1st law of thermodynamics |
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the total energy of the universe is constant |
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2nd law of thermodynamics |
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the total entropy of the universe is always
incresing |
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3rd law of thermodynamics |
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the entropy of every pure perfectly formed crystalline substance at absolute zero is zero |
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a negative delta H is what kind of reaction? |
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exothermic |
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a positive delta H is what kind of reaction? |
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endothermic |
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definition of entropy |
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measure of disorder |
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4 rules of entropy |
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1. gases have greater entropy than liquids 2. liquids have greater entropy than solids 3. entropy of a system increases as temp increases 4. in a chemical reaction the side with more mols has greater entropy |
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thermochemistry |
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the heat changes that occur during chemical reactions |
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energy |
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the capacity for doing work or supplying heat |
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what is the energy stored in chemical bonds called? |
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chemical potential energy |
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heat |
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energy that transfers from one object to another becuase of a temperature difference between them. |
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calorie |
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the quantity of heat needed to raise the temp of 1g of pure water 1 degree C |
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kilocalorie |
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equal to 1000 calories |
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joule |
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the SI unit of heat and energy named after the English physicist James Prescott Joule |
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how many joules in 1 calorie? |
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4.184 Joules |
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Heat capacity |
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the amount of heat needed to increase the temp of an object exactly 1 degree C |
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Specific heat capacity |
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the amount of heat it takes to raise the temp of 1g of the substance 1 degree C |
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calorimeter |
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a device for measuring heat changes |
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enthalpy |
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the heat content of a system at constant pressure |
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what does delta H stand for? |
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heat of reaction or enthaply of reaction |
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Hess's law |
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if you add two or more thermochemical equations to get the final equation, then you can also add the heat of reaction to five the final heat reaction. |
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standard heat of formation |
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the change in enthaply that accompanies the formation of one mol of a compound from its elements with all substances in their standard states at 25 degrees C |
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free energy |
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energy that is available to do work |
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spontaneous reactions |
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reactions that occur naturally and that facor the formation of products at the specified conditions |
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nonspontaneous reactions |
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reactions that do not facor the formation of products at the specified conditions |
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standard entropy |
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the entropy of a substance in its stable state at 25 degrees C |
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Gibb's free energy |
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the maximum amount of energy that can be coupled to another provess to do useful work |
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CaCO3(s) + 176kJ ----> CaO(s) + CO2(g) a. caculate the energy required to decompose 5.20 mol of CaCO3
b. how many kcal are required? |
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a. 915 kJ
b. 219 kcal |
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SO3 + H2O -----> H2SO4 + 129.6 kJ
how much heat in kJ and kcal is released when 583 grams of SO3 reacts with water? |
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a. |
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2CO2 + 43.9 kJ ----> 2CO + O2
how many molecules of CO2 can be decomposed by the addition of 22.2 kJ of heat? |
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6.09x10^23 molecules |
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2C2H6(g) + 7O2(g) ---> 4CO2(g) + 6H2O(l)
calculate delta H, delta S, and delta G |
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a. H= -3119.6 kJ/mol
b. S= -620.7 J/kmol
c. G= -2934.57 kJ/mol |
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2NO2(g) ---> N2O4(g)
calculate delta H,S and G |
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|
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2Fe + 3CO2 + 26.3kJ ---> Fe2O3 + 3CO
a. calculate kJ for 7.3 mols of Fe
b. is this a positive or negative enthalpy change? |
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a. 96 kJ
b. positive |
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2Mg + O2 ----> 2MgO + 288kcal
a. calculate kcal for 0.12 mols of Mg
b. calculate kJ |
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a. -17kcal
b. -71kJ |
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C2H4 + 3O2 ----> 2CO2 + 2H2O + 1.39x10^3
calculate the heat for 1.87g of C2H4 |
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-92.7kJ |
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I2(s) ----> I2(g)
calculate delta H,S and G |
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H=62.438 kJ/mol
S=144.56 J/kmol
G=19.327 kJ/mol |
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3CO(g) + Fe2O3(s) ----> 2Fe(s) + 3CO2(g)
calculate delta H,S and G |
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H= -24.7 kJ/mol
S= 16.36 J/kmol
G= -29.4 kJ/mol |
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2NO2(g) ---> 2NO(g) + 2H2O(g)
calculate delta H,S and G |
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H= -369.5 kJ/mol
S= 319.05 J/kmol |
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2NO(g) + O2(g) ----> 2NO2(g)
calculate delta H,S and G |
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H= -144.1 kJ/mol
S= -146.54 J/kmol |
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2HF(g) ---> H2(g) + F2(g) at 1030. C
calculate delta H,S and G |
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H= 542.2 kJ/mol
S= -14.10 J/kmol
G= 560.6 kJ/mol |
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NaOH(s) + HCl(aq) ---> NaCl(aq) + H2O(l)
at 85.0 C
calculate delta H,S and G |
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H= 100.33 kJ/mol
S= 64.4 J/kmol
G= -123.4 kJ/mol |
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