# Gas Stoichiometry Ideal Gas Law - PowerPoint PPT Presentation

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Gas Stoichiometry Ideal Gas Law. Putting it all together…. Balance the following equation…. C 8 H 18 (l) + O 2 (g) → CO 2 (g) + H 2 0(g) 2 C 8 H 18 (l) + 25 O 2 (g) → 16 CO 2 (g) + 18 H 2 0(g) Coefficients of balanced equations can be used as mole ratios in stoichiometry problems.

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Gas Stoichiometry Ideal Gas Law

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## Gas Stoichiometry Ideal Gas Law

Putting it all together…

### Balance the following equation…

• C8H18(l) + O2(g) → CO2(g) + H20(g)

• 2 C8H18(l) + 25 O2(g) → 16 CO2(g) + 18 H20(g)

• Coefficients of balanced equations can be used as mole ratios in stoichiometry problems

• ### Mass-Mass Stoichiometry

• Problem 11.13 c (p.332)

• Mg + HCl → H2 + MgCl2

• 60.1 g HCl

### Volume Ratio = Mole Ratio

• Problem 12.85 (p.373)

• 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g)

### Avogadro’s LawOne mole of a gas will occupy 22.4 L

• This means that the mole ratio is the same as the volume ratio

### Volume Ratio = Mole Ratio

• Problem 12.85 (p.373)

• 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g)

• 200. L O2

### Volume Ratio = Mole Ratio

• Problem 12.85 (p.373)

• 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g)

• Problem 12.81 (p.373)

• 2 C2H2(g) + 5 O2(g) → 4 CO2(g) + 2H2O(g)

• 2.5 tanks O2

### Gas @ STP

• Problem 12.92 (p374)

• NaN3(s) + Fe2O3(s) → Na2O(s) + Fe(s) + N2(g)

• 6 NaN3(s) + Fe2O3(s) → 3 Na2O(s) + 2 Fe(s) + 9 N2(g)

• 10.6 g NaN3

### Standard Molar Volume

• The volume of 1.0 mole of any gas at STP is 22.4 L.

• This is called the standard molar volume.

• The volume of any gas at STP can be calculated if the number of moles is known:

• V = (moles)(22.4 L)

### Gas Not at STP

• Problem 12.88 (p.373)

• CaC2(s) + 2 H2O(l) → Ca(OH)2(s) + C2H2(g)

### Ideal Gas Law

• All of the variables used to describe gases can be compared using the Ideal Gas Law

• The IGL is often called an equation of state, as it is very useful when finding some property of a gas at a certain condition

• Not so great when conditions are changing

• Entropy is another condition of state

### Ideal Gas Law

• PV = nRT

• P = pressure

• V = volume

• T = temperature

• n = number of moles of gas

• R = Gas Constant

• value depends on the desired unit

### Gas Constant (“R”)

• R is a constant that is used in the IGL so that it may be used for all gases

• It has a different value, depending on the pressure unit being used in the problem

### Gas Not at STP

• Problem 12.88 (p.373)

• CaC2(s) + 2 H2O(l) → Ca(OH)2(s) + C2H2(g)

• 960 ml C2H2

• Problem 12.90 (p.373)

• 2 C8H18(l) + 25 O2(g) → 16 CO2(g) + 18 H20(g)

### Gas Not at STP

• Problem 12.88 (p.373)

• CaC2(s) + 2 H2O(l) → Ca(OH)2(s) + C2H2(g)

• 960 ml C2H2

• Problem 12.90 (p.373)

• 2 C8H18(l) + 25 O2(g) → 16 CO2(g) + 18 H20(g)

• 837 L CO2