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| the study of the relationships between chemical reactions and energy changes. |
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| Energy used to cause an object that has mass to move against a force. |
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| Formula of the relationship of work and force and distance |
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w = F d
w-work
f-force
d-distance |
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| Energy transferred from a hotter object to a colder one. |
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| energy associated the motion of an object. |
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| energy associated with the position or composition of an object |
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| The SI unit of energy is the? |
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| (cal) the amount of energy required to raise the temperature of one gram of water 1oC |
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| Relationship of cal and J |
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| First Law of Thermodynamics Law of Conservation of Energy? |
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| Energy is neither created nor destroyed |
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| Energy can be transferred between ? |
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| a system and the surroundings. |
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| In a Chemical reaction the system and surroundings are? |
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system-reactants and products, can beOpen, closed, or isolated
Surroundings-container and everything else |
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| the sum of all kinetic and potential energies of all its components. |
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| The change in internal energy is? |
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&E = Efinal − Einitial
&= triangle that means change |
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| The change in internal energy in a chemical reaction formula? |
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| &E = E products − E reactants |
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| Energy can be exchanged through ? |
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| Relationship of energy to heat and work? |
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WORK
A system absorbs 125 J of heat from the surroundings and does 62 J of work on the surroundings.
Calculate the change in internal energy (E) in J. |
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| depends only on the present state of the system, not on the path by which the system arrived at that state. |
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| Internal energy is/ is not a state function? |
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| q and q are/ are not state functions? |
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| w= is neg and work is done By the system ONTO the surroundings |
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| H- the heat transferred between the system and surroundings during a chemical reaction carried out under constant pressure. |
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| heat is absorbed from the surroundings by the system |
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| heat is released by the system to the surroundings |
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| = &H,rxn= H products- H reactants |
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| Enthalpy is an _____ property |
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| Extensive meaning it differs with the states of the substances |
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| H for any reaction written in reverse will have the same magnitude of heat associated with it, but ? |
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WORK
2 H2(g) + O2(g) → 2 H2O(g) ∆H = - 483.6 kJ
What is ∆H for
2 H2O(g) → 2 H2(g) + O2(g) |
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WORK
2 H2(g) + O2(g) → 2 H2O(g) ∆H = - 483.6 kJ
What is ∆H for
4 H2O(g) → 4 H2(g) + 2 O2(g) |
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WORK
2 H2(g) + O2(g) → 2 H2O(g) ∆H = - 483.6 kJ
What is ∆H for
3 H2(g) + 3/2 O2(g) → 3 H2O(g) |
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Definition
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| C,s- the amount of energy required to raise the temperature of 1 g of a substance by 1 K (1C). |
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| C,m- is the heat capacity of 1 mole of a substance. |
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| = heat transfer/ (mass)(change in temp) |
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WORK
How much heat (kJ) is needed to warm 325 g of water from
24 oC to 75 oC. The specific heat (Cs) of water is 4.18 J/g-K? |
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WORK
How much heat (kJ) is needed to warm 325 g of water from
24 oC to 75 oC. The specific heat (Cs) of water is 4.18 J/g-K?
Answer: 69 kJ
b. What is the molar heat capacity of water (Cm)? |
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| (specific heat of solution) x (grams of solution) x ∆T |
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WORK
When 25.0 ml of 0.450 M AgNO3 and 33.0 ml of
0.341 M HCl are mixed in a constant-pressure
calorimeter, the temperature of the mixture increases
from 21.42 oC to 22.31 oC.
Calculate H of the reaction in kJ/mol AgNO3,
assuming the mixture has a density of
1.00 g/ml and that its specific heat is 4.18 J/g oC. |
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| Constant-Volume Calorimetry aka? |
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| Formula of Bomb Calorimety? |
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| q reaction = - C,cal x ∆T |
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WORK
A 1.146 g sample of lactic acid (HC3H5O3)
is burned in a calorimeter whose heat capacity
is 4.812 kJ/°C. The temperature increases
from 23.07°C to 26.12°C.
Calculate the heat of combustion of lactic acid per gram. |
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Definition
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| If a reaction is carried out in a series of steps, H for the overall reaction is the sum of the enthalpy changes for the individual steps. |
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WORK
Calculate H for the overall reaction
2 C(s) + H2(g) C2H2(g)
given the following chemical equations and their respective enthalpy changes:
See page 182 for reactions |
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Definition
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| Standard Enthalpy of formation |
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| &Hof), is the enthalpy change for the formation of 1 mol of compound from its elements, with all substances in their standard states (appendix C). |
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| at 1 atm and 25 oC (298K). |
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| &Hof of any element in its most stable form is |
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WORK
For which of the following reactions at 25°C would the enthalpy change represent a standard enthalpy of formation? For each that does not, what changes would need to be made to make it an equation whose H is an enthalpy of formation?
See page 184 |
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| = n&Hf (products) - m&Hf reactants |
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WORK
Calculate &Horxn for
C3H8(g) + O2(g) → CO2(g) + H2O(l)
Given Hof C3H8(g) = -103.85 kJ/mol
Hof CO2(g) = -393.5 kJ/mol
Hof H2O(l) = -285.8 kJ/mol |
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