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57 Cards in this Set
- Front
- Back
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When a reaction is spontaneous at a high T only, ∆H is ___, ∆S is ______. |
When a reaction is spontaneous at high T only, ∆H is positive, and ∆S is positive as well. |
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When a reaction is never spontaneous, ∆H is _____, ∆S is _______ |
When a reaction is never spontaneous, ∆H is positive, while ∆S is negative. |
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When a reaction is spontaneous at all T, ∆H is _____, ∆S is ________. |
When a reaction is spontaneous at all T, ∆H is negative, while ∆S is positive. |
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When a reaction is spontaneous only at low T, ∆H is ______, ∆S is _______. |
When a reaction is spontaneous only at low T, ∆H is negative, and ∆S is negative as well. |
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At low temperatures, reactions are spontaneous (∆G < 0) only if they are (endothermic, exothermic) |
At low temperatures, reactions are spontaneous (∆G < 0) only if they are exothermic. |
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At high temperatures, reactions are spontaneous (∆G < 0) only if they (increase, decrease) entropy. |
At high temperatures, reactions are spontaneous (∆G < 0) only if they increase in entropy. |
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Elements in their standard state are defined to have a standard free energy of formation (∆G) of what? |
Elements in their standard state have ∆G = 0. |
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What is the formula for work? (Both regular and for gases? |
w = -P∆V or -∆nRT |
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Express change in energy formulas |
∆E = E[products] - E[reactants] |
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Relationship between gases and work |
We only see energy changes due to work when gases are involved. Reactions involving gases often result in an increase or decrease in volume. For a gas to expand, it has to push out. Force needs to be applied to expand volume. |
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Endothermic Reaction |
Heat transfer to the system from surroundings ∆EN > 0 Work being done on the system Bonds being made |
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Exothermic Reaction |
Heat transfer from the system to the surroundings ∆EN < 0 Energy lost by system Bonds being broken |
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Spontaneous only at high temperatures ∆H =? ∆S = ? |
For reactions spontaneous only at high temperatures, ∆H and ∆S are positive |
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Never spontaneous ∆H = ? ∆S = ? |
For reactions that are never spontaneous, ∆H is positive, and ∆S is negative |
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For reactions spontaneous at all temperatures, ∆H = ? ∆S = ? |
For reactions spontaneous at all temperatures, ∆H is negative, and ∆S is positive |
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For reactions spontaneous at low temperatures only, ∆H = ? ∆S = ? |
For reactions spontaneous at low temperatures ∆H is negative, and ∆S is negative. |
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When gases form from solids or liquids (all the reactants are solids, liquids, or solutions, and at least one product is a gas) change in entropy is (positive, negative) |
When gases form from solids or liquids, change in entropy is positive |
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Entropy (increases, decreases) when mixtures are formed from pure substances |
Entropy rises when mixtures are formed from pure substances |
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Entropy (increases, decreases) when the moles of gases increases |
Entropy increases when moles of gases increases |
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Weak IMF (Vapor Pressure, surface tension, viscosity, evaporation rate, phase change temperature) |
Weak Intermolecular Forces: Higher Vapor Pressure Lower Surface Tension Lower Viscosity Faster Evaporation Rate Lower Phase Change Temperature |
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Strong IMF (vapor pressure, surface tension, viscosity, evaporation rate, phase change temperature) |
Strong Intermolecular Forces: Lower Vapor Pressure Higher Surface Tension Higher Viscosity Slower Evaporation Rate Higher Phase Change Temperature |
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You are told that the enthalpy of the gas mixture goes up, which means that heat was (absorbed, released) during the reaction and the reaction is (endothermic, exothermic) |
When enthalpy of a gas mixture goes up, heat is absorbed during the reaction and the reaction is endothermic. |
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Entropy (increases, decreases) when pure substances are mixed, as long as temperature and volume stay constant. |
Entropy increases when pure substances are mixed, as long as temperature and volume stay constant. |
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Heat flow is considered (positive, negative) when heat flows into a system |
Positive |
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Heat flow is considered (+, -) when work is done on a system |
Heat flow is considered positive when work is done on a system |
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If a real gas has a volume that is larger thanyou would predict based on the ideal gas law,then the intermolecular forces for that gas aredominated by |
Repulsive Forces If the volume of the real gas is larger thanyou would predict based on the ideal gas law,then the compression factor Z > 1. Thismeans the intermolecular forces are dominatedby repulsions between the gas particles(atoms or molecules). |
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When gas pressure increases, ∆S (+, -) |
When gas pressure increases, ∆S < 0 |
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When you increase moles of gas, ∆S (+, -) |
When you increase moles of gas, ∆S > 0 |
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When you decrease moles of gas, ∆S (+, -) |
When you decrease moles of gas, ∆S < 0 |
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If you have an endothermic process in which the change in entropy is positive, you can make it spontaneous by increasing ______________ |
Temperature |
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∆H > 0 for (endothermic, exothermic) processes |
Endothermic |
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If ∆G is negative and T is very large, increasing the temperature makes the process (endothermic, exothermic) |
Endothermic |
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Nitrate |
NO3(-) |
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Nitrite |
NO2(-) |
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Chromate |
CrO4(2-) |
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Dichromate |
Cr2O7(2-) |
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Cyanide |
CN(-) |
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Hydroxide |
OH(-) |
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Carbonate |
CO3(2-) |
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Sulfate |
SO4(2-) |
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Sulfite |
SO3(2-) |
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Oxalate |
C2O4(2-) |
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Phosphate |
PO4(3-) |
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Phosphite |
PO3(3-) |
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Perchlorate |
ClO4(-) |
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Chlorate |
ClO3(-) |
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Chlorite |
ClO2(-) |
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Hypochlorite |
ClO(-) |
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Permanganate |
MnO4(-) |
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Peroxide |
O2(2-) |
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Hydrogen Carbonate |
HCO3(-) |
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Hydrogen Sulfate |
HSO4(-) |
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Hydrogen Sulfite |
HSO3(-) |
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Hydrogen Oxalate |
HC2O4(-) |
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Hydrogen Phosphate |
HPO4(2-) |
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Dihydrogen Phosphate
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H2PO4(-) |
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Hydrogen Sulfide |
HS(-) |
