# 7.5: Stoichiometry Calculations Using Enthalpy

Learning Objective

• Perform stoichiometry calculations using energy changes from thermochemical equations.

In Chapter 5 - Stoichiometry and the Mole, we related quantities of one substance to another in a chemical equation by performing calculations that used the balanced chemical equation; the balanced chemical equation provided equivalences that we used to construct conversion factors. For example, in the balanced chemical equation2H2(g) + O2(g) → 2H2O(ℓ)

we recognized the equivalences

2 mol H2 ⇔ 1 mol O2 ⇔ 2 mol H2O

where ⇔ is the mathematical symbol for "is equivalent to." In our thermochemical equation, however, we have another quantity-energy change:

2H2(g) + O2(g) → 2H2O(ℓ) ΔH = −570 kJ

This new quantity allows us to add another equivalence to our list:

2 mol H2 ⇔ 1 mol O2 ⇔ 2 mol H2O ⇔ −570 kJ

That is, we can now add an energy amount to the equivalences-the enthalpy change of a balanced chemical reaction. This equivalence can also be used to construct conversion factors so that we can relate enthalpy change to amounts of substances reacted or produced.

Note that these equivalences address a concern. When an amount of energy is listed for a balanced chemical reaction, what amount(s) of reactants or products does it refer to? The answer is that relates to the number of moles of the substance as indicated by its coefficient in the balanced chemical reaction. Thus, 2 mol of H2 are related to −570 kJ, while 1 mol of O2 is related to −570 kJ. This is why the unit on the energy change is kJ, not kJ/mol.

For example, consider the thermochemical equation

H2(g) + Cl2(g) → 2HCl(g) ΔH = −184.6 kJ

The equivalences for this thermochemical equation are

1 mol H2 ⇔ 1 mol Cl2 ⇔ 2 mol HCl ⇔ −184.6 kJ

Suppose we asked how much energy is given off when 8.22 mol of H2 react. We would construct a conversion factor between the number of moles of H2 and the energy given off, −184.6 kJ:

$8.22\not{mol\, H_{2}}\times \frac{-184.6\, kJ}{1\not{mol\, H_{2}}}=-1520\, kJ$

The negative sign means that this much energy is given off.

Example $$\PageIndex{1}$$:

Given the thermochemical equation

N2(g) + 3H2(g) → 2NH3(g) ΔH = −91.8 kJ

how much energy is given off when 222.4 g of N2 reacts?

Solution

The balanced thermochemical equation relates the energy change to moles, not grams, so we first convert the amount of N2 to moles and then use the thermochemical equation to determine the energy change:

$222.4\not{g\, N_{2}}\times \frac{1\not{mol\, N_{2}}}{28.00\not{g\, N_{2}}}\times \frac{-91.8\, kJ}{1\not{mol\, N_{2}}}=-729\, kJ$

Exercise $$\PageIndex{1}$$

Given the thermochemical equation

N2(g) + 3H2(g) → 2NH3(g) ΔH = −91.8 kJ

how much heat is given off when 1.00 g of H2 reacts?

−15.1 kJ

Like any stoichiometric quantity, we can start with energy and determine an amount, rather than the other way around.

Example $$\PageIndex{1}$$:

Given the thermochemical equation

N2(g) + O2(g) → 2NO(g) ΔH = 180.6 kJ

if 558 kJ of energy are supplied, what mass of NO can be made?

Solution

$558\not{kJ}\times \frac{2\not{mol\, NO}}{180.6\not{kJ}}\times \frac{30.0\, g\, NO}{1\not{mol\, NO}}=185\, g\, NO$

Exercise $$\PageIndex{1}$$

How many grams of N2 will react if 100.0 kJ of energy are supplied?

N2(g) + O2(g) → 2NO(g) ΔH = 180.6 kJ

15.5 g

Chemistry Is Everywhere: Welding with Chemical Reactions

One very energetic reaction is called the thermite reaction. Its classic reactants are aluminum metal and iron(III) oxide; the reaction produces iron metal and aluminum oxide:

2Al(s) + Fe2O3(s) → Al2O3(s) + 2Fe(s) ΔH = −850.2 kJ

When properly done, the reaction gives off so much energy that the iron product comes off as a liquid. (Iron normally melts at 1,536°C.) If carefully directed, the liquid iron can fill spaces between two or more metal parts and, after it quickly cools, can weld the metal parts together.

Thermite reactions are used for this purpose even today. For civilian purposes, they are used to reweld broken locomotive axles that cannot be easily removed for repair. They are used to weld railroad tracks together. Thermite reactions can also be used to separate thin pieces of metal if, for whatever reason, a torch doesn't work.

Fig. 7.5.1 Thermite mixture

A small clay pot contains a thermite mixture. It is reacting at high temperature in the photo and will eventually produce molten metal to join the railroad tracks below it.

Key Takeaway

• The energy change of a chemical reaction can be used in stoichiometry calculations.

Exercise $$\PageIndex{1}$$

1. Write the equivalences that this balanced thermochemical equation implies.PCl3(g) + Cl2(g) → PCl5(g) ΔH = −87.9 kJ
2. Write the equivalences that this balanced thermochemical equation implies.

2SO3(g) → 2SO2(g) + O2(g) ΔH = 197.9 kJ
3. How many kilojoules are given off when 17.8 mol of CH4(g) react?

CH4(g) + 2O2(g) → CO2(g) + 2H2O(ℓ) ΔH = −890.1 kJ
4. How many kilojoules are absorbed when 0.772 mol of N2(g) reacts?

N2(g) + 2NO(g) → 2N2O(g) ΔH = 73.8 kJ
5. How many kilojoules are absorbed when 23.09 mol of C6H6(ℓ) are formed?

6C(s) + 3H2(g) → C6H6(ℓ) ΔH = 49.0 kJ
6. How many kilojoules are given off when 8.32 mol of Mg react?

2Mg(s) + O2(g) → 2MgO(s) ΔH = −1,213 kJ
7. Glucose is the main fuel metabolized in animal cells:

C6H12O6 + 6O2 → 6CO2 + 6H2O ΔH = −2,799 kJ

How much energy is given off when 100.0 g of C6H12O6 react?

8. Given the thermochemical equation

2Al(s) + Fe2O3(s) → Al2O3(s) + 2Fe(s) ΔH = −850.2 kJ

how much energy is given off when 288 g of Fe are produced?

9. Given the thermochemical equation

2CO2(g) → 2CO(g) + O2(g) ΔH = 566 kJ

how much energy is absorbed when 85.2 g of CO2 are reacted?

10. Given the thermochemical equation

2Na+(aq) + SO42−(aq) → Na2SO4(s) ΔH = 819.8 kJ

how much energy is absorbed when 55.9 g of Na+(aq) are reacted?

11. NaHCO3 decomposes when exposed to heat:

2NaHCO3(s) → Na2CO3(s) + CO2(g) + H2O(ℓ) ΔH = 91.5 kJ

What mass of NaHCO3 is decomposed by 256 kJ?

12. HgO decomposes when exposed to heat:

2HgO(s) → 2Hg(ℓ) + O2(g) ΔH = 181.6 kJ

What mass of O2 can be made with 100.0 kJ?

13. For the thermochemical equation

Fe2O3(s) + 3SO3(g) → Fe2(SO4)3 (s) ΔH = −570.2 kJ

what mass of SO3 is needed to generate 1,566 kJ?

1. For the thermochemical equation

H2(g) + Br2(ℓ) → 2HBr(g) ΔH = −72.6 kJ

what mass of HBr will be formed when 553 kJ of energy are given off?