the units for molar heat capacity?

  J/mol·°C or J/mol·K
• What does molar heat capacity help compare across substances?

  Thermal properties per mole
• What is the basic principle of calorimetry?

  Heat released equals heat exchanged
• A higher heat capacity means less heat is needed to raise the temperature

  False
• Match the state of matter with its typical specific heat capacity:

  Solids ↔️ Generally low

  Liquids ↔️ Intermediate

  Gases ↔️ High
• The heat absorbed or released is calculated using the formula Q
• What does 'ΔT' represent in the molar heat capacity formula?

  Change in temperature
• What is calorimetry in the context of chemistry?

  Measuring heat exchange
• A constant-pressure calorimeter is often used for reactions in solutions


  True
• The formula for specific heat capacity is Q
• What is the formula for calculating the heat absorbed or released in terms of heat capacity and temperature change?

  $Q =$$C \Delta T$
• Specific heat capacity varies for different states of matter.


  True
• What is the specific heat capacity of water in J/g°C?

  4.18
• Match the state of matter with its typical specific heat capacity range:

  Solids ↔️ Generally low

  Liquids ↔️ Intermediate

  Gases ↔️ High
• The specific heat capacity formula includes the mass of the substance in grams
• What is the formula for calculating heat in a constant-volume calorimeter?

  $Q =$$C_{cal} \Delta T$
• What are the two main types of calorimeters?

  Constant-volume and constant-pressure
• The formula for heat capacity is Q = C ΔT
• Arrange the states of matter in order of increasing specific heat capacity:

  1️⃣ Solids

  2️⃣ Liquids

  3️⃣ Gases
• Calorimetry is used to measure the heat released or absorbed during chemical reactions