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36 Cards in this Set
- Front
- Back
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nitrogen oxide
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NO
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nitrogen oxide is a pollutant that contributes to . . .
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the formation of ozone and smog at the lower levels of the atmosphere
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how is nitrogen oxide formed (give me that motherlovin equation)
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n2(g) + o2(g)<=>2NO(g)
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the equilibrium constant is
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a measure of the extent to which a reaction proceeds or how much product is formed
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equilibrium constant is symbolized by
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K_eq
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the amount of nitrous oxide that forms depends on
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starting concentrations of reactants
equilibrium constant associated w/ reaction |
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at low temps,
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the relative amount of NO formed is negligible because Keq is very small
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equilibrium constant for formation of nitrous oxide increases significantly within
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the internal combustion engine of a car
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what's Keq at 25*C?
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~10^-15
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what's Keq inside a car engine, at temps of >1000*C
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~10^-6 to 10^-1
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nitrogen and oxygen react to a much greater extent at
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high temps
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an arrow pointing to the right in a chemical reaction indicates that
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all of the reactant A molecules will be converted into product B molecules, and reaction will go to completion
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chemical equilibrium
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the state where the concentrations of products and reactants are no longer changing
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equilibrium is denoted by
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that forward reverse arrow thing
<=> |
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reactant-favored equilibrium
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more A exists than B
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product-favored equilibrium
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more B exists than A
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the easiest way to communicate the position of the equilibrium is with an
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equilibrium constant
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an equilibrium constant is defined as
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the ratio of products to reactants at equilibrium
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Keq=
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[B]eq/[A]eq
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large equilibrium constants are indicative of
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product-favored reactions
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small equilibrium constants are indicative of
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reactant-favored reactions
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the equilibrium constant can be thought of as a measure of
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the extent to which a reaction proceeds
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rate_fwd=
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k_(A->B) [A]eq
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rate_rev =
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k_(B->A) [B]eq
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equilibrium is reached when (equation)
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k_(A->B)[A]eq = k_(B->A)[B]eq
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ratio of the rate constants can be expressed as
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k_(A->B)/k_(B->A) = [B]eq/[A]eq
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the equilibrium constant can be calculated as . . .
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Keq=k_(a->b)/k_(b->a)
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the rate constants for the forward and the reverse reactions are . . .
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temperature dependent
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equilibrium constants vary with
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temperature
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the extent to which a reaction occurs is independent of
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time required to reach equilibrium
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what are we using to represent chemical molecules
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dice
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each reactino will begin with all dice representing
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reactant molecules
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each experiment finishes when
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the system reaches equilibrium
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materials
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1 plastic bag with 20 dice
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how many rolls are we doing for each experiment
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20
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how many experiments are we doing
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8
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