1. What is the Calorimetry Equation?

The calorimetry equation (Q = -mcΔT) calculates the heat absorbed or released during a chemical reaction or physical change. It's fundamental in thermochemistry for measuring energy changes in processes.

2. How Does the Calculator Work?

The calculator uses the calorimetry equation:

Where:

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

Explanation: The negative sign indicates that heat released by the system is gained by the surroundings (exothermic) and vice versa for endothermic processes.

3. Importance of Calorimetry Calculation

Details: Calorimetry calculations are essential for determining enthalpy changes, studying reaction thermodynamics, and designing industrial processes.

4. Using the Calculator

Tips: Enter mass in kg, 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: Why is there a negative sign in the equation?
A: The negative sign indicates the direction of heat flow - from the system to surroundings (exothermic) when Q is negative.

Q2: What are typical specific heat values?
A: Water has c = 4186 J/kg·K, while metals typically range from 100-1000 J/kg·K.

Q3: When is calorimetry used?
A: Common applications include determining heats of reaction, measuring nutritional calories, and studying phase changes.

Q4: What are limitations of this equation?
A: Assumes no heat loss to surroundings and constant specific heat capacity over the temperature range.

Q5: How does this relate to enthalpy?
A: At constant pressure, the heat change (Q) equals the enthalpy change (ΔH) of the system.