M4Q5: Heat and Stoichiometry


The section explores how heat is an intrinsic component of physical and chemical changes. This section includes worked examples, sample problems, and a glossary.

Learning Objectives for Heat and Stoichiometry

| Key Concepts and Summary | Glossary | End of Section Exercises |

Reactions and Energy

Every physical and chemical change involves energy changes as well. For example, when water is boiled and evaporated, heat must be added to the liquid water to form gaseous water. In this example, the process is endothermic, meaning that it requires energy.

H2O(ℓ) + energy  ⟶  H2O(g)

Conversely, when liquid water freezes to form ice, heat is lost during this process. In this example, the process is exothermic, meaning that it releases energy.

H2O(ℓ)  ⟶  H2O(s) + energy

Like other quantities in balanced chemical equations, energy scales with the amount of reactants used and products formed. We can examine the combustion and electrolysis of water (two chemical changes) to see this scaling.

Demonstration: Energy can be released in the form of sound, light, and heat

Set up. Combustion of hydrogen gas in the presence of oxygen is an exothermic process. This demonstration shows the combustion of a balloon filled with hydrogen gas and oxygen gas.

Explanation. The combustion of the hydrogen and oxygen gases causes an explosion that releases energy. This energy can be observed in the forms of sound, light, and heat. When more hydrogen gas is used in the second explosion, the explosion releases even more energy.

Intuitively, one would predict that if we ignited a larger balloon filled with more hydrogen and oxygen that the explosion would be larger.  In chemistry terms, more energy would be released. Conversely, if we ignited a balloon with less hydrogen and oxygen then the explosion would be smaller. Again, in chemistry terms, less energy would be released. In other words, the energy scales with reaction stoichiometry.

2 H2(g) + O2(g)  ⟶  2 H2O(ℓ) + energy

One can carefully quantify this energy released. When two moles of hydrogen gas combust in the presence of one mole of oxygen gas, then two moles of liquid water are formed and 483.6 kJ of energy are released.

2 H2(g) + O2(g)  ⟶  2 H2O(ℓ) + 483.6 kJ

If we double the amount of reactants, then we double the products, including the amount of energy released:

4 H2(g) + 2 O2(g)  ⟶  4 H2O(ℓ) + 967.2 kJ

Electrolysis of liquid water to form hydrogen and oxygen is the reverse chemical reaction to the combustion. The amount of energy is the same, but it is a reactant in the chemical equation instead of a product.

2 H2O(ℓ) + 483.6 kJ  ⟶  2 H2(g) + O2(g)

Demonstration: Electrolysis of water requires energy

Set up. In this demonstration, electrolysis is performed on a solution of water that has been slightly acidified with H2SO4. The sulfuric acid acts as the electrolyte in this demonstration, carrying the charge between the anode and cathode. A DC voltage is applied to two electrodes, labeled “DC (-)” and “DC (+)”. These are the anode (negative electrode) and cathode (positive electrode), respectively. The following image explains the different parts of the apparatus that you will see in the video.

A screenshot of the demonstration is shown and the parts of the electrolysis setup are labeled. There is an energy source in the lower left. Two inverted burets are clamped on a ring stand side by side. The burets are filled with a solution of water and sulfuric acid. A positive electrode is inserted into the bottom of the right buret, and a negative electrode is inserted into the bottom of the left buret. A bridge near the bottom of the burets connects the two burets and acidified water enters the apparatus at the bridge. The electrodes are connected to the energy source. Gas will collect at the top of the burets during the electrolysis. Tubes connected to the stems of the burets will be used to collect samples.

When the energy source is turned on, you will see small bubbles appear in the two columns of solution. These bubbles are filled with H2 and O2 gas. These bubbles will float upward and gather at the top of the columns. We can then collect samples of the gas and ignite them to show that they are indeed H2 and O2 gas.

Prediction. Do you predict more H2 or more Ogas will be produced?

