Gas Stoichiometry Ideal Gas Law

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# Gas Stoichiometry Ideal Gas Law - PowerPoint PPT Presentation

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

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