Endo vs Exothermic
∆H, ∆S, ∆G
Calorimetry
Spontinaity
Thermodynamics
100
A reaction has a ∆H of -483.k kJ/mole
What is Exothermic
100
Entropy is increasing or decreasing in the following reaction?
NaCl(s) --> Na1++Cl1-
What is increasing
100
2 moles of water are formed in a reaction because the energy of formation is 18.0kJ/mole.
How many moles of water are reacted if a reaction releases 36kJ of energy?
100
These are the two driving forces for all reactions.
What are enthalpy and entropy?
100
The entropy of a perfect crystal at absolute zero is exactly equal to zero.
What is the third law of thermodynamics
200
A system takes in 500J of energy and does 600J of work to the surroundings.
What is exothermic
200
Does this reaction happen spontaneously?
NaCl(s) --> Na1++Cl1-
What is yes
200
The following reaction has a enthalpy change of +26.5kJ/mole. The reaction creates 12.0g of HI creating this much energy total.
.5H2+.5I2--> 2HI
What is 2.48kJ of energy?
200
A reaction is said to be this if it occurs without being driven by some outside force
What is spontaneous?
200
Calculate the enthalpy of the following chemical reaction:
CS2(ℓ) + 3O2(g) ---> CO2(g) + 2SO2(g)
Given:
C(s) + O2(g) ---> CO2(g) ΔH = -393.5 kJ/mol
S(s) + O2(g) ---> SO2(g) ΔH = -296.8 kJ/mol
C(s) + 2S(s) ---> CS2(ℓ) ΔH = +87.9 kJ/mol
What is -1,075 kJ/mole?
300
The ∆H for the below reaction is -66.36kJ. Calculate the heat released when 12.0g of Nitrogen reacts completely with oxygen.
N2 + 2O2 --> 2NO2
What is -56.88kJ of energy
300
In thermodynamics this is a process that can be "reversed" by means of infinitesimal changes in some property of the system.
What is a reversible process.
300
The following picture shows this type (endo vs exothermic) reaction.
What is exothermic reaction?
300
This is a measure of the disorder of a system, and systems tend to favor a more disordered system: nature tends toward chaos
What is Entropy?
300
Given the following ΔHf
NO2(g) 33.2 kJ/mol
N2O4 (g) 9.2 kJ/mol
Fe2O3(s) -822.16 kJ/mol
What is the Energy of the following reaction:
2NO2(g)--> N2O4 (g)
What is 57.2 kJ/mole?
400
How much heat is released when 2.80g of methane is burned in a constant-pressure system?
CH4+2O2-->CO2+H2
What is -155kJ
400
The law of conservation of energy states that the total energy of an isolated system is constant; energy can be transformed from one form to another, but cannot be created or destroyed.
What is the First Law of Thermodynamics.
400
A chemistry student dissolves 4.51 grams of sodium hydroxide in 100.0 mL of water at 19.5°C (in a calorimeter cup). As the sodium hydroxide dissolves, the temperature of the surrounding water increases to 31.7°C. Determine the heat of solution of the sodium hydroxide in J/g.
What is -1130.7 J/g?
400
When a reaction has a +∆S, -∆H, and -∆G then the reaction would be this.
What is a spontaneous reaction?
400
Given the following ΔHf:
Fe3O4 (s) -118 kJ/mol
FeO(s) -271.9 kJ/mol
Fe2O3(s)(s) -822.16 kJ/mol
What is the enthalpy of the following reaction?
4FeO(s) + O2 (g) --> 2Fe2O3(s)
What is -1100 kJ?
500
The specific heat of nickel is 0.440 J/goC. How much energy would it take to warm a 20.0g sample of nickel from 0.00oC to 30.0oC?
What is 264J
500
This law states that in every real process the sum of the entropies of all participating bodies is increased.
What is the second law of thermodynamics.
500
Calculate the enthalpy for this reaction:
2C(s) + H2(g) ---> C2H2(g) ΔH° = ??? kJ
Given the following thermochemical equations:
C2H2(g) + (5/2)O2(g) ---> 2CO2(g) + H2O(ℓ)ΔH° = -1299.5
C(s) + O2(g) ---> CO2(g) ΔH° = -393.5 kJ
H2(g) + (1/2)O2(g) ---> H2O(ℓ) ΔH° = -285.8 kJ
What is +1299.5 kJ + (-787 kJ) + (-285.8 kJ) = +226.7 kJ
500
The following reaction is an example of this type of reaction?
What is spontaneous?
500
This is an example of this kind of reaction.
http://www.mikeblaber.org/oldwine/chm1046/notes/SolnProp/SolnProc/Hsolv2gif.gif
What is an endothermic reaction (spontaneous).