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Calorimetry Calculator

\( \Delta Q = m c \) \( \Delta T \)

\( C = \dfrac{\Delta Q}{m} \)\( \Delta T \)

\(m = \dfrac{\Delta Q}{c}\)\( \Delta T \)

\(T_i = \dfrac{\Delta Q}{m c-T_f}\)

\(T_f = \dfrac{\Delta Q}{mc + T_i}\)

\(t = m c\)\(\dfrac {\Delta T }{\Delta Q}\)

\(\Delta H = \dfrac{M \Delta Q}{mol}\)


The calorimetry calculator estimates the heat and energy that is released or absorbed by the chemical reaction. With this calculator, you can find the enthalpy change associated with a chemical reaction performed in a coffee cup calorimeter.

What Is Calorimetry?

The term is used to quantify the amount of heat that is transformed to and from the substance is referred as calorimetry.

Calorimetry calculations are based on the law of conservation of energy. There are two conditions to evaluate the heat energy that is as follows:

  • From the chemical reaction, the release of heat indicates that the reaction is exothermic. 
  • If the chemical reaction absorbs the heat then the calorimetry calculator displays that the reaction is endothermic. 

Calorimetry Formula:

By understanding the thermodynamics of chemical reactions the calorimetry formula helps to measure the energy content whether the reaction is exothermic or endothermic. 

$$ \text{Total heat energy} = Q = \Delta{Q_{1}} + \Delta{Q_{2}} + \Delta{Q_{3}}+ … + \Delta {Q_ {I}} $$

$$ \text{Total heat energy} = Q = {m_{1} } × c_{1} × \left(T_{final} – T_{initial}\right) + m_{2} × c_{2} × \left(T_{final} – T_{initial}) (2)\right) +… + m_{i} × c_{i} × \left(T_{final} – T_{initial}\right) $$

$$ \Delta Q = m c \Delta T $$ 


  • ΔQ _ Change in heat and energy  = Q2 - Q1
  • m _ Mass of the given body
  • c _ Heat capacity of an object
  • ΔT _ Rate of change of temperature = T2 - T1

How To Calculate Heat Capacity of Calorimeter?

In a coffee cup calorimetry, the calorimetry calculator estimates the enthalpy change in the chemical reaction. A better way to understand calorimetry problems can be demonstrated by an example below:


Let us suppose 0.5kg of ice is poured into the 2kg mercury that is in a bucket at 27°C on the other side the mercury has a temperature of 100°C and the temperature of ice is -25°C. The specific heat capacity of the ice is 1.999 (J/g.k) and mercury is 4.2 (J/g.k).

You need to evaluate the final temperature that is at the end of the reaction. 


Given Data: 

  • Mass of Ice = 0.5kg or 500g
  • Mass of Mercury = 2kg or 2000g
  • Initial temperature of Ice Ti2 = -25°C  + 273°C  = 248k
  • Initial temperature of Mercury Ti1 = 27°C + 273°C = 300k
  • Final Temperature of Mercury Tf2 = 100°C

To Find:

  • Final temperature of Ice Tf1 =?


$$ T_{f1} = \dfrac{-m_2c_2(T_{f2} - T_{i2})+T_{i1}}{m_1c_1} $$

Putting the values:

$$ T_{f1} = \dfrac{(-2000000)(4.2)(100-300)+(248)}{(500)(1.999)} $$

$$ T_{f1} = \dfrac{(-8400000)(-200)+(248)}{(999.5)} $$

$$ T_{f1} = \dfrac{(--1680000000)+(248)}{(999.5)} $$

$$ T_{f1} = \dfrac{(--1679999752)}{(999.5)} $$

$$ T_{f1} = -1680840.172 $$

What Are The Steps To Use Calorimetry Calculator?

To understand the working of a calorimetry calculator it is important to take into account the following points. Look at these:


  • Choose the type of reaction
  • Set the factor that you want to calculate
  • Put the mass with their appropriate unit 
  • Set the value of specific heat capacity by setting their unit 
  • Place the change in temperature ΔT
  • Tap “Calculate”


  • Specific heat capacity from the chemical reaction
  • The change in the temperature, energies, and masses of bodies 
  • Step-by-step calculations 

Concept of Enthalpy In Calorimetry Calculations:

A thermodynamic quantity that is equal to the total heat content of a system. It is equal to the internal energy of a system and the product of pressure and volume. It realizes  how much heat is available in the system  


Example: If water freezes into the ice some amount of energy is lost during this task. This is called enthalpy. 

According to the law of conservation of energy, the enthalpy change is equal to the transfer to the system. In essence, calorimetry focuses on heat whereas stoichiometry deals with the quantitative aspects of chemical reactions. 

You can also try a stoichiometry calculator to predict the amount of heat released or absorbed in a chemical reaction.   


What Is The Heat Capacity of an Object?

Heat capacity is the physical property of the matter and is defined as:

“The amount of heat that is required to raise the temperature of 1°C or 1 kelvin”. Joule per kelvin per kg (J/g.K) is the unit that is used to indicate the heat capacity of a body. 

Where Is Calorimetry Used In Industry?

In the pharmaceutical industry, calorimetry is used to design drugs and measure heat change. These are used to control the quality control and for the examination of metabolic rate. 

What Does Calorimetry Depend On?

The calorimetry depends on the conservation of the energy that tells us the energy neither be created nor destroyed but changes from one state to another 

Why Water Is Used In The Calorimetry?

Water is an excellent heat absorber and it has the highest specific heat. It means that it takes into account the maximum energy to enhance the temperature of water compared to other substances. 


From the source Wikipedia: Calorimetry, Classical calorimetric calculation of heat, Relation between classical calorimetric quantities, how to find heat capacity of the calorimeter.