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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

Gas Stoichiometry Ideal Gas Law

Putting it all together…

balance the following equation
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
Mass-Mass Stoichiometry
  • Problem 11.13 c (p.332)
    • Mg + HCl → H2 + MgCl2
    • 60.1 g HCl
volume ratio mole ratio
Volume Ratio = Mole Ratio
  • Problem 12.85 (p.373)
    • 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g)
avogadro s law one mole of a gas will occupy 22 4 l
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 ratio1
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 ratio2
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
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
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
Gas Not at STP
  • Problem 12.88 (p.373)
    • CaC2(s) + 2 H2O(l) → Ca(OH)2(s) + C2H2(g)
ideal gas law
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 law1
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
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 stp1
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 stp2
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
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