How far?

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Define mole fraction.
A measure of how much of a given substance is present in a reaction mixture.
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What is the equation to calculate mole fraction?
Mole fraction, Xa= no. mol of A/total no. mol of all substance
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Define partial pressure.
The pressure an individual gaseous substance would exert if it occupied a whole reaction vessel on its own.
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What is the equation to calculate partial pressure?
Partial pressure, Pa= mole fraction of A x total pressure, P (includes gaseous species only)
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What titles would you use in a calculating equilibrium quantities table?
Component, initial amount of moles, change in moles and amount of moles at equilibrium.
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How can you determine quantities and equilibrium?
Titrations - using a known concentration of one substance to calculate how much reactant/product is present. Colorimetry - monitor concentration of reactant/product as coloured substance alter amount light that can pass through them.
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What is the equation for Kc?
Kc=[C]^c[D]^d/[A]^a[B]^b (moldm^-3 dependent on reaction)
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What's the difference between calculating Kc for homogenous and heterogenous reaction?
In homogeneous reactions, Kc includes concentration of all species. In heterogenous reactions, Kc includes gaseous or aqueous species only because solids and liquids are effectively constant.
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What is the equation for Kp?
Kp=(p(C)^c x p(D)^d)/ (p(A)^a x p(B)^b) (KPa/ATM dependant on reaction)
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What's the difference between calculating Kp for homogenous reactions and heterogenous reactions?
In homogenous reactions, Kp includes p(X) of all species. In heterogenous reactions, Kc includes p(X) of gaseous species only.
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What does the magnitude of K indicate?
The extent of the reaction. K>1 - equilibrium favours the products, K=1 -equilibrium is mid way, K
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What is the effect of temperature increase on K?
If the forward reaction is endothermic, K increases so product yield increase. If reaction is exothermic, K decreases so product yield decreases.
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What is the effect of increasing concentration of reactants or products on K?
No effect on K, however equilibrium will shift to opposite side to increase that concentration.
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What is the effect of increasing pressure on K?
No effect on K, however equilibrium will shift to side with fewer gaseous moles.
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What is the effect of a catalyst on K?
No effect on K or equilibrium position, however equilibrium will be reached sooner.
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Other cards in this set

Card 2

Front

What is the equation to calculate mole fraction?

Back

Mole fraction, Xa= no. mol of A/total no. mol of all substance

Card 3

Front

Define partial pressure.

Back

Preview of the front of card 3

Card 4

Front

What is the equation to calculate partial pressure?

Back

Preview of the front of card 4

Card 5

Front

What titles would you use in a calculating equilibrium quantities table?

Back

Preview of the front of card 5
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