Thermodynamics Thermochemistry Carol Brown Saint Mary’s Hall.
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Transcript of Thermodynamics Thermochemistry Carol Brown Saint Mary’s Hall.
The 1st Law
In all changes, energy is conserved
The energy of the universe is constant
∆E=q + w(both q and w are from the system’s
point of view)
Calorimetry-Basics
Heat: The total amount of thermal energy contained in a sample of matter– Measured in calories or joules
Temperature: The average kinetic energy of the molecules in a sample of mater.– Measured in Kelvins or degrees Celsius
More basics
Specific heat capacity: The amount of heat it takes to raise one gram of a substance one degree Celsius. – Units: J/g oC
Heat capacity: The amount of heat it takes to raise a system one degree Celsius.– Units--J/oC
q = mc∆T
How much heat, in kJ, is necessary to take 20 g of ice at -5o C to steam at 100o C? The specific heat of ice is 2.1 J/g oC; of liquid water is 4.2 J/g oC. The latent heat of fusion is 334 J/g. The latent heat of vaporization is 2268 J/g.
60.7 kJ
Important Terms
Enthalpy (heat of reaction)--The amount of heat lost or absorbed during the course of a reaction when the only work done is expansion or contraction at a constant pressure (P∆V). Change in enthalpy is a state function and is symbolized by ∆H.
Stoichiometric Thermochemistry
When 2.50 g of methane burns in oxygen, 125 kJ of heat is produced. What is the molar heat of combustion of methane under these conditions?
Stoichiometric Thermochemistry: Answer
When 2.50 g of methane burns in oxygen, 125 kJ of heat is produced. What is the molar heat of combustion of methane under these conditions?
-802 kJ/mol
Stoichiometric Thermochemistry: Your Turn
The oxidation of glucose is described by the following equation:
C6H12O6 + 6O2 --> 6CO2 + 6H2O ∆Ho = -2816 kJ
How much heat in kJ is produced by the oxidation of 1.0 g of glucose?
Stoichiometric Thermochemistry:Your Turn Answer
The oxidation of glucose is described by the following equation:
C6H12O6 + 6O2 --> 6CO2 + 6H2O ∆Ho = -2816 kJ
How much heat in kJ is produced by the oxidation of 1.0 g of glucose?
16 kJ
Another term
Standard molar heat of combustion: The amount of heat released when one mole of a substance is burned in oxygen. The measurements must be taken at standard thermodynamic conditions. i.e. 298 K and 1.00 atm pressure. Symbolized by ∆Ho
comb.
Still another important term
Standard molar heat of formation: The amount of heat lost or absorbed when one mole of product is formed from its elements in their most stable state. Again, the measurements must be taken at thermodynamic standard conditions. Symbolized by ∆Ho
f.
Is this an example of ∆Hocomb,
∆Hof, neither, or both?
C + 1/2 O2 --> CO
CO + 1/2 O2 --> CO2
CH3OH + 3/2 O2 --> CO2 + 2H2O
8 C + 9H2 --> C8H18
CH4 + 2O2 --> CO2 + 2H2O
FeCl2 + 1/2Cl2--> FeCl3
S + O2 --> SO2
Hess’s Law
Since enthalpy is a state function, the change in enthalpy in going from some initial state to some final state is independent of the pathway. This means that in going from a particular set of reactants to a particular set of products, the change in enthalpy is the same whether the reaction takes place in a single step or in a series of steps. This principle is known as Hess’s Law.
Hess’s Law Problem #1
Given the following data:H2 + 1/2O2 --> H2O(l) ∆Ho=-285.8 kJ
N2O5 + H2O --> 2HNO3 ∆Ho= -76.6 kJ
1/2N2 + 3/2O2 + 1/2H2_--> HNO3 ∆Ho=-174.1 kJ
Calculate ∆Ho for the reaction
2N2 + 5O2 --> 2N2O5
Answer
Given the following data:H2 + 1/2O2 --> H2O(l) ∆Ho=-285.8 kJ
N2O5 + H2O --> 2HNO3 ∆Ho= -76.6 kJ
1/2N2 + 3/2O2 + 1/2H2 -->HNO3 ∆Ho=-174.1 kJ
Calculate ∆Ho for the reaction
2N2 + 5O2 --> 2N2O5
28.4 kJ
Another Hess’s Law Problem
Calculate ∆Ho for the processSb(s) + 5/2 Cl2(g) --> SbCl5(g)
from the following information.
Sb(s) + 3/2 Cl2(g) --> SbCl3(g) ∆Ho -314 kJ
SbCl3(g) + Cl2(g) --> SbCl5(g) ∆Ho -80 kJ
Another Hess’s Law Problem:Answer
Calculate ∆Ho for the processSb(s) + 5/2 Cl2(g) --> SbCl5(g)
from the following information.
Sb(s) + 3/2 Cl2(g) --> SbCl3(g) ∆Ho -314 kJ
SbCl3(g) + Cl2(g) --> SbCl5(g) ∆Ho -80 kJ
Answer: -394 kJ