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18 Cards in this Set
- Front
- Back
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Synthesis/composition
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Zn+S=ZnS
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Decomposition
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H2O= H2+ O2
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Single replacement
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Fe + CuSO4= Cu + FeSO4
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Double replacement
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AgNO3 + NaCl= NaNO3 + AgCl
AgCl= precipitate |
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Salt + water
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---> Acid + Base
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NaCl+H2O--> NaOH + HCl
PH? |
the PH is neutral because a strong acid is paired with a strong base
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Na2CO3 + H2O --> NaOH + H2CO3
PH? |
the PH is basic because a strong base is paired with a weak acid
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(NH4)2CO3 + 2H2O--> 2NH4OH + H2CO3
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the PH is neutral because a weak acid is paired with a weak base
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Entropy
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the bigger the entropy the more disordered it is
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Enthalpy
and Enthalpy equation |
change in H= Hproducts- Hreactants
H=mcT <-- use when there's no phase change happening H=mc <-- use when there's a phase change happening m=mass C= specific heat T= temperature |
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Molar heat of formation
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change in enthalpy that accompanies the formation of 1 mole of a compound at 25 C
written deltaHf describes the PRODUCT |
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Heat of combustion
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heat released by the complete combustion of 1 mole of substance
written deltaHc describes the REACTANT |
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Hess's law
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change the equations so they cancel out- remember to also change the enthalpies if needed
add up all the enthalpies |
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Enthalpy big equation
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H of reaction= sum of Hf products - sum of Hf reactants
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all elements including diatomics have an enthalpy of...
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zero
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for a double displacement reaction to go to completion a product or products must deposit as a...
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precipitate
or leave the reaction as a gas so there's either a gas or a precipitate in the products |
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first law of thermodynamics
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total energy of the universe is constant and can't be destroyed
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spontaneous
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a reaction that will occur without any energy imput from its surroundings
usually exothermic reactions are spontaneous DeltaG a negative DeltaG means it's spontaneous |
