Calorimetry Calculator
Calculate heat transfer, temperature changes, and energy exchange in thermal systems
Calorimetry Analysis
Object 1
Object 2
Heat Exchange Results
Object 1 Heat Change
Object 2 Heat Change
Common Substances
Water
c = 4.18 kJ/kg·K
H = 334 kJ/kg
Ice
c = 2.05 kJ/kg·K
H = 334 kJ/kg
Aluminum
c = 0.9 kJ/kg·K
Copper
c = 0.38 kJ/kg·K
Iron
c = 0.45 kJ/kg·K
Silver
c = 0.24 kJ/kg·K
Gold
c = 0.13 kJ/kg·K
Lead
c = 0.13 kJ/kg·K
Mercury
c = 0.14 kJ/kg·K
Glass
c = 0.84 kJ/kg·K
Calorimetry Formulas
Heat Change
Q = m × c × ΔT
Sensible heat transfer
Phase Change
Q = m × H
Latent heat transfer
Energy Conservation
ΣQ = 0
Total heat change is zero
Enthalpy Change
ΔH = (M × Q) / m
Chemical reaction enthalpy
Understanding Calorimetry
What is Calorimetry?
Calorimetry is the science of measuring heat transfer during chemical reactions, phase transitions, or temperature changes. It's based on the law of conservation of energy, which states that energy cannot be created or destroyed in an isolated system.
Types of Heat Transfer
- •Sensible Heat: Heat that causes temperature change
- •Latent Heat: Heat absorbed or released during phase changes
- •Reaction Heat: Heat involved in chemical reactions
Key Principles
Energy Conservation: Q₁ + Q₂ + Q₃ + ... = 0
Heat Equation: Q = mcΔT
Phase Change: Q = mH
Temperature Change: ΔT = T_final - T_initial
Applications
- Material Analysis: Determining specific heat capacities
- Chemical Reactions: Measuring enthalpy changes
- Phase Studies: Analyzing melting and boiling points
- Quality Control: Testing material properties
Problem Solving Steps
Heat Exchange Problems
- 1. Identify all objects and their properties
- 2. Write heat equation for each object
- 3. Apply conservation of energy
- 4. Solve for the unknown variable
- 5. Check that energy is conserved
Example:
Mix 0.5 kg copper (100°C) with 1.0 kg water (20°C). Find the final temperature.
Solution: T_final = (m₁c₁T₁ + m₂c₂T₂) / (m₁c₁ + m₂c₂)
Chemical Reaction Analysis
- 1. Measure solution temperature change
- 2. Calculate heat absorbed by solution
- 3. Determine reaction heat (opposite sign)
- 4. Calculate enthalpy per mole
- 5. Classify as exo- or endothermic
Coffee-Cup Calorimeter:
Measures enthalpy changes in solution reactions at constant pressure.
ΔH = (Molar Mass × Q_solution) / mass_substance