Calorimetry Calculator
Solve thermodynamics problems with ease. Support for specific heat, final temperature, mass, and bomb calorimetry calculations.
Substance Properties
Conditions
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Enter values to compute unknown variables.
Mastering Heat Transfer
Calorimetry is the science of measuring heat flow. Whether you're determining the energy content of food or the specific heat of a mystery metal, our tool handles the math so you can focus on the chemistry.
Exothermic vs Endothermic
Positive q (+): Heat absorbed (Endothermic). Temperature drops.
Negative q (-): Heat released (Exothermic). Temperature rises.
Specific Heat Capacity
The amount of energy required to raise 1 gram of a substance by 1°C. Water has a high specific heat (4.18 J/g°C).
System vs Surroundings
In calorimetry, we assume q_system = -q_surroundings. Heat lost by the reaction is gained by the water.
The Core Equation
For most non-combustion experiments (like mixing solutions or adding a hot metal to water), we use the "Coffee Cup" assumption: pressure is constant.
Bomb Calorimetry
For combustion reactions, we use a rigid container called a "Bomb Calorimeter" (constant volume). Here, the heat capacity of the entire device is used.
Common Specific Heat Capacities
| Substance | Specific Heat (J/g°C) | State |
|---|---|---|
| Water (Liquid) | 4.184 | Liquid |
| Aluminum | 0.897 | Solid |
| Iron | 0.449 | Solid |
| Copper | 0.385 | Solid |
| Ethanol | 2.44 | Liquid |
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Frequently Asked Questions
What is the formula for calorimetry?
The fundamental equation for constant-pressure calorimetry (coffee cup) is q = mcΔT, where 'q' is heat energy, 'm' is mass, 'c' is specific heat capacity, and 'ΔT' is the change in temperature.
How does a bomb calorimeter differ from a coffee cup calorimeter?
A Coffee Cup Calorimeter operates at constant pressure (measuring enthalpy change, ΔH), ideal for solution reactions. A Bomb Calorimeter operates at constant volume (measuring internal energy change, ΔE), used for combustion reactions.
What is the specific heat of water?
The specific heat capacity of liquid water is approximately 4.184 J/g°C (or 1 cal/g°C). This high value means water resists temperature changes well, making it excellent for calorimetry.
Why is my heat (q) negative?
A negative 'q' value indicates an exothermic process, where the system releases heat to the surroundings (temperature rises). A positive 'q' means an endothermic process (heat absorbed).
How do I find the final temperature?
To find the final temperature (Tf), rearrange the equation: Tf = (q / mc) + Ti. Ensure you use the correct sign for 'q' depending on whether heat is gained or lost.
Can I use this calculator for metals?
Yes! Select the 'Find Specific Heat' mode or choose a metal from the substance list (like Aluminum or Copper) to solve for heat transfer in metal blocks.
What assumes are made in simple calorimetry?
We typically assume: 1) The calorimeter itself absorbs no heat (or a negligible amount). 2) No heat is lost to the outside air (perfect insulation). 3) The solution has the same specific heat and density as pure water.
How do I calculate the calorimeter constant?
The calorimeter constant (C_cal) is found by combusting a known standard (like benzoic acid) and measuring ΔT. Then, C_cal = q_known / ΔT.
What units should I use?
Standard scientific units are: Mass in grams (g), Temperature in Celsius (°C) or Kelvin (K), and Specific Heat in J/g°C. The result 'q' will be in Joules (J).
Is ΔT the same in Celsius and Kelvin?
Yes! Since the magnitude of 1 degree Celsius is identical to 1 Kelvin, the change in temperature (ΔT) is exactly the same in both scales.