Explanation. At the frame that is labeled “20 minutes later”, you can see how much gas has been collected in each column. These columns were filled with solution at the beginning of the experiment, but now one column (the left column, negative electrode) has less solution than the other (and therefore it has more gas). The left column actually contains twice the amount of gas as the right column. This is because H2 is collected in the left column and O2 is collected in the right column. According to the stoichiometry of the reaction, for every one O2 that is produced, two H2 molecules are produced:

2 H2O(ℓ) + energy  ⟶  O2(g) + 2 H2(g)

This reaction would not have occurred if we did not turn on the energy source, though. This reaction required an input of energy, and is therefore an endothermic reaction.

Example 1

Combustion and Limiting Reagents
How much heat is released when 10.0 g hydrogen gas is burned in the presence of 10.0 g oxygen gas?

First, determine the amount of heat that can be released by burning the 10.0 g hydrogen in excess oxygen.  Note that the balanced chemical equation states that 483.6 kJ of energy is released per two mol hydrogen used up:

10.0 g H2 × \dfrac{1 \;\rule[0.5ex]{3em}{0.1ex}\hspace{-3em}\text{mol H}_2}{2.02 \;\rule[0.5ex]{2em}{0.1ex}\hspace{-2em}\text{g H}_2} \times \dfrac{483.6\;\text{kJ}}{2\;\rule[0.5ex]{3em}{0.1ex}\hspace{-3em}\text{mol H}_2} = 1200 kJ

Second, determine the amount of heat that can be released by burning the 10.0 g oxygen in excess hydrogen.  Note that the balanced chemical equation states that 483.6 kJ of energy is released per one mol oxygen used up:

10 g O2 × \dfrac{1 \;\rule[0.5ex]{3em}{0.1ex}\hspace{-3em}\text{mol O}_2}{32.00 \;\rule[0.5ex]{2em}{0.1ex}\hspace{-2em}\text{g O}_2} \times \dfrac{483.6\;\text{kJ}}{1\;\rule[0.5ex]{3em}{0.1ex}\hspace{-3em}\text{mol O}_2} = 151 kJ

Notice that less energy is produced when 10.0 g oxygen is used.  Thus, oxygen is the limiting reagent and 151 kJ energy is produced in this reaction.

Check Your Learning
How many grams of water can be generated if 242 kJ energy was released when hydrogen and oxygen were burned.


18.0 g H2O

Key Concepts and Summary

Energy can be viewed as either a reactant or a product in a chemical reaction, just like any other reactant or product. In an endothermic reaction, energy is viewed as the reactant because it is put into the reaction; an exothermic reaction contains energy as a product. The amount of energy scales with the amount of reactants used or products made.


a reaction in which energy is absorbed from the surroundings
a reaction in which energy is released to the surroundings

Chemistry End of Section Exercises

  1. Consider the following equation:
    2 H2(g) + O2(g)  ⟶  2 H2O(ℓ) + 483.6 kJ
    1. How many grams of O2 can be produced if 2901.6 kJ of energy is added to H2O(ℓ) to form H2(g) and O2(g)?
    2. How many grams of H2 can be produced if 2901.6 kJ of energy is added to H2O(ℓ) to form H2(g) and O2(g)?
  2. One can create an instant cold pack by reacting solid barium hydroxide with solid ammonium chloride to form water, ammonia gas, and barium chloride.
    1. Write a balanced chemical equation for this reaction.
    2. Is this process endothermic or exothermic (remember that it can be used in an instant cold pack)?
    3. Add the term “energy” to the proper side of your equation in part (a) to match your determination of endo- or exothermic in part (b).
  3. Sugar can be burned to form carbon dioxide and water, and release heat:
    C12H22O11(s) + 12 O2(g)  →  12 CO2(g) + 11 H2O(g)   [Releases 5.64 × 103 kJ of heat]
    1. What is the molar mass of the sugar?
    2. How much energy is released by burning 4.2 g of sugar (a teaspoon of sugar)?

Answer to Chemistry End of Section Exercises

  1. (a) 192 g; (b) 24 g
  2. (a) Ba(OH)2(s) + 2 NH4Cl(s)  →  2 H2O(ℓ) + 2 NH3(g) + BaCl2(aq)
    (b) Endothermic
    (c) Energy + Ba(OH)2(s) + 2 NH4Cl(s)  →  2 H2O(ℓ) + 2 NH3(g) + BaCl2(aq)
  3. (a) 342.34 g/mol
    (b) 69 kJ released
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