15.5-15.7 Quiz

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21 Terms

1
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What equation do you use to calculate the equilibrium constant?

Keq or Kc = ([C]c[D]d) / ([A]a[B]b) or KP = (PCc * PDd) / (PAa * PBb)

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How do you calculate Q?

= ([C]c[D]d) / ([A]a[B]b) or = (PCc * PDd) / (PAa * PBb); it is the reaction quotient; current/given concentrations NOT equilibrium concentrations

3
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K = Q

at equilibrium; rates of forward and reverse reactions are equal and the concentrations remain constant over time

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Q > K

reverse reaction must occur to reach equilibrium (produce reactants); products are consumed, reactants are formed, numerator in Keq decreases and Q decreases until it equals K; favor reactants as system shifts left

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Q < K

forward reaction must occur to reach equilibrium (produce products); favor products as system shifts right

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Le Châtelier’s Principle

if a system at equilibrium is disturbed, the system will move in such a way as to counteract the disturbance; tries to reestablish equilibrium

7
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Add concentration at equilibrium

equilibrium shifts away from increase; system reacts to consume more of substance it will shift away from the side that just gained more reactant or product to decrease that concentration; ex: If reactant is added, the forward reaction will be favored to decrease reactants and increase product concentration until a new equilibrium is reached.

8
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Removing concentration at equilibrium

equilibrium shifts toward decrease; system reacts to produce more of substance; it will shift toward the side where the reactant or product was just removed to increase that product; ex: If a reactant is removed, the reverse reaction will be favored to increase reactant concentration and decrease product concentration.

9
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Decrease Volume at equilibrium

will increase pressure; equilibrium shifts in direction with fewer moles of gas; remove gases and decrease pressure; IF EQUAL MOLES OF GAS, no effect

10
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Increase Volume at Equilibrium

will decrease pressure; equilibrium shifts in direction with more moles of gas; add gases and increase pressure; IF EQUAL MOLES OF GAS, no effect

11
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Increase Pressure at equilibrium

shifts in direction with fewer moles

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Decrease pressure at equilibrium

shifts in direction with more moles of gas

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ΔH > 0 meaning

endothermic; heat is a reactant; forward direction is favorable; adding heat favors away from increase

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ΔH < 0 meaning

exothermic; heat is a product; reverse reaction is favorable

15
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increasing temperature in endothermic reaction

reaction shifts right (toward products)

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decreasing temperature in endothermic reaction

reaction shifts left (toward reactants)

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increasing temperature in exothermic reaction

reaction shifts left toward reactants

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decreasing temperature in exothermic reaction

reaction shifts right toward products

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With temperature, the equilibrium shifts in the direction that consumes the _______

excess reagent; heat

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Effect of a catalyst on an equilibrium

no effect; will only speed up the reaction rate

21
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What will happen if insert substances are added?

does not affect the equilibrium