CHEM 111 EXAM 2

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  1. Hydrate is
    Ionic Compound associated with water.
  2. What is an Ionic Compound composed of?
    Metal & Non-Metal
  3. What is Avagadros number? whats the conversion factor?
    • 6.022 x 1023
    • 1 mole/6.022 x 1023
  4. What does Formula mass =
    Molar mass (Molecular weight)
  5. Percent Composition:
    Formlua:
    • % by mass of each element in a compound
    • % comp.= (n x MM of element)/MM of compound
    • n=# moles of element in 1 mole of compound
  6. When determining Empirical Formula what must always be assumed?
    100 g of sample
  7. Stoichiometry:
    What's used ot relate different equations to one another?
    • quantitative study of the reactants & products in a chem equation.
    • Mole Method
  8. All Alkali metals react with water to form what?
    H2 gas and an alkali metal Hydroxide
  9. When determining a limiting reagent what must you have?
    balanced equation
  10. Theoretical Yield:
    What will one never get?
    • most product that can be produced from a given amt of reactants.
    • 100%
  11. formula for % Yield=
    what does this measure
    • (actual/ theoretical)x 100
    • measures efficency of a rxn
  12. Solution= ?
    ?= is being dissolved
    ?= doing the dissolving
    • solute+solvent
    • solute
    • solvent
  13. PPM= ?
    ?/?
    • Parts Per Million
    • mg solute/kg solvent
  14. Molarity=?
    mols solute/L solution
  15. Stock Solution's:
    Dilution Equation:
    • concentreated soultion's used to make diluted solution
    • M1V1=M2V2
  16. ? is proton donor while ? it proton acceptor.
    acid, base
  17. Acids react with ? to form?
    metals to form H2
  18. 3 Types of Acids:
    Monoaprotic, Diprotic, Triprotic
  19. Acid base titration:
    uSE KNOWN CONC OF ACID/BASE TO REACT W/ ACID/BASE TO FIND UNKNOWN
  20. Types of rxn:
    • Redox:transfer of electrons
    • Combustion: 2H2+ O2-> 2H2O
    • Decomposition: 2H2O->
  21. Temp measures?
    Flow of heat
  22. Energy Units
    KE=
    1 J=
    1 cal=
    1Calorie=
    • KE= (1/2)mv2
    • 1J= kg x m2/s2
    • 1 cal= 4.184 J
    • 1 Calorie=1000 cal=1kcal
  23. 2 Laws of Thermodynamics
    • energy is neither created or destroyed
    • Internal Energy= KE + PE
  24. Internal Energy
    • EI=KE+PE
    • Ei= Ef-Ei
  25. Heat:
    transfer of thermal energy, always flows from high to low
  26. ?=q+w
    Change E= heat + work
  27. Exothermic vs Endothermic
    Lose heat vs Gain heat
  28. q= ?
    mxdeltaTxCs

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Author:
tbby5065
ID:
71553
Filename:
CHEM 111 EXAM 2
Updated:
2011-03-08 13:38:52
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CHEM EXAM
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CHEM 111 EXAM 2
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