F325 3

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Author:
JustinL
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262763
Filename:
F325 3
Updated:
2014-02-19 08:20:00
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Chemistry
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F325 OCR A
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  1. What are the units of rate?
    mol dm-3s-1
  2. Simplified Kc expression:
  3. Define dynamic equilibrium:
    A closed system in which the rate of the forward reaction is equal to the rate of the reverse reaction.
  4. How does temperature affect Kc in a reaction where the forward reaction is endothermic?
    • Kc increases as the temperature increases if the forward reaction is endothermic. 
    • Equilibrium shifts to the right. 
  5. How does temperature affect Kc in a reaction where the forward reaction is exothermic?
    • Kc decreases as the temperature rises if the forward reaction is exothermic.
    • Equilibrium shifts to the left. 
  6. What is the acid dissociation constant?
    • pKa=-log10Ka
    • Ka= 10-pKa
  7. What is a pair of two species that transform into each other by the gain or loss of a proton?
    Acid-base pair
  8. Define an Alkali:
    A type of base that dissolves in water to form hydroxide ions, OH-(aq) ions. 
  9. Define a Complex ion.
    A transition metal ion bonded to one or more ligands by coordinate bonds.
  10. Define a Conjugate acid.
    A species formed when a proton is added to a base.
  11. Define a conjugate base.
    A species formed when a proton is added to a an acid.
  12. Define a coordinate bond.
    A shared pair of electrons in which the bonded pair has been provided by one of the bonding atoms only; also called a dative covalent bond. 
  13. What is standard enthalpy change of atomisation?
    The enthalpy change that takes place when one mole of gaseous atoms forms from the element in its standard state.
  14. What is the standard enthalpy change of combustion?
    The enthalpy change that takes place when one mole of a substance reacts completely with oxygen under standard conditions, all reactants and products under their standard states.
  15. Standard enthalpy change of formation?
    The enthalpy change that takes place when one mole of a compound is formed from its constituent elements in their standard states under standard conditions.
  16. How do acids react with metals?
    • Aqueous acids react with metals to form a salt and Heg.
    • 2HCl(aq) + Mg(s) → MgCl2(aq) + H2(g)
    • 2H+(aq) +Mg(s) → Mg2+(aq) + H2 (g)
  17. How do acids react with Carbonates?
    • Aqueous acids react with carbonates to form a salt, CO2 and H2O eg.
    • 2HCl(aq) + CaCO3 (s) → CaCl2(aq) + CO2(g) H2O(l)
    • 2H+(aq) + CaCO3(s) → Ca2+(aq) + CO2(g) + H2O(l)


  18. How do acids react with bases?
    • Aqueous acids react with bases forming a slat and water, eg.
    • 2HNO3(aq) + 2KOH(aq) → K2SO4(aq) + H2O(l) 

    2H+(aq) + MgO(s) → Mg2+(aq) + H2O(l)
  19. How do acids react with alkalis?
    • Aqueous acids react with alkalis to form a salt and water, eg.
    • H2SO4(aq) + 2KOH(aq) → K2SO4(aq) + 2H2O(l) 

    • H+ + OH- (aq) → H2O(l)

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