1. What is Calorimetry?

Calorimetry is the science of measuring the heat of chemical reactions or physical changes. The fundamental equation q = m × c × ΔT relates heat energy to mass, specific heat capacity, and temperature change.

2. How Does the Calculator Work?

The calculator uses the calorimetry equation:

Where:

• \( q \) — Heat energy (Joules)
• \( m \) — Mass of the substance (kg)
• \( c \) — Specific heat capacity (J/kg·K)
• \( \Delta T \) — Temperature change (Kelvin)

Explanation: The equation shows that heat transfer depends on the mass of the substance, its ability to absorb heat (specific heat capacity), and the temperature difference.

3. Importance of Calorimetry

Details: Calorimetry is essential in thermodynamics, chemistry, and engineering for determining heat changes in reactions, designing heating/cooling systems, and studying material properties.

4. Using the Calculator

Tips: Enter mass in kilograms, specific heat capacity in J/kg·K, and temperature change in Kelvin. All values must be valid (mass > 0, specific heat > 0).

5. Frequently Asked Questions (FAQ)

Q1: What units should I use?
A: For consistent results, use kg for mass, J/kg·K for specific heat, and Kelvin for temperature change.

Q2: Can I use Celsius instead of Kelvin?
A: Yes, because ΔT is the same in Celsius and Kelvin (1°C change = 1K change).

Q3: What are typical specific heat values?
A: Water: 4186 J/kg·K, Aluminum: 900 J/kg·K, Iron: 450 J/kg·K.

Q4: What if the temperature decreases?
A: A negative ΔT indicates heat release (exothermic process), resulting in negative q (heat lost).

Q5: How accurate is this calculation?
A: This assumes perfect conditions. Real systems may have heat losses to the environment.