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Or # Calorimetry Calculator

The tool will find all the parameters involved in a calorimetry reaction scheme.

$$\Delta Q = m c$$ $$\Delta T$$

$$C = \dfrac{\Delta Q}{m}$$$$\Delta T$$

$$m = \dfrac{\Delta Q}{c}$$$$\Delta T$$

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

$$T_f = \dfrac{\Delta Q}{mc + T_i}$$

$$t = m c$$$$\dfrac {\Delta T }{\Delta Q}$$

$$\Delta H = \dfrac{M \Delta Q}{mol}$$

Heat Energy ($$\Delta Q$$)

Mass (m)

Specific heat capacity (c)

Substance mass

Molar mass

Initial Temperature

Final Temperature

Change of Temperature ($$\Delta T$$)

Mass ($$m_1$$)

Mass ($$m_2$$)

Specific heat capacity ($$c_1$$)

Specific heat capacity ($$c_2$$)

Initial Temperature ($$T_{i1}$$)

Initial Temperature ($$T_{i2}$$)

Final Temperature ($$T_{f1}$$)

Final Temperature ($$T_{f2}$$)

Final Temperature ($$T_f$$)

Tfusion

Hfusion

Mass ($$m_1$$)

Mass ($$m_2$$)

Mass ($$m_3$$)

Specific heat capacity ($$c_1$$)

Specific heat capacity ($$c_2$$)

Specific heat capacity ($$c_3$$)

Initial Temperature ($$T_{i1}$$)

Initial Temperature ($$T_{i2}$$)

Initial Temperature ($$T_{i3}$$)

Final Temperature ($$T_{f1}$$)

Final Temperature ($$T_{f2}$$)

Final Temperature ($$T_{f3}$$)

Final Temperature ($$T_f$$)

$$T_{fusion}$$

$$\Delta H_{fusion}$$

Table of Content

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The calorimetry calculator estimates the heat energy released or absorbed in a chemical reaction. By knowing the change in the heat energy, we can determine whether the reaction is exothermic or endothermic.

## What Is Calorimetry?

“Calorimetry is the process of calculating the amount of heat energy released or absorbed in a chemical reaction”

When heat energy is released in a chemical reaction, then the chemical reaction is exothermic and a calorimetry calculator will indicate a positive value. On the other hand, if the heat energy is absorbed by the reaction, the reaction is endothermic and the calorimeter calculator will indicate a negative value.

### Unit of Calorimetry:

The calorimeter constant is usually presented in units of joules per degree Celsius (J/°C) or joules per Kelvin (J/K).

## How to Find the Heat Capacity of Calorimeter?

The total heat energy released in the chemical reaction is:

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

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

The amount of heat gained or lost can be calculated by the following equation.

$$\Delta Q = m c \Delta T$$

Where:

ΔQ = Heat change

m = mass of an object

The C = Heat capacity of an object (The amount of heat energy required to raise the temperature to 1 °C or 1 K)

ΔT = Change of temperature between the initial temperature and the final temperature

### Example:

Consider you have dropped 100 g of ice into 5kg of water at a temperature of 20 °C. Let’s assume the only materials exchanging heat or water and ice. The temperature of the ice was -25 °C, then find the final temperature of the system. The heat capacity of water and ice are 4.18 J/g.K and 2.05 J/g.K, respectively, and the heat of the fusion of water is 334 J/g.

#### Given:

Mass of water = 5 Kg

Mass of Ice = 100 g

The initial temperature of water = 20 °C + 273 = 293 K

Initial temperature of ice = -25 °C +273 = 248 K

The final temperature of water =?

#### Solution:

The calorimetry equation for the final temperature is:

$$\delta{Q_{1}}+\delta{Q_{2}}+\delta{Q_{3}}+\delta{Q_{4}} =$$

Putting in all the values

$$m_{ice}c_{ice}\left(T_{fusion}-T_{ice}\right)+m_{ice}\deltaH_{fusion}+m_{water}c_{water}\left(T_{f}-T_{fusion}\right)$$

Re-Arranging all the values of the final temperature as follows:

$$T_f = \dfrac{m_1c_1(T_{fusion} – T_{i1})+m_1H_{fusion}-m_1c_2T_{fusion}-m_2c_2T_{i2}}{-m_1c_2-m_2c_2}$$

Now by putting the values in the given equation.

$$T_f = \dfrac{(10)(25)(40-0.00027003080950275)+(10)(30)-(10)(50)(40)-(20)(50)(20)}{-(10)(50)-(20)(50)}$$

$$T_f = \dfrac{(10)(25)(39.99972996919)+(10)(30)-(10)(50)(40)-(20)(50)(20)}{-(10)(50)-(20)(50)}$$

$$T_f = \dfrac{(9999.9324922976)+(300)-(10000)-(20000)}{-(500)-(1000)}$$

$$T_f = \dfrac{(-19700.067507702)}{(-1500)}$$

The final temperature is given below:

$$T_f = 13.133K$$

The calorimetry problems can be used to find the initial or the final temperature of the substances when participating in a chemical reaction. The coffee cup calorimeter calculator can find the specific heat and the system’s enthalpy involved in a chemical change.

## Working of Calorimetry Calculator:

The calorimeter constant calculator is simple to use by following the instruction as under:

Input:

• Select the type of reaction and number of objects from respective drop-down lists
• Select if object 1 changes state or not
• Select the parameter to be calculated
• Enter all the required parameters in their designated fields
• Hit the calculate button

Output:

• Specific heat capacities, temperature changes, energies, and masses of objects in the reaction
• Enthalpy changes and isolation time of the calorimetry reaction

## FAQs:

### What Is the Latent Heat of the Fusion?

The latent heat of fusion is the amount of heat required to change the physical state of a substance from a solid to a liquid or gaseous state. The latent heat of a substance is specific and you can calculate the latent heat with the online calorimetry calculator

### What Is Enthalpy in Chemistry?

The enthalpy is the total content of heat energy of the whole system. It is equivalent to the system’s internal energy plus the product of the pressure or volume of the system. The enthalpy of a system is different at a particular pressure. The coffee cup calorimeter calculator can spot the change in enthalpy by the minor change in the pressure or volume of the system.

## References:

From the source of hem.libretexts.org: Calorimetry, Calculate Heat Capacity of Calorimeter

From the source of wikipedia.org: Calorimetry, Heat Calculation