Chemical stoichiometry describes the quantitative relationships between reactants and products in chemical reactions.
We have previously measured quantities of reactants and products using masses for solids, and volumes in conjunction with the molarity for solutions; now we can also use gas volumes to indicate quantities. If we know the volume, pressure, and temperature of a gas, we can use the ideal gas equation to calculate how many moles of the gas are present. If we know how many moles of a gas are involved, we can calculate the volume of a gas at any temperature and pressure.
Sometimes we can take advantage of a simplifying feature of the stoichiometry of gases that solids and solutions do not exhibit: all gases that show ideal behavior contain the same number of molecules in the same volume (at the same temperature and pressure). Thus, the ratios of volumes of gases involved in a chemical reaction are given by the coefficients in the equation for the reaction, provided that the gas volumes are measured at the same temperature and pressure.
We can extend Avogadro’s law (that the volume of a gas is directly proportional to the number of moles of the gas) to chemical reactions with gases: gases combine, or react, in definite and simple proportions by volume, provided that all gas volumes are measured at the same temperature and pressure. For example, since nitrogen and hydrogen gases react to produce ammonia gas according to N2(g) + 3 H2(g) → 2 NH3(g), a given volume of nitrogen gas reacts with three times that volume of hydrogen gas to produce two times that volume of ammonia gas, if pressure and temperature remain constant.
The explanation for this is illustrated in Figure 1. According to Avogadro’s law, equal volumes of gaseous N2, H2, and NH3, at the same temperature and pressure, contain the same number of molecules. Because one molecule of N2 reacts with three molecules of H2 to produce two molecules of NH3, the volume of H2 required is three times the volume of N2, and the volume of NH3 produced is two times the volume of N2.
Reaction of Gases
Propane, C3H8(g), is used in gas grills to provide the heat for cooking. What volume of O2(g) measured at 25 °C and 760 torr is required to react with 2.7 L of propane measured under the same conditions of temperature and pressure? Assume that the propane undergoes complete combustion.
The ratio of the volumes of C3H8 and O2 will be equal to the ratio of their coefficients in the balanced equation for the reaction:
1 mole + 5 moles → 3 moles + 4 moles
From the equation, we see that one volume of C3H8 will react with five volumes of O2:
A volume of 13.5 L of O2 will be required to react with 2.7 L of C3H8.
Check Your Learning
An acetylene tank for an oxyacetylene welding torch provides 9340 L of acetylene gas, C2H2, at 0 °C and 1 atm. How many tanks of oxygen, each providing 7.00 × 103 L of O2 at 0 °C and 1 atm, will be required to burn the acetylene?
3.34 tanks (2.34 × 104 L)
Volumes of Reacting Gases
Ammonia is an important fertilizer and industrial chemical. Suppose that a volume of 683 billion cubic feet of gaseous ammonia, measured at 25 °C and 1 atm, was manufactured. What volume of H2(g), measured under the same conditions, was required to prepare this amount of ammonia by reaction with N2?
Because equal volumes of H2 and NH3 contain equal numbers of molecules and each three molecules of H2 that react produce two molecules of NH3, the ratio of the volumes of H2 and NH3 will be equal to 3:2. Two volumes of NH3, in this case in units of billion ft3, will be formed from three volumes of H2:
The manufacture of 683 billion ft3 of NH3 required 1020 billion ft3 of H2. (At 25 °C and 1 atm, this is the volume of a cube with an edge length of approximately 1.9 miles.)
Check Your Learning
What volume of O2(g) measured at 25 °C and 760 torr is required to react with 17.0 L of ethylene, C2H4(g), measured under the same conditions of temperature and pressure? The products are CO2 and water vapor.
Volume of Gaseous Product
What volume of hydrogen at 27 °C and 723 torr may be prepared by the reaction of 8.88 g of gallium with an excess of hydrochloric acid?
To convert from the mass of gallium to the volume of H2(g), we need to do something like this:
The first two conversions are:
Finally, we can use the ideal gas law:
Check Your Learning
Sulfur dioxide is an intermediate in the preparation of sulfuric acid. What volume of SO2 at 343 °C and 1.21 atm is produced by burning l.00 kg of sulfur in oxygen?
1.30 × 103 L
The ideal gas law can be used to derive a number of convenient equations relating directly measured quantities to properties of interest for gaseous substances and mixtures. Avogadro’s law may be used in stoichiometric computations for chemical reactions involving gaseous reactants or products.
- Avogadro’s law
- The volume of any ideal gas is directly proportional to the number of moles of the gas.
- Cavendish prepared hydrogen in 1766 by the novel method of passing steam through a red-hot gun barrel:
4 H2O(g) + 3 Fe(s) → Fe3O4(s) + 4 H2(g)
- Outline the steps necessary to answer the following question: What volume of H2 at a pressure of 745 torr and a temperature of 20 °C can be prepared from the reaction of 15.0 g of H2O?
- Answer the question.
- Automobile air bags are inflated with nitrogen gas, which is formed by the decomposition of solid sodium azide (NaN3). The other product is sodium metal. Calculate the volume of nitrogen gas at 27 °C and 756 torr formed by the decomposition of 125 g of sodium azide.
- What volume of oxygen at 423.0 K and a pressure of 127.4 kPa is produced by the decomposition of 129.7 g of BaO2 to BaO and O2?
- What volume of O2 at STP is required to oxidize 8.0 L of NO at STP to NO2? What volume of NO2 is produced at STP?
- Ethanol, C2H5OH, is produced industrially from ethylene, C2H4, by the following sequence of reactions:
3 C2H4 + 2 H2SO4 → C2H5HSO4 + (C2H5)2SO4C2H5HSO4 + (C2H5)2SO4 + 3 H2O → 3 C2H5OH + 2 H2SO4
What volume of ethylene at STP is required to produce 1.000 metric ton (1000 kg) of ethanol if the overall yield of ethanol is 90.1%?
- Under what conditions are the ratio of stoichiometric coefficients used to balance a chemical equation the same as the volume ratio of the gaseous reactants or products? Are these conditions met when the chemical reaction takes place in a glass flask or a syringe with a moveable piston?
- If a syringe contains 30.0 mL of NO(g), what stoichiometric volume of O2(g) must be added to the syringe for the NO(g) and O2(g) to react and form NO2(g)?
- Under what conditions are the ratio of stoichiometric coefficients used to balance a chemical equation the same as the pressure ratio of the gaseous reactants or products? Are these conditions met when the chemical reaction takes place in a glass flask or a syringe with a moveable piston?
- If a glass flask contains 75 mmHg of O2(g), what stoichiometric pressure of NO(g) must be added to the flask for the NO(g) and O2(g) to react and form NO2(g)?
- (a) First, convert grams H2O to moles of H2. Then, solve for pressure using the ideal gas law; (b) 20.4 L H2
- 71.4 L
- 10.57 L O2
- 4.0 L O2; 8.0 L NO2
- 5.40 × 105 L
- When the reaction is carried out at constant pressure and temperature; a syringe with a moveable piston.
- 15.0 mL
- When the reaction is carried out at constant volume and temperature; a glass flask.
- 150 mmHg
- “Quotations by Joseph-Louis Lagrange,” last modified February 2006, accessed February 10, 2015, http://www-history.mcs.st-andrews.ac.uk/Quotations/Lagrange.html ↵