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NitroglycerineNitroglycerine4C3H5N3O9(l) 12CO2(g) + 10H2O(g) + 6N2(g) + O2(g)
100 g Nitro1mol Nitro227 g Nitro
29 mol gas4mol Nitro
= 3.193 mol gas
Or = .110 mol O2
= .661 mol N2
= 1.10 mol H2O= 1.32 mole CO2
NitroglycerineNitroglycerine4C3H5N3O9(l) 12CO2(g) + 10H2O(g) + 6N2(g) + O2(g)
V =
PV = nRT V = nRT/P
3.193 mol(0.082057 L atm/mol K)425 C
1atm
698 K
V = 183 L
HH22 + Cl + Cl22 2HCl(g) 2HCl(g)
g of Cl2
Limiting Reactant Problem – the hard way
Moles HCl
Moles HClg of H2
Moles Cl2
Moles H2
FW
FW
Balanced Eq
Balanced Eq Select limiting
reagent
Moles Cl2 Moles H2 used
Final pressure = pressure of HCl + pressure of excess reagent
Starting moles H2
- Moles H2 used
Excess moles H2
Moles HCl Moles H2 xs Total moles of gas+PV = nRT
P = 193 torr
HH22 + Cl + Cl22 2HCl(g) 2HCl(g)
g of Cl2
Understanding Gases – the easy way
Pressure Cl2
Pressure H2g of H2
Moles Cl2
Moles H2
FW
FW
PV = nRT
PV = nRTAdd to get
Initial pressure
Final pressure = Initial P = P Cl2 + P H2
Remember that the composition of a gas does NOT effect the pressure it exerts. So, since there is no change in the number of MOLES of gas during the reaction, there will be no change in the pressure. Thus the initial pressure equals the final pressure.
StoichiometryStoichiometryA B C D+ +
Moles A Moles C
g of C
FW
Volume of C
Molarity
Molarity of CVolume
Molecular weight
# grams
g of AFW
Volume of A
Molarity
Molarity of AVolume
Molecular weightOf A
# grams
Balanced Eq
Gases only!!!!
GasGas Stoichiometry StoichiometryA B C D+ +
Moles A Moles C
g of A FW g of CFW
Volume of A
Molarity
Volume of C
Molarity
Molarity of CVolume
Molarity of AVolume
Molecular weight
# grams
Molecular weightOf A
# grams
Balanced Eq
Balanced Eq
(T and P/V same)
Volume of A
Pressure of A
PV = nRT
Pressure of C
Volume of C
PV = nRT
What is RMS for HWhat is RMS for H22 at room at room temp?temp?
Μ
RTu
32 )298)(/3145.8(3 KKmolJ
=
What is RMS for HWhat is RMS for H22 at room at room temp?temp?
Μ
RTu
32 )298)(/3145.8(3 KKmolJ
=
What is RMS for HWhat is RMS for H22 at room at room temp?temp?
Μ
RTu
32 )298)(/3145.8(3 KKmolJ
=2.0g/mol
1kg _1000g
= 1.92 x 103 m/s≈ 2000 m/s≈ 4300 mi/hr
Why does it take so long Why does it take so long to smell gas that is to smell gas that is
released in the same released in the same room?room?
Problems involving GasesProblems involving Gases
PV=nRT can be used to get moles of PV=nRT can be used to get moles of gas from P, V and T. Once you have gas from P, V and T. Once you have mole then it is just a normal limiting mole then it is just a normal limiting reagent or stoichiometry or titration reagent or stoichiometry or titration or ….or ….
Gas Law ShortcutsGas Law Shortcuts All revolve around the fact that in gases, V All revolve around the fact that in gases, V
and P does NOT depend on nature of gas.and P does NOT depend on nature of gas. ImplicationsImplications
Can sum moles of all products and then find P Can sum moles of all products and then find P or V. (Dalton’s Law of Partial Pressures.)or V. (Dalton’s Law of Partial Pressures.)
Ratio of n:V or n:P is constant (at a given temp Ratio of n:V or n:P is constant (at a given temp and P or V) So 2 moles of gas C takes up twice and P or V) So 2 moles of gas C takes up twice the volume of 1 mole of gas A at the same the volume of 1 mole of gas A at the same conditions.conditions.
Caution: Shortcuts are NOT always Caution: Shortcuts are NOT always present.present.
Polarity and IMFPolarity and IMF
Polarity is the key to IMFs.Polarity is the key to IMFs. Select 2 molecules involved, find Select 2 molecules involved, find
polarity of each.polarity of each. Polar/polar = dipole/dipole -strongestPolar/polar = dipole/dipole -strongest Nonpolar/nonpolar = induced/induced - Nonpolar/nonpolar = induced/induced -
strongeststrongest Polar / Nonpolar = dipole induced-dipole -Polar / Nonpolar = dipole induced-dipole -
strongeststrongest If dipole/dipole look for H-BondingIf dipole/dipole look for H-Bonding
Requires:Requires:
O H
(F,N)
+-
N
(F,O)
-
Why don’t oil and Why don’t oil and water mix?water mix?