By default, you can only calculate for two reactants/products. Click the advanced mode button to include more compounds in the reaction.
This enthalpy calculator will help you calculate the change in enthalpy of a reaction. Read on to learn how to calculate enthalpy and what is its definition. We will also explain the difference between endothermic and exothermic reaction, as well as provide you with an example of calculations.
Check out our ideal gas law calculator, too!
What is enthalpy?
Enthalpy measures the total energy of a thermodynamic system - either in the form of heat or volume multiplied by pressure. It is a state function, depending only on the equilibrium state of a system.
The more interesting quantity is the change of enthalpy - the total energy that was exchanged within a system. It is a simplified description of the energy transfer (energy is in the form of heat or work done during expansion).
Endothermic or exothermic reaction?
There are two main types of thermodynamic reactions: endothermic and exothermic. An endothermic reaction causes absorption of heat from the surroundings. An exothermic one releases heat to the surroundings.
Both these reaction types cause energy level differences and therefore differences in enthalpy. All you need to remember for the purpose of this calculator is:
- If the reaction is endothermic, change in enthalpy is positive, as heat is gained (absorbed from the surroundings).
- If the reaction is exothermic, change in enthalpy is negative, as heat is lost (released to the surroundings).
Enthalpy, be definition, is the sum of heat absorbed by the system and the work done when expanding:
H = Q + pV
where Q stands for internal energy, p for pressure and V for volume.
If you want to calculate the change in enthalpy, though, you need to consider two states - initial and final. We will assume that the pressure is constant while the reaction takes place. Then, the change in enthalpy is actually
ΔH = (Q₂ - Q₁) + p * (V₂ - V₁)
ΔH = ΔQ + p * ΔV
- Q₂ and V₂ are the internal energy and volume of the products of the reaction;
- Q₂ and V₂ are the internal energy and volume of the reactants;
- p is the constant pressure;
- ΔQ is the change in internal energy;
- ΔV is the change in volume;
- ΔH is the change in enthalpy.
Standard enthalpy of formation table and definition
For more particular problems, we can define the standard enthalpy of formation of a compound, denoted as
ΔH°f. It's the change in enthalpy,
ΔH, during the formation of one mole of the substance in its standard state,
° (pressure 10⁵ Pa = 1 bar and temperature 25°C = 298.15 K), from its pure elements,
The standard enthalpy of formation formula for a reaction is as follows:
ΔH°reaction = ∑ΔH°f(products) - ∑ΔH°f(reactants)
ΔH°reactionis the standard enthalpy change of formation expressed in kJ;
∑ΔH°f(products)is the sum of the standard enthalpies of formation of the products expressed in kJ/mol; and
∑ΔH°f(reactants)is the sum of the standard enthalpies of formation of the reactants expressed in kJ/mol.
If you're paying attention, you might have observed that
∑ΔH°f(reactants) have different units than
ΔH°reaction. This is because you need to multiply them by the number of moles, i.e., the coefficient before the compound in the reaction. We'll show you later an example that should explain it all.
But before that, you may ask "How to calculate standard enthalpy of formation for each compound?" The most straightforward answer is to use the standard enthalpy of formation table! Here's an example one:
The symbols in the brackets indicate the state: s - solid, l - liquid, g - gas, and aq - dissolved in water. If you need the standard enthalpy of formation for other substances, select the corresponding compound in the enthalpy calculator's drop-down list. We included all the most common compounds!
Let's practice our newly obtained knowledge using the above standard enthalpy of formation table. For example, we have the following reaction:
2 SO₃(g) → 2 SO₂(g) + O₂(g)
What is the enthalpy change in this case? We sum
O₂(g) and subtract the
SO₃(g). Remember to multiply the values by corresponding coefficients!
ΔH°reaction = 2 mol * (−296.83 kJ/mol) + 1 mol * 0 kJ/mol - 2 mol * (−395.72 kJ/mol)
Notice that the coefficient units
mol eliminates the
mol in the denominator, so the final answer is in
ΔH°reaction = 197.78 kJ
That's it! Still, isn't our enthalpy calculator a quicker way than all of this tedious computation?
How to calculate the enthalpy of a reaction? The enthalpy calculator
The enthalpy calculator has two modes. You can calculate the enthalpy change from the reaction scheme or by using the enthalpy formula. If you select the former:
- Look at the reaction scheme that appeared at the top of the calculator. Do you need an additional reactant/product (C or F)? If so, click the
- Fill in the fields in the Reactants section. You need to provide the coefficient before the compound and select your substance from the drop-down list (they're ordered alphabetically). If you can't find a right one, select the Custom option and enter the standard enthalpy of formation in kJ/mol (if you don't have this on hand, check some online reference tables, like this one at Chemistry LibreTexts).
- Do the same thing for the Products.
- Verify the reaction scheme below and read the result. That's the standard enthalpy change of formation for your reaction!
- Optionally, check the standard enthalpy of formation table (for your chosen compounds) we listed at the very bottom.
If you want to calculate the enthalpy change from the enthalpy formula:
- Begin with determining your substance's change in volume. Let's assume your liquid expanded by 5 liters.
- Find the change in the internal energy of the substance. Let's say your substance's energy increased by 2000 J.
- Measure the pressure of the surroundings. We will assume 1 atmosphere.
- Input all of these values to the equation
ΔH = ΔQ + p * ΔVto obtain the change in enthalpy:
ΔH = 2000 J + 1 atm * 5 l = 2000 J + 101,325 Pa * 0.005 m³ = 2506.63 J
- You can also open the
advanced modeof our enthalpy calculator to find the enthalpy based on the initial and final internal energy and volume